module three chem 101 problems
How many moles of precipitate will be formed when 60.0 mL of 0.250 M AgNO₃ is reacted with excess CaBr₂ in the following chemical reaction? 2 AgNO₃(aq) + CaBr₂(aq) → 2 AgBr(s) + Ca(NO₃)₂(aq)
0.0150 mol
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00483 mol of Ca(OH)₂ were present, what was the concentration of the initial Ca(OH)₂ solution?
0.097 mol
Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle's Law is described as P₁V₁ = P₂V₂. Assume the initial volume is 4.0 L at 0.050 atm and the final volume is 2.00 L. Calculate the final pressure in the container in atm.
0.1 atm
What is the oxidation number of each oxygen atom in HOOH?
-1
The oxidation number of oxygen in O²⁻ is
-2
How many moles of K₂S will be required to completely react with 50.0 mL of 0.200 M FeCl₃? 3 K₂S(aq) + 2 FeCl₃(aq) → Fe₂S₃(s) + 6 KCl(aq)
0.0150 mol
An evil mastermind is attempting to take over the world, but he needs your patent for a new power source. He has trapped you in a room and a lethal nerve gas, sarin, is effusing into the room. You must figure out a way to escape in time. Sarin is a toxic nerve gas. What is the molecular weight of sarin gas (shown below)? Submit your answer to two decimal places.
140.11 g/mol
What volume in liters would 20.0 moles of sulfur dioxide occupy at 75.3 °C with a pressure of 3.00 atm?
190 L
Write a balanced chemical equation based on the following description: solid chromium reacts with solid iodine to form solid chromium(III) iodide
2 Cr(s) + 3 I₂(s) → 2 CrI₃(s)
Consider the chemical reaction that takes place between solid copper and oxygen gas. Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow 2 Cu(s) + O₂(g) →
2 Cu(s) + O₂(g) → 2 CuO(s)
Container A contains 1 mole of Xe gas and Container B contains 1 mole of He gas. Both gases are at 100 °C. If both gases behave ideally, then what would be the average kinetic energy for 1 mol of either gas, in joules?
4650 J
What is the mass (in grams) of 5.00 L of O₂ at STP?
7.14 g
Which of the following gas samples would have the largest volume, measured at 25 °C and one atmosphere pressure? A) 4 g of methane B) 5 g of nitrogen C) 6 g of oxygen D) 7 g of carbon dioxide E) 8 g of chlorine
A) 4 g of methane
Which of the following aqueous solutions would NOT form a precipitate when added to a solution of silver nitrate? A) NaF B) NaCl C) NaBr D) NaI
A) NaF
Which one of the following would form a precipitate when mixed with aqueous Ba(NO₃)₂? A) Na₂SO₄ B) KCl C) LiC₂H₃O₂ D) CsOH E) None of these would form a precipitate.
A) Na₂SO₄
For a constant temperature, which will have the greatest average speed? A) Ne B) Ar C) Kr D) They'll all have equal speeds
A) Ne
What is represented by A on the phase diagram? (image four) A) solid B) liquid C) gas D) cannot determine without exact pressure and temperature
A) solid
Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow AgNO₃(s) →
AgNO₃(s) → Ag⁺(aq) + NO₃⁻(aq)
What is Standard Temperature and Pressure (STP)? A) 298.15 K and 1.00 atm B) 273.15 K and 1.00 atm C) 273.15 K and 0.00 atm
B) 273.15 K and 1.00 atm
Combusting an unknown hydrocarbon produces 5 mol CO₂ and 6 mol H₂O. What is the empirical formula of the hydrocarbon? A) C₅H₆ B) C₅H₁₂ C) C₆H₅ D) CH E) Not enough information to solve the problem.
B) C₅H₁₂
Which best explains why the meniscus of mercury in a glass tube is convex? A) The greater attraction of mercury to the glass than to itself. B) The lower attraction of mercury to the glass than to itself. C) The low surface tension of mercury. D) The high density of mercury compared to water. E) The repulsion between mercury and the glass.
B) The lower attraction of mercury to the glass than to itself.
Which one of the following gases would be expected to have the highest speed? A) O₂ at 1000 K B) O₃ at 500K C) H₂ at 1000 K D) H₂ at 500 K
C) H₂ at 1000 K
Which of the following substances would not exhibit any hydrogen bonding interactions in a pure substance? A) H₂O B) HF C) N(CH₃)₃ D) CH₃CH₂OH E) CH₃NH₂
C) N(CH₃)₃
Ammonia and hydrogen fluoride both have unusually high boiling points due to _____ A) dispersion forces. B) dipole-dipole interactions. C) hydrogen bonding. D) ion-dipole interactions. E) low molar masses.
C) hydrogen bonding.
Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle observed the change in pressure and volume relationship in a gas. The pressure of a gas in a closed container is __________ to the volume of the gas in the container (assuming constant temperature). A) proportional B) exponentially larger C) inversely proportional D) exponentially smaller E) has no relation
C) inversely proportional
In a molecule of HI, what intermolecular forces are present? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding
D) dispersion and dipole-dipole
There are two compounds which have the chemical formula C₄H₁₀. What are intermolecular forces are present in Compound A? (image one) A) dispersion forces, dipole-dipole interactions and hydrogen bonding B) dispersion forces and hydrogen bonding C) dispersion forces and dipole-dipole interactions D) dispersion forces only
D) dispersion forces only
Which of the following liquid substances has the highest vapor pressure at its normal boiling point? A) CH₃OH (b.p. = 65°C) B) C₆H₆ (b.p. = 80°C) C) C₂H₅OH (b.p. = 65°C) D) H₂O (b.p. = 100°C) E) All would have same vapor pressure at their boiling points.
E) All would have same vapor pressure at their boiling points.
Which of the following straight-chain hydrocarbons will have the highest viscosity at 298 K? A) C₅H₁₂ B) C₆H₁₄ C) C₇H₁₆ D) C₈H₁₈ E) C₉H₂₀
E) C₉H₂₀
Which is expected to have the highest heat of vaporization? A) CH₄ B) SiH₄ C) NH₃ D) PH₃ E) H₂O
E) H₂O
Write the balanced NET ionic equation for the reaction when AgC₂H₃O₂ and Ni(ClO₄)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR.
NR
The oxidation number of aluminum in Al³⁺ is
3
The oxidation number of the chlorine atom in ClF₃ is
3
Write the balanced COMPLETE ionic equation for the reaction when Cs₃PO₄ and AgNO₃ are mixed in aqueous solution. If no reaction occurs, simply write only NR.
3 Cs⁺(aq) + PO₄³⁻(aq) + 3 Ag⁺(aq) + 3 NO₃⁻(aq) → Ag₃PO₄(s) + 3 Cs⁺(aq) + 3 NO₃⁻(aq)
A sample of 1.00 mol of gas in a 8.00 L container is at 45.0 °C. What is the pressure (in bar) of the gas? R = 0.08314 L･bar/mol･K.
3.3 bar
Methanol can be formed by the following UNBALANCED equation below. What is the mass in grams of methanol that can be formed from 101 molecules of CO? H₂(g) + CO(g) → CH₃OH(l).
5.37 × 10⁻²¹ g
A gas has a density of 1.57 g/L at 40.0 °C and 2.00 atm of pressure. What is the identity of the gas? A) He B) Ne C) Ar D) Kr
B) Ne
Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles converted his observation into a mathematical formula. Which equation best represents the relationship between the temperature (T) and the volume (V) of the gas before and after heat is added? A) T₁V₁ = T₂V₂ B) V₁ / T₁ = V₂ / T₂ C) P₁T₁ = P₂T₂ D) PV = nRT E) V = T₁ / T₂
B) V₁ / T₁ = V₂ / T₂
Which of the following substances would have the highest vapor pressure at 298 K? A) propanol (b.p. = 97°C) B) acetone (b.p. = 56°C) C) water (b.p. = 100°C) D) benzene (b.p. = 80°C) E) chloroform (b.p. = 61°C)
B) acetone (b.p. = 56°C)
What is represented by B on the phase diagram? (image four) A) solid B) liquid C) gas D) cannot determine without exact pressure and temperature
B) liquid
How does the root mean square velocity of an ideal gas vary as the molar mass of the gas increases? A) u(rms) increases as the mass of the gas increases B) u(rms) decreases as the mass of the gas increases C) u(rms) is not dependent upon the molar mass of the gas
B) u(rms) decreases as the mass of the gas increases
Write the balanced NET ionic equation for the reaction when aqueous BaCl₂ and aqueous (NH₄)₂SO₄ are mixed in solution to form aqueous NH₄Cl and solid BaSO₄.
Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)
Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a gas provided in the questions below. Which combination of lines would be equivalent to the enthalpy of sublimation for this substance? (image seven) A) A + B B) B + C C) B + D D) C + D E) D + E
C) B + D
Consider the phase diagram for an unknown substance provided in the questions below. Which point in the phase diagram represents the liquid phase? (image six) A) A B) B C) C D) D E) E
C) C
Which property typically indicates strong intermolecular forces are present in a liquid? A) low heat of vaporization B) low critical temperature C) low vapor pressure D) low boiling point E) low melting point
C) low vapor pressure
Calculate the root mean square velocity, in m/s, of He at -23.0°C. Assume ideal gas behavior.
1.25 × 10³ m/s
Which one of the following correctly ranks the compounds in order of lowest vapor pressure to highest vapor pressure based only in intermolecular forces? A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃ B) CH₃OCH₃ < CH₃CH₂CH₃ < CH₃CH₂OH C) CH₃CH₂CH₃ < CH₃CH₂OH < CH₃OCH₃ D) CH₃CH₂CH₃ < CH₃OCH₃ < CH₃CH₂OH
A) CH₃CH₂OH < CH₃OCH₃ < CH₃CH₂CH₃
Which one of the following would have the largest dispersion forces? A) CH₃CH₂SH B) CH₃NH₂ C) CH₄ D) CH₃CH₃
A) CH₃CH₂SH
Which one of the following would have the highest heat of vaporization? A) CH₃OH B) CH₂F₂ C) NF₃ D) CHF₃
A) CH₃OH
At the same temperature, which of the following gases will have the fastest rate of effusion? A) CO B) SF₆ C) Cl₂ D) HBr
A) CO
Consider the chemical reaction that takes place between solid copper and oxygen gas. In the reaction, identify which element in what species is oxidized? A) O in CuO B) O₂ C) Cu in CuO D) Cu(s)
D) Cu(s)
Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a gas provided in the questions below. The heat added for which line would represent the enthalpy of vaporization for this substance? (image seven) A) A B) B C) C D) D E) E
D) D
Consider the phase diagram for an unknown substance provided in the questions below. Which point on the phase diagram is in the gas phase? (image five) A) A B) F C) C D) D E) E
D) D
Consider the phase diagram for an unknown substance provided in the questions below. Which point in the phase diagram represents the triple point? (image six) A) A B) B C) C D) D E) E
E) E
Which is expected to have the lowest vapor pressure? A) CH₄ B) SiH₄ C) NH₃ D) PH₃ E) H₂O
E) H₂O
Which of the following phase changes represents sublimation? A) gas ⟶ liquid B) liquid ⟶ gas C) liquid ⟶ solid D) solid ⟶ liquid E) solid ⟶ gas
E) solid ⟶ gas
Under what conditions are gases most likely to behave ideally? A) High pressures B) Low temperatures C) Polar molecules D) Low pressures E) Large molecules
D) Low pressures
Which of the following has the lowest boiling point? A) C₅H₁₂ B) C₇H₁₆ C) C₉H₂₀ D) C₁₁H₂₄ E) C₁₃H₂₈
A) C₅H₁₂
Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a gas provided in the questions below. Which line on the heating curve represents heating the solid phase? (image seven) A) A B) B C) C D) D E) E
A) A
In a 4.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.20 atm, how many moles of steam are in the cooker?
0.4 mol
How many moles of lithium hydroxide would be required to produce 38.5 g of Li₂CO₃ in the following chemical reaction? 2 LiOH(s) + CO₂(g) → Li₂CO₃(s) + H₂O(l)
1.04 mol
A balloon is filled to a volume of 1.50 L with 3.00 moles of gas at 25 °C. With pressure and temperature held constant, what will be the volume (in L) of the balloon if 0.20 moles of gas are added?
1.6 L
Gaseous molecules can quickly spread throughout a room. Recall you calculated that this gas has a mass of 37.345 g/mol. Calculate the density, in g/L, of this gas at STP, if 1.00 L of this gas effuses through an apparatus in 6.6 min.
1.67 g/L
Gaseous molecules can quickly spread throughout a room. Graham's Law states that rate of effusion A/rate of effusion of B = (square root of Mass of B)/(square root of Mass of A). Calculate how fast Cl₂ gas effuses compared to I₂ gas. Assume the temperature remains constant.
1.89
An evil mastermind is attempting to take over the world, but he needs your patent for a new power source. He has trapped you in a room and a lethal nerve gas, sarin, is effusing into the room. You must figure out a way to escape in time. 1.00 mmol of nitrogen gas takes 60.89 min to effuse through a small hole. Based on your calculation, sarin gas effuses 2.24 times slower than nitrogen gas. Assuming that sarin will behave as an ideal gas at STP, how many minutes do you have to escape the room before 1.0 mmol of sarin has effused into the room?
136 min
The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. Compare the value of 16.079 to the answer you obtain when you assume that CO is an ideal gas. Use the ideal gas law to determine the pressure, in atmospheres, of 2.0 moles of CO gas in a 3.00 L flask at 25.0°C.
16.3 atm
Write a balanced chemical equation based on the following description: aqueous potassium phosphate reacts with aqueous nickel(II) bromide to produce solid nickel(II) phosphate and aqueous potassium bromide.
2 K₃PO₄(aq) + 3 NiBr₂(aq) → Ni₃(PO₄)₂(s) + 6 KBr(aq)
An evil mastermind is attempting to take over the world, but he needs your patent for a new power source. He has trapped you in a room and a lethal nerve gas, sarin, is effusing into the room. You must figure out a way to escape in time. Air is mostly nitrogen, with a molecular mass of 28 g/mol. Sarin has molecular mass of 140.11 g/mol. Using Graham's Law of effusion, determine the rate of nitrogen effusion into the room compared to the rate of sarin gas effusion.
2.24
What volume (in mL) of 0.200 M HCl would be required to completely react with 4.40 g of Al in the following chemical reaction? 2 Al(s) + 6 HCl(aq) → 2 AlCl₃ (aq) + 3 H₂(g)
2.45 × 10³ mL
The oxidation number of C in C₂O₄²⁻ is
3
What is the mass in grams of CO₂ that can be produced from the combustion of 2.76 moles of butane according to this equation: 2 C₄H₁₀(g) + 13 O₂(g) → 8 CO₂(g) + 10 H₂O(g)
486 g
What is the volume in liters of hydrogen gas that would be produced by the reaction of 40.0 g of Al with excess HCl at STP according to the following reaction? 2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)
49.8 L
Container A contains 1 mole of Xe gas and Container B contains 1 mole of He gas. Both gases are at 100 °C. How much faster will the He diffuse than Xe?
5.73
Which one of the following would have the lowest magnitude for the heat of fusion? A) CH₃OH B) NH₃ C) CH₄ D) CHF₃
C) CH₄
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Write the balanced chemical equation for the reaction
Ca(OH)₂(aq) + 2 HNO₃(aq) → 2 H₂O(l) + Ca(NO₃)₂(aq)
Consider the phase diagram for an unknown substance provided in the questions below. Which point on the phase diagram indicates the phase boundary where sublimation takes place? (image six) A) A B) C C) D D) F
D) F
Which of the following reactions is a precipitation reaction? A) HNO₂(aq) + NaOH(aq) → NaNO₂(aq) + H₂O(l) B) 2C₂H₅OH(l) + 7O₂(g) → 4CO₂(g) + 6H₂O(l) C) 2H₂O₂(l) → 2H₂O(l) + O₂(g) D) FeSO₄(aq) + K₂S(aq) → FeS(s) + K₂SO₄(aq)
D) FeSO₄(aq) + K₂S(aq) → FeS(s) + K₂SO₄(aq)
Which of the following halogens would have the highest melting point? A) F₂ B) Cl₂ C) Br₂ D) I₂
D) I₂
Identify the type or types of intermolecular forces present between molecules of the compound pictured below: (image three) A) dispersion only B) dipole-dipole C) hydrogen bonding D) dispersion and dipole-dipole only E) dispersion, dipole-dipole, and hydrogen bonding
E) dispersion, dipole-dipole, and hydrogen bonding
Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. HI(aq) →
HI(aq) → H⁺(aq) + I⁻(aq)
Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow Pb(NO₃)₂(aq) + 2 KI(aq) →
Pb(NO₃)₂(aq) + 2 KI(aq) → PbI₂(s) + 2 KNO₃(aq)
COF₂ is a highly toxic compound that was used as a chemical weapon in World War I. Is the molecule COF₂ polar? A) Yes B) No
A) Yes
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. How many moles of HNO₃ are used in the titration?
0.0096 mol
How many moles of precipitate will be formed when 20.0 mL of 0.550 M AgNO₃ is reacted with excess MgBr₂ in the following chemical reaction? 2 AgNO₃(aq) + MgBr₂(aq) → 2 AgBr(s) + Mg(NO₃)₂(aq)
0.0110 mol
15.0 L of an ideal gas at 298 K and 3.36 atm are heated to 383 K with a new pressure of 6.00 atm. What is the new volume in liters?
10.8 L
How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 12.0 L?
12.39 mol
What volume (in mL) of 0.2600 M HBr is required to neutralize 40.00 mL of 0.8000 M NaOH?
123.1 mL
What would be the density (in g/L) of a sample of N₂ gas at 70.0 °C and 2.50 atm of pressure?
2.5 g/L
There are two compounds which have the chemical formula C₄H₁₀. Which of the compounds will have the lowest boiling point? (image one) A) Compound A B) Compound B C) Neither, since they have the same molar mass and will have the same dispersion forces.
A) Compound A
Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a gas provided in the questions below. For which line on the heating curve would both solid and liquid be present? (image seven) A) A B) B C) C D) D E) E
B) B
What is the oxidizing agent in the reaction Zn + 2 H⁺ → Zn²⁺ + H₂? A) Zn B) H⁺ C) Zn²⁺ D) H₂ E) This is not a redox reaction.
B) H⁺
What phase change is represented by the transition from A to C? (image four) A) fusion B) sublimation C) vaporization D) condensation E) solidification
B) sublimation
Which of the following phases does a sample of water exist in at its triple point? A) gas B) liquid C) solid D) all of these E) none of these
D) all of these
In the van der Waals equation, for what aspect does the factor 'b' correct in from ideal gases? A) It accounts for the isotopic distribution of atoms in the gas. B) It corrects for inelastic collisions between molecules. C) It corrects for the distribution of speeds of gas molecules at the given temperature. D) It corrects for the possible polarity of the molecule. E) It corrects for the volume of the gas particle.
E) It corrects for the volume of the gas particle.
What temperature (in °C) did an ideal gas shift to if it was initially at -20.0 °C at 4.33 bar and 35.0 L and the pressure was changed to 8.71 bar and the volume changed to 15.0 L?
-54.91 degrees celsius
A 50.0 mL solution of Ca(OH)₂ with an unknown concentration was titrated with 0.340 M HNO₃. To reach the endpoint, a total of 28.4 mL of HNO₃ was required. Given that 0.00966 mol of HNO₃ are used in the titration, how many moles of Ca(OH)₂ had to be present in the initial reaction?
0.00483 mol
When the ideas from Boyle's Law, Charles' Law and Gay-Lussac's Law are combined, you get the combined gas law. This law combines the effects of pressure, temperature and volume changes on a gas. Remember the combined gas law is P₁V₁/T₁ = P₂V₂/T₂ Imagine an ideal gas in a cylinder with a piston, starting at a pressure of 1 atm and a volume of 10 L at 298 K. This system is cooled to 273 K and compressed to 5.0 L. What is the final pressure in the cylinder?
1.8 atm
A chemist conducts an experiment in which 2.0 L of hydrogen gas is collected over water at 1 atm and 298 K. Remember the pressure due to the hydrogen gas is 0.97 atm. Using the combined gas law, calculate the volume in L of the dry hydrogen gas at 273 K and a pressure of 1 atm.
1.83 L
At STP, 5.00 mol of gas occupies approximately what volume in liters?
112 L
The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. For CO, a = 1.505 L²atm/mol² and b = 0.03985 L/mol. Use the van der Waals equation to determine the pressure, in atmospheres, of 2.0 moles of CO gas in a 3.00 L flask at 25.0°C. Remember the gas constant, R, is 0.08206 L･atm/mol･K.
16.079 atm
Gay-Lussac's Law explores the relationship between temperature and pressure of an ideal gas. Gay-Lussac's Law is described as P₁/T₁ = P₂/T₂. Assume the initial pressure is 15.0 atm at 275 K and the final temperature is 375 K. Calculate the final pressure of the gas in the container in atm.
20.5 atm
A 30.0 g sample of O₂ at standard temperature and pressure (STP) would occupy what volume in litres?
21 L
Solid sodium reacts with liquid water to form hydrogen gas according to the equation 2 Na(s) + 2 H₂O(l) → 2 NaOH(aq) + H₂(g) What is the pressure (in atm) of hydrogen gas in the 20.0 L headspace of a reactor vessel when 1.00 kg sodium is reacted with excess water at 50.0°C?
28.82 atm
Complete the balanced neutralization equation for the reaction below 3 NH₄OH(aq) + H₃PO₄(aq) →
3 NH₄OH(aq) + H₃PO₄(aq) → (NH₄)₃PO₄(aq) + 3 H₂O(l)
An evil mastermind is attempting to take over the world, but he needs your patent for a new power source. He has trapped you in a room and a lethal nerve gas, sarin, is effusing into the room. You must figure out a way to escape in time. Nitrogen gas effuses 2.24 times faster than sarin gas. Nitrogen gas effuses at the rate of 79.0 mL/s. Assuming the same temperature and pressure, at what rate will sarin effuse in mL/s?
35.3 mL/s
Gaseous molecules can quickly spread throughout a room. Graham's Law states that rate of effusion A/rate of effusion of B = (square root of Mass of B)/(square root of Mass of A). Calculate the mass of the diatomic gas that effuses 2.5845 times faster than I₂ gas. Assume the temperature and pressure remain constant.
37.998 g/mol
When solid calcium carbonate is reacted with aqueous hydrochloric acid, the products of the reaction include aqueous calcium chloride, liquid water, and gaseous carbon dioxide. Calculate the volume of CO₂ gas (in L) collected over water at 25.0 °C when 25.1 g of calcium carbonate is added to excess hydrochloric acid if the total pressure is 911 mm Hg. The vapor pressure of water at 25.0 °C is 23.8 mm Hg.
5.25 L
Charles' Law explores the effects of temperature on the volume of an ideal gas. Charles' Law is described as V₁/T₁ = V₂/T₂. A gas with an initial volume of 2.0 L at 275 K is heated. The final volume is 4.0 L. Calculate the final temperature of the gas, in K.
550 K
What would be the pressure (in atm) of a 5.00 mol sample of Cl₂ at 400.0 K in a 2.00 L container found using the van der Waals equation? For Cl₂, a = 6.49 L²･atm/mol² and b = 0.0652 L/mol.
57.5 atm
Calculate the root-mean-square velocity, in m/s, for a neon atom at 15.3 °C. The universal gas constant, R=8.314 J/mol･K
597 m/s
How many moles of NH₃ can be produced from 3.76 moles of nitrogen in the following reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
7.52 mol
An unknown gas effuses at a rate of 2.00 times the rate of Cl₂. What is the molar mass of the unknown gas?
70.6 g/mol
Avogadro's Law explores the relationship between volume and number of moles of an ideal gas. Avogadro's Law is described as V₁/n₁ = V₂/n₂. Assume you have 2.0 moles of a gas with an initial volume of 4.0 L. Another 2.0 moles of gas were added to the container. Calculate the final volume of the gas in the container in L.
8.0 L
Which of the following aldehydes has the highest solubility in water? A) CH₃CH₂C(=O)H B) CH₃CH₂CH₂CH₂C(=O)H C) CH₃(CH₂)₅C(=O)H D) CH₃(CH₂)₁₀C(=O)H E) All of these have equal solubility.
A) CH₃CH₂C(=O)H
Dispersion forces would be weakest in which of the following substances? A) He B) Ne C) Ar D) Kr E) Xe
A) He
Which combination of properties would be expected to lead to the most viscous liquid? A) Strong intermolecular forces, low temperature B) Strong intermolecular forces, high temperature C) Weak intermolecular forces, low temperature D) Weak intermolecular forces, high temperature.
A) Strong intermolecular forces, low temperature
Container A contains 1 mole of Xe gas and Container B contains 1 mole of He gas. Both gases are at 100 °C. Which gas is expected to behave less like an ideal gas? A) The gas in Container A would behave less ideally because the particle size is greater. B) The gas in Container B would behave less ideally because the particles size is smaller. C) Both gases would be equally ideal because they are at the same temperature.
A) The gas in Container A would behave less ideally because the particle size is greater.
Which of the following represents the intermolecular forces present in CO₂? A) dispersion only B) dipole-dipole only C) hydrogen bonding only D) dispersion and dipole-dipole E) dispersion and hydrogen bonding
A) dispersion only
Gaseous molecules can quickly spread throughout a room. The movement of gas molecules can occur through a process called effusion. Choose the best definition for effusion. A) movement of gas molecules from one container to another through a tiny hole B) movement of gas molecules through one or more other types of gas via random molecular motion C) movement of gas molecules from an empty container to a full container D) movement of gas molecules through one or more other types of gas via directed transport
A) movement of gas molecules from one container to another through a tiny hole
Consider the phase diagram for an unknown substance provided in the questions below. What is the name of the transition that takes place from point C to point G? (image six) A) vaporization B) condensation C) fusion D) melting
A) vaporization
Consider the phase diagram for an unknown substance provided in the questions below. Which point on the phase diagram is at the normal boiling point for this substance? (image five) A) A B) B C) C D) F
B) B
There are two compounds which have the chemical formula C₄H₁₀. Which of the compounds will have the lowest vapor pressure? (image one) A) Compound A B) Compound B C) Neither, since they have the same molar mass and will have the same dispersion forces.
B) Compound B
Container A contains 1 mole of Xe gas and Container B contains 1 mole of He gas. Both gases are at 100 °C. In which of the two containers would the gas particles be expected to have a higher average speed? A) Container A B) Container B C) Both gases would have the same speed.
B) Container B
What intermolecular forces are present in CH₃F and CF₄? A) Dispersion forces, dipole-dipole forces, and hydrogen bonding. B) Dispersion forces only. C) Dispersion forces and dipole-dipole forces D) Dipole-dipole forces only.
B) Dispersion forces only.
Consider the phase diagram for an unknown substance provided in the questions below. From between which two points does melting take place? (image five) A) Point F to Point E B) Point E to Point F C) Point E to Point D D) Point D to Point E
B) Point E to Point F
The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. Not all gases behave ideally. An ideal gas is one that... A) follows kinetic molecular theory, occupies a gas particle volume that is negligible relative to the total volume of the container, and exhibits strong intermolecular attractions. B) follows kinetic molecular theory, occupies a gas particle volume that is negligible relative to the total volume of the container, and exhibits no appreciable intermolecular attractions or repulsions. C) follows kinetic molecular theory, occupies a gas particle volume proportional to the total volume of the container, and exhibits no appreciable intermolecular attractions or repulsions. D) follows kinetic molecular theory, occupies a gas particle volume proportional to the total volume of the container, and exhibits strong intermolecular attractions.
B) follows kinetic molecular theory, occupies a gas particle volume that is negligible relative to the total volume of the container, and exhibits no appreciable intermolecular attractions or repulsions.
Gaseous molecules can quickly spread throughout a room. The movement of gas molecules can occur through a process called diffusion. Choose the best definition for diffusion. A) movement of gas molecules from one container to another through a tiny hole B) movement of gas molecules through one or more other types of gas via random molecular motion C) movement of gas molecules from an empty container to a full container D) movement of gas molecules through one or more other types of gas via directed transport
B) movement of gas molecules through one or more other types of gas via random molecular motion
Consider the phase diagram for an unknown substance provided in the questions below. Point G on the phase diagram represents (image five) A) the triple point. B) the critical point. C) the normal boiling point. D) the normal sublimation point.
B) the critical point.
What is represented by point D on the phase diagram? (image four) A) melting point B) triple point C) boiling point D) sublimation point E) freezing point
B) triple point
How much faster does ²³⁵UF₆ effuse than ²³⁸UF₆? A) 1.0086/1 B) 0.9957/1 C) 1.0043/1 D) 0.9914/1 E) 1.0064/1
C) 1.0043/1
Container A contains 1 mole of Xe gas and Container B contains 1 mole of He gas. Both gases are at 100 °C. What can be said about the average kinetic energy in the two containers if both gases are considered to have ideal behavior? A) The gas in Container A would have a higher kinetic energy than the gas in Container B. B) The gas in Container A would have a lower kinetic energy than the gas in container B. C) Both gases would have the same kinetic energy.
C) Both gases would have the same kinetic energy.
Which one of the following correctly ranks the compounds in order of lowest enthalpy of vaporization to highest enthalpy of vaporization based only in intermolecular forces? A) CH₃NH₂ < CH₃SH < CH₃CH₃ B) CH₃NH₂ < CH₃CH₃ < CH₃SH C) CH₃CH₃ < CH₃SH < CH₃NH₂ D) CH₃SH < CH₃NH₂ < CH₃CH₃
C) CH₃CH₃ < CH₃SH < CH₃NH₂
Which compound contains chlorine (Cl) with an oxidation number of +3 A) Cl₂O B) ClO₃ C) Cl₂O₃ D) ClO₂ E) Cl₂O₅
C) Cl₂O₃
Which of the following exhibits dipole-dipole intermolecular forces in a pure substance? A) BF₃ B) CO₂ C) NH₃ D) Br₂ E) CF₄
C) NH₃
COF₂ is a highly toxic compound that was used as a chemical weapon in World War I. What intermolecular forces are present in a molecule of COF₂? A) dispersion forces only B) dispersion forces and hydrogen bonding C) dispersion forces and dipole-dipole interactions D) dispersion forces, dipole-dipole interactions and hydrogen bonding
C) dispersion forces and dipole-dipole interactions
Gaseous molecules can quickly spread throughout a room. Thomas Graham studied the rates of effusion for gases with different molecular masses. He found that the rate of effusion of a gas is _______proportional to the square root of its molar mass. This means that gases with a _________ molecular weight have higher effusion rates. A) directly; lighter B) directly; heavier C) inversely; lighter D) inversely; heavier
C) inversely; lighter
The van der Waals equation compensates for non-ideal behavior of gases by taking into account intermolecular forces and the volume of the gas molecules. In the van der Waals equation, (a) is a constant for intermolecular forces and (b) is a constant for the volume of the gas molecules. The van der Waals equation is shown below. If the values for (a) and (b) are close to zero, then A) the equation results in an artificially increased value for the volume. B) the equation results in an artificially increased value for the pressure. C) the equation simplifies to the ideal gas law, PV = nRT. D) the equation is no longer valid.
C) the equation simplifies to the ideal gas law, PV = nRT.
n the van der Waals equation, the factor 'a' is a correction for A) the distribution of speeds of gas molecules at the given temperature. B) the volume taken up by the gas particles. C) the inelastic collisions that take place between gas particles (intermolecular forces). D) the possibility of a chemical reaction between gas particles.
C) the inelastic collisions that take place between gas particles (intermolecular forces).
Which quantity is not determined from a heating or cooling curve for a substance? A) boiling point B) heat of vaporization C) triple point D) melting point E) heat of fusion
C) triple point
What phase change is represented by the transition from B to C? (image four) A) fusion B) sublimation C) vaporization D) condensation E) solidification
C) vaporization
What intermolecular forces are present in both molecules of CH₃CH₂CH₂F and CH₃CH₂CH₂OH? A) Dispersion forces only. B) Dipole-dipole forces only. C) Dispersion forces, dipole-dipole forces, and hydrogen bonding. D) Dispersion forces and dipole-dipole forces
D) Dispersion forces and dipole-dipole forces
Gaseous molecules can quickly spread throughout a room. Recall you calculated that this gas has a mass of 37.345 g/mol. Determine the identity of the diatomic gas that effuses 2.5845 times faster than I₂ gas. Assume the temperature remains constant. A) O₂ B) N₂ C) Ar D) F₂ E) Br₂
D) F₂
According to the Kinetic Molecular Theory A) The volume of the gas particles will impact the volume available to the gas. B) Gas particles exert pressure by colliding with one another C) The gas particles are moving in circular motions throughout the container. D) The average kinetic energy is proportional to the temperature of the system.
D) The average kinetic energy is proportional to the temperature of the system.
Which of the following properties does NOT impact the vapor pressure of a particular liquid in a closed container? A) Amount of hydrogen bonding in the liquid B) The temperature of the liquid C) The surface tension of the liquid D) The volume of liquid E) The viscosity of the liquid
D) The volume of liquid
There are two compounds which have the chemical formula C₄H₁₀. What are intermolecular forces are present in Compound B? (image one) A) dispersion forces, dipole-dipole interactions and hydrogen bonding B) dispersion forces and hydrogen bonding C) dispersion forces and dipole-dipole interactions D) dispersion forces only
D) dispersion forces only
The intermolecular force between molecules of I₂ is _____ A) ionic bonds. B) dipole-dipole interactions. C) ion-dipole interactions. D) dispersion forces. E) covalent bonds.
D) dispersion forces.
Consider the heating curve for 1.00 mole of an unknown substance as it is heated from a solid to a gas provided in the questions below. Which line on the heating curve represents heating the gas phase? (image seven) A) A B) B C) C D) D E) E
E) E
dentify the type or types of intermolecular forces present between molecules of the compound pictured below: (image two) A) dispersion only B) dipole-dipole C) hydrogen bonding D) dispersion and dipole-dipole only E) dispersion, dipole-dipole, and hydrogen bonding
E) dispersion, dipole-dipole, and hydrogen bonding
Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow HClO₄(aq) →
HClO₄(aq) → H⁺(aq) + ClO₄⁻(aq)
A chamber contains equal molar amounts of He, Ne, Ar, and Kr. If the total chamber pressure is 1 atm, then the partial pressure (in atm) of Kr is:
0.25 atm
A 15.0 mL solution of Sr(OH)₂ is neutralized with 27.5 mL of 0.350 M HCl. What is the concentration of the original Sr(OH)₂ solution?
0.32 M
A glass container was initially charged with 1.50 moles of a gas sample at 3.75 bar and 21.7 °C. Some of the gas was released as the temperature was increased to 28.5 °C, so the final pressure in the container was reduced to 0.998 bar. How many moles of the gas sample are present at the end?
0.390 mol
A chemist conducts an experiment in which 2.0 L of hydrogen gas is collected over water at 1 atm and 298 K. The phrase 'over water" means that the gas was collected by bubbling it into an inverted bottle filled with water, which is sitting in a water bath. The gas is trapped in the bottle, displacing the water into the water bath. However, the gas collected is now saturated with water vapor. The partial pressure of water vapor at 298 K is 0.03 atm. Using Dalton's Law, calculate the pressure of the hydrogen gas in atm.
0.97 atm
Complete the balanced neutralization equation for the reaction below 2 HCl(aq) + Sr(OH)₂(aq) →
2 HCl(aq) + Sr(OH)₂(aq) → SrCl₂(aq) + 2 H₂O(l)
What is the mass in grams of Al that were reacted with excess HCl if 5.20 L of hydrogen gas were collected at STP in the following reaction? 2 Al (s) + 6 HCl (aq) → 2 AlCl₃ (aq) + 3 H₂ (g)
4.2 g
What is the volume (in L) of carbon dioxide at 1.00 atm and 298.15 K are released from a car's engine upon consumption of a 60.0 L LIQUID tank gasoline? (Gasoline density: 0.77 kg/L, Molar mass of C₈H₁₈: 114.2 g/mol) C₈H₁₈ (l) + ²⁵/₂ O₂ (g) → 8 CO₂ (g) + 9 H₂O (g)
7.92 × 10⁴ L
Milk of magnesia, which is an aqueous suspension of magnesium hydroxide, is used as an antacid in the reaction below. How many molecules of HCl would have to be present to form 75.82 g of MgCl₂? Mg(OH)₂(s) + 2 HCl(aq) → 2 H₂O(l) + MgCl₂(aq)
9.591 × 10²³ molecules
Balance the following chemical reaction: Al₂(SO₄)₃ (aq) + K₃PO₄ (aq) → AlPO₄ (s) + K₂SO₄ (aq) A) Al₂(SO₄)₃ (aq) + 2 K₃PO₄ (aq) → 2 AlPO₄ (s) + 3 K₂SO₄ (aq) B) 2 Al₂(SO₄)₃ (aq) + 6 K₃PO₄ (aq) → 3 AlPO₄ (s) + 6 K₂SO₄ (aq) C) 2 Al₂(SO₄)₃ (aq) + 4 K₃PO₄ (aq) → 4 AlPO₄ (s) + 6 K₂SO₄ (aq) D) AlSO₄ (aq) + KPO₄ (aq) → AlPO₄ (s) + KSO₄ (aq)
A) Al₂(SO₄)₃ (aq) + 2 K₃PO₄ (aq) → 2 AlPO₄ (s) + 3 K₂SO₄ (aq)
In the following reaction, which element in what species is oxidized? C₂H₄ (g) + 3 O₂ (g) → 2 CO₂ (g) + 2 H₂O (g) A) C in C₂H₄ B) H in C₂H₄ C) O in O₂ D) This is not an oxidation/reduction type of reaction.
A) C in C₂H₄
What are the reactants in the following equation: HCl(aq) + NaHCO₃(aq)→ CO₂(g) + H₂O(l) + NaCl(aq) A) HCl, NaHCO₃ B) HCl, CO₂ C) NaHCO₃, H₂O D) CO₂, H₂O E) H₂O, NaCl, CO₂
A) HCl, NaHCO₃
Boyle's Law explores the effects of pressure on the volume of an ideal gas. Boyle converted his observation into a mathematical formula. Which equation best represents the relationship between the pressure (P) and the volume (V) of the gas before and after compression? A) P₁V₁ = P₂V₂ B) P₁ / V₁ = P₂ / V₂ C) P₁T₁ = P₂T₂ D) PV = nRT E) P = V₁ / V₂
A) P₁V₁ = P₂V₂
When the ideas from Boyle's Law, Charles' Law and Gay-Lussac's Law are combined, you get the combined gas law. This law combines the effects of pressure, temperature and volume changes on a gas. The combined gas law can be defined as a mathematical relationship. Which equation best represents the relationship between the pressure (P), the volume (V), and the temperature (T) of a gas? A) P₁V₁/T₁ = P₂V₂/T₂ B) P₁V₁T₁ = P₂V₂T₂ C) P₁T₁/V₁ = P₂T₂/V₂ D) PV = nRT
A) P₁V₁/T₁ = P₂V₂/T₂
Consider the image of a manometer below. Based on the image, how does the pressure of the gas in the manometer compare to the pressure of the atmosphere? A) The gas pressure is higher than the atmospheric pressure. B) The gas pressure is lower than the atmospheric pressure. C) The gas pressure is the same as the atmospheric pressure.
A) The gas pressure is higher than the atmospheric pressure
Avogadro's Law explores the relationship between volume and number of moles of an ideal gas. Avogadro converted his observation into a mathematical formula. Which equation best represents the relationship between the number of moles and the volume (V) of the gas? A) V₁ / n₁ = V₂ / n₂ B) n₁V₁ = n₂V₂ C) T₁n₁ = T₂n₂ D) PV = nRT E) V = n₁ / n₂
A) V₁ / n₁ = V₂ / n₂
What type of reaction is represented by the following equation: KOH(aq) + NH₄Cl(aq) → NH₃(aq) + KCl(aq) + H₂O(l) A) acid-base B) decomposition C) precipitation D) redox (oxidation-reduction)
A) acid-base
Avogadro measured the volume of a gas when the number of moles changes. Avogadro noticed that the volume of a gas in a closed container is __________ to the number of moles of gas in the container. A) directly proportional B) exponentially larger C) inversely proportional D) exponentially smaller E) has no relation to
A) directly proportional
Charles' Law explores the effects of temperature on the volume of an ideal gas. Jacques Charles observed the change in volume of a gas when the temperature changes. A picture of a gas contained in a cylinder is shown below. Charles noticed that the volume of a gas in a closed container is __________ to the temperature of the gas in the container (assuming constant pressure). A) directly proportional B) exponentially larger C) inversely proportional D) exponentially smaller E) has no relation to
A) directly proportional
Gay-Lussac's Law explores the relationship between temperature and pressure of an ideal gas. Joseph Gay-Lussac measured the pressure of a gas when the temperature changes. Gay-Lussac noticed that the pressure of a gas in a closed container is __________ to the temperature of the gas in the container (assuming constant volume). A) directly proportional B) exponentially larger C) inversely proportional D) exponentially smaller E) has no relation to
A) directly proportional
Write the balanced NET ionic equation for the reaction when AlCl₃ and NaOH are mixed in aqueous solution. If no reaction occurs, simply write only NR.
Al³⁺(aq) + 3 OH⁻(aq) → Al(OH)₃(s)
Write the balanced COMPLETE ionic equation for the reaction when aluminum nitrate and sodium phosphate are mixed in aqueous solution. If no reaction occurs, simply write only NR.
Al³⁺(aq) + 3NO₃⁻(aq) + 3Na⁺(aq) + PO₄³⁻(aq) → AlPO₄(s) + 3Na⁺(aq) + 3NO₃⁻(aq)
Which of the following reactions is a double displacement reaction? A) HCl (g) → H₂ (g) + Cl₂ (g) B) HCl (aq) + NaOH (aq) → H₂O (l) + NaCl (aq) C) Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂ (g) D) HCl (g) + C₅H₁₀ (g) →C₅H₁₁Cl (g)
B) HCl (aq) + NaOH (aq) → H₂O (l) + NaCl (aq)
Which one of the following represents the net ionic equation for the reaction of HBr with Ca(OH)₂? A) Ca²⁺ (aq) + 2 Br⁻ (aq) → CaBr₂ (s) B) H⁺ (aq) + OH⁻ (aq) → H₂O (l) C) Ca²⁺ (aq) + 2 OH⁻ (aq) → Ca(OH)₂ (aq) D) H⁺ (aq) + Br⁻ (aq) → HBr (aq)
B) H⁺ (aq) + OH⁻ (aq) → H₂O (l)
Which of the following reactions is an acid-base reaction? A) AgNO₃(aq) + KF(aq) → AgF(s) + KNO₃(aq) B) NH₃(aq) + HF(aq) → NH₄⁺(aq) + F⁻(aq) C) NO₂⁻(aq) + Al(s) → NH₃(g) + AlO₂⁻(aq) D) CH₄(g) + 2O₂(g) → 2H₂O(g) + CO₂(g)
B) NH₃(aq) + HF(aq) → NH₄⁺(aq) + F⁻(aq)
Boyle's Law explores the effects of pressure on the volume of an ideal gas. A picture of a gas contained in a cylinder is shown below. When the piston is pushed down, the gas is compressed and the gas pressure inside is increasing. Which statement best describes the cause of gas pressure? A) The gas molecules take up more space. B) The collisions between rapidly moving gas molecules and the sides of the container increase in the smaller space. C) The weight of gas molecules pushing down on the bottom of this container increases in the smaller space. D) The repulsion between the charge of a gas molecule and the charge of the sides of the container increase in the smaller space. E) The air molecules are pushed out of the container.
B) The collisions between rapidly moving gas molecules and the sides of the container increase in the smaller space.
Write a balanced chemical equation based on the following description: solid barium carbonate decomposes into solid barium oxide and carbon dioxide gas when heated
BaCO₃(s) → BaO(s) + CO₂(g)
At 25.0° C, a 10.00 L vessel is filled with 7.00 atm of Gas A and 5.89 atm of Gas B. What is the mole fraction of Gas B? A) 12.89 B) 0.543 C) 0.457 D) 2.89
C) 0.457
What numbers belong in the blank spaces to fully balance the following reaction? __Fe (s) + __Cl₂ (g) → __FeCl₃ (s) A) 1,1,1 B) 1,2,1 C) 2,3,2 D) 2,2,2 E) 3,3,2
C) 2,3,2
Which one of the following changes would cause the pressure of a gas to double assuming volume and moles were held constant? A) Increasing the temperature from 20.0 °C to 40.0 °C. B) Decreasing the temperature from 400 K to 200 K. C) Increasing the temperature from 200K to 400K. D) Decreasing the temperature from 40.0 °C to 20.0 °C.
C) Increasing the temperature from 200K to 400K.
Balance the following chemical equation (if necessary) for the combustion reaction of propane: C₃H₈(g) + O₂(g) → CO₂(g) + H₂O(g
C₃H₈(g) + 5O₂(g) → 3CO₂(g) + 4H₂O(g
Which one of the following statements is correct about the reaction below? Mg(s) + 2 HCl(aq) → MgCl₂(s) + H₂(g) A) Mg is the oxidizing agent because it is losing electrons. B) H is the reducing agent because it loses electrons. C) Cl is the reducing agent because it is an anion. D) H is the oxidizing agent because it gains electrons.
D) H is the oxidizing agent because it gains electrons.
Which of the following is true for the reaction N₂(g) + 3 H₂(g) → 2 NH₃(g)? A) Nitrogen is oxidized. B) Hydrogen is reduced. C) Nitrogen is the reducing agent. D) Hydrogen is the reducing agent. E) Hydrogen is the oxidizing agent.
D) Hydrogen is the reducing agent.
In the reaction between FeCl₃ and NaOH, the spectator ions are A) Fe³⁺ and Cl⁻ B) Fe³⁺ and OH⁻ C) Na⁺ and OH⁻ D) Na⁺ and Cl⁻
D) Na⁺ and Cl⁻
Which of the following gases would be expected to have the highest density at STP? A) O₂ B) N₂ C) Ar D) O₃
D) O₃
Gay-Lussac's Law explores the relationship between temperature and pressure of an ideal gas. Gay-Lussac converted his observation into a mathematical formula. Which equation best represents the relationship between the temperature (T) and the pressure (P) of the gas before and after heat is added? A) P = T₁ / T₂ B) PV = nRT C) V₁T₁ = V₂T₂ D) P₁ / T₁ = P₂ / T₂ E) P₁V₁ = P₂V₂
D) P₁ / T₁ = P₂ / T₂
Which choice correctly identifies the oxidation number (O.N.) for the given species? A) Mn²⁺, O.N. = 0 B) Ca, O.N. = +2 C) F₂, O.N. = -1 D) Se²⁻, O.N. -2 E) P₄, O.N. = -1
D) Se²⁻, O.N. -2
The reaction of an alkane with oxygen to produce carbon dioxide and water is known as what? A) substitution B) displacement C) precipitation D) combustion E) double replacement
D) combustion
Which of the following species contains manganese with the highest oxidation number? A) Mn B) MnF₂ C) Mn₃(PO₄)₂ D) MnCl₄ E) NaMnO₄
E) NaMnO₄
Complete the balanced neutralization equation for the reaction below: HCl(aq) + NaOH(aq) →
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
Consider the chemical reaction that takes place between aqueous hydrochloric acid and aqueous sodium hydroxide. Complete the balanced neutralization equation for the reaction below: HCl(aq) + NaOH(aq) → Write the balanced COMPLETE ionic equation for the reaction. If no precipitation reaction occurs, simply write only NR. Write the balanced NET ionic equation for the reaction. If no reaction occurs, simply write only NR.
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) H⁺(aq) + Cl⁻(aq) + Na⁺ (aq) + OH⁻(aq) → Na⁺ (aq) + Cl⁻(aq) + H₂O(l) H⁺(aq) + OH⁻(aq) → H₂O(l)
Complete the balanced molecular chemical equation for the reaction below. If no reaction occurs, write NR after the reaction arrow. LiCl(aq) + K₃PO₄(aq) →
LiCl(aq) + K₃PO₄(aq) → NR
Write the balanced NET ionic equation for the reaction when nickel(II) iodide and aluminum sulfate are mixed in aqueous solution. If no reaction occurs, simply write only NR.
NR
Balance the following chemical equation (if necessary): V₂O₅(s) + HCl(aq) → VOCl₃(s) + H₂O(l
V₂O₅(s) + 6 HCl(aq) → 2 VOCl₃(s) + 3 H₂O(l
