General Chemistry I Exam 2 (Chapter 3 and 4)
Gaseous butane (CH3(CH2)2CH3 will react with gaseous oxygen to produce gaseous CO2 and gaseous H2O. Suppose 4.1 g of butane is mixed with 26.9 g of oxygen. Calculate the minimum mass of butane that could be left over
0 g
How many moles are present in 17.4 g of lead (Pb)? A. 0.0840 moles B. 0.0994 moles C. 1.05*10^25 D. 10.06 moles E. 11.9 moles
0.0840 moles
The chemical formula for lithium fluoride is LiF. A chemist measured the amount of lithium fluoride produced during an experiment. She finds that 59.3 g of lithium fluoride is produced. Calculate the number of moles of lithium fluoride produced.
2.29 moles
Calculate the molecular mass of barium acetate
255.43
Gaseous ethane (CH3CH3) reacts with gaseous O2 to produce gaseous CO2 and gaseous H2O. If 22.1 g of water is produced from the reaction 26.16 g of ethane and 181.2 g of O2, calculate percent yield of water.
47%
Determine the mass of 7.92*10^19 carbon dioxide molecules
5.79*10^-3 g
What is a combustion reaction?
A substance burns in the presence of oxygen
What is a reactant?
A substance present at the start of a reaction
Is H3SO3 ionic, molecular, acid or base?
Acid and molecular
Is H3PO3 ionic, molecular, acid or base?
Acid, molecular
Al
Aluminium
Sb
Antimony
Ba
Barium
Bk
Berkelium
Measurements show that unknown compound X has the following composition: Carbon-62.4% Hydrogen-4.19% Oxygen-33.2% Write the empirical formula
C5H4O2
Ds
Darmstadtium
Db
Dubnium
Dihydrogen Phosphate
H2PO4-
Which of these compounds is a strong electrolyte? A. H2SO4 B. C6H12 C. H2O D. O2 E CH3COOH (acetic acid)
H2SO4
H2SO4 (aq) + NaOH (aq) ---> ? Fill in products and balance. What type of reaction is this?
H2SO4 (aq) + 2NaOH (aq) ---> Na2SO4 (aq) + 2H2O (l) Acid-base
What is the ionization equation for sulfuric acid?
H2SO4(aq)---->H^+(aq)+HSO4^-(aq) HSO4^-(aq)<---->H^+(aq) SO4^2-(aq)
perbromic acid
HBrO₄ (aq)
What are the strong acids?
HCl, HBr, HI, HNO3, HClO3, HClO4, H2SO4
phosphoric acid
H₃PO₄ (aq)
Hypoiodite
IO-
I
Iodine
potassium hydroxide
KOH
Md
Mendelevium
Hg
Mercury
What is the reducing agent in the following reaction? A. Mg(OH)2 B. Mg C. H2O D. NiO2 E. Ni(OH)2
Mg
Permaganate
MnO4-
What is the oxidation number of each atom in NaH?
Na= +1 H = -1
sodium hydroxide
NaOH
Ru
Ruthnium
Sulfite
SO3 (2-)
Na
Sodium
Is AgNO3 soluble or insoluble?
Soluble
V
Vanadium
Is hydrofluoric acid a non-electrolyte, a weak electrolyte or a strong electrolyte?
Weak Electrolyte
Yb
Ytterbium
What element is undergoing oxidation in the following equation Zn (s) + 2AgNO3 (aq) ---> Zn(NO3)2 (aq) + 2Ag (s)
Zn
What is the formula for percent yield?
actual yield/theoretical yield x 100
What is the symbol for aqueous?
aq
What is the oxidation state of Cu in Cu2O(s)?
+1
What is the oxidation state of Cu in CuCl (s)?
+1
What is the oxidation state of K in K^+ (aq)?
+1
What is the oxidation state of Mn in KMnO4 (s) ?
+1
What is the oxidation state of N in NH4^+ (aq)?
+1
What is the oxidation state of Fe in Fe^3+ (aq) ?
+3
What is the oxidation state of V in V2O5 (s)?
+5
What is the oxidation state of I in I^- (aq)?
-1
What is the oxidation state of O in H3O (aq)?
-2
What is the oxidation state of O in OH^-(aq)
-2
What is the oxidation state of oxygen in Zn(NO3)2? A. -2 B. +2 C. -5 D. +5 E. -6
-2
What is the oxidation number of N in K3Fe(CN)6? A. -3 B. +4 C. -5 D. +1 E. +3
-3
What is the oxidation state of Cl in Cl2 (g)?
0
What is the oxidation state of H in H2(g)?
0
What is the oxidation state of N in N2 (g)?
0
What is the oxidation state of O in O2 (g)?
0
Green plants use light from the sun to drive photosynthesis, a chemical equation in which liquid water and carbon dioxide gas form aqueous glucose (C6H12O6) and oxygen (O2) gas. Calculate the moles of water needed to produce 0.060 mol of oxygen.
0.060 mol
Gaseous ammonia chemically reacts with oxygen (O2) gas to produce nitrogen monoxide gas and water vapor. Calculate the moles of nitrogen monoxide produced by the reaction of 0.080 mol of O2
0.064 mol
A chemist makes a 950 mL barium chlorate (Ba(ClO3)2) working solution by adding distilled water to 180 mL of 0.380 mol/L stack solution of barium chlorate in water. Calculate concentration in mol/L
0.072 mol/L
A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250 mL. What is the ammonium nitrate concentration in the resulting solution? A. 0.349 M B. 0.523 M C. 0.174 M D. 0.0872 M E. 2.18 M
0.0872 M
A chemist makes 680 mL of barium chlorate (Ba(ClO3)2) wokring solution by adding distilled water to 210 mL of a 0.314 M stock solution of barium chlorate in water. Calculate concentration in M.
0.0970 M
For an aqueous solution of glucose (C6H12O6) determine the molarity of 2.00 L of a solution that contains 50.0 g of glucose, the volume of this solution that contain 0.250 mol of glucose, and the number of moles of glucose in 0.500 L
0.139 M, 1.80 L and 0.069 mol
The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution (in M)? A. 0.10 M B. 0.20 M C. 0.40 M D. 0.36 M
0.20 M
Sodium hydrogen carbonate (NaHCO3) can be used to relieve indigestion. Which you get when your stomach contains too much HCl acid. Drinking water containing dissolved NaHCO3 neutralizes excess HCl. HCl (aq) + NaHCO3 (aq) ---> NaCl (aq) + H2O (l) + CO2 (g). The CO2 gas is what makes you burp. Suppose the fluid in the stomach can be considered to be 100 mL of a 0.029 M HCl solution. What mass of NaHCO3 would have to be ingested to neutralize that much HCl?
0.24 g
What volume (in L) of 0.150 M KCl solution will completely react with 0.150 L of a 0.175 M Pb(NO3)2 solution?
0.350 L
What is the molarity of 250 mL of a solution containing 5.9 g of sodium chloride?
0.40 M
Fe (s) + CuSO4 (aq) ---> Cu (s) + FeSO4 (aq) Suppose 200 mL of powdered iron is added to a CuSO4 sample until no more copper will precipitate. Then weighs it to come up with a mass of 59 mg. Calculate the original concentration of copper (II) sulfate in g/L
0.74 g/L
A major compound of gasoline is octane (C8H18). When liquid octane is burned in air it reacts with oxygen gas to produce carbon dioxide gas and water vapor. Calculate the moles of water produced by a reaction of 1.20 mol oxygen
0.864 mol H2O
What are the rules for assigning oxidation states?
1. Free elements are always 0 2. Monoatomic ions are equal to their charge 3. The sum of the states in a compound are 0 or the 4. The sum of the states in a polyatomic ion is the charge of the ion 5. Group 1 metals are +1 6. Group 2 metals are +2 7. Fluorine is -1 8. Hydrogen is +1 9. Oxygen is -2 10. Group 7A is -1 11. Group 6A is -2 12. Group 5A is -3
How to write a net ionic equation
1. Write a balanced molecular equation for the reaction. 2. Rewrite the equation to show the ions that form in solution when each soluble strong electrolyte dissociates into its ions. Only strong electrolytes dissolved in aqueous solution are written in ionic form. 3. Identify and cancel spectator ions.
What amount of Al2Cl3 (s) would be produced when 2.0 mol of Al (s) reacts with excess O2 (g) according to the balanced equation? 4Al (s) + 3O2 (g) ---> 2Al2Cl3 (s) A. 1.0 mol B. 1.3 mol C. 2.0 mol D. 4.0 mol E. 8.0 mol
1.0 mol
Determine the number of water molecular and the number of H and O atoms in 3.26 g of water.
1.09*10^23 molecules, 2.18*10^23 atoms, 1.09*10^23 atoms
Automobile batteries use sulfuric acid as an electrolyte. How much 1.20 M NaOH will be needed to neutralize 225 mL of 3.0 M H2SO4? H2SO4 (aq) + 2NaOH (aq) ----> 2H2O (l) + Na2SO4 (aq) A. 1.1 L B. 0.28 L C. 0.045 L D. 0.90 L E. 0.56 L
1.1 L
Calculate the volume in L of a 0.00321 mol/L copper (II) fluoride solution that contains 4.00 mol.
1.25*10^3 L
Ammonium phosphate (NH4)3 PO4 is an important ingredient in many solid fertilizers. It can be made reacting aqueous phosphoric acid (H3PO4) with liquid ammonia. Calculate the moles of ammonium phosphate produced by the reaction of 1.30 mol phosphoric acid
1.30 mol
A chemist adds 0.70 L of a 0.00224 M calcium sulfate (CaSO4) solution to a flask. Calculate the mmol of CaSO4 the chemist has added to the flask.
1.6 mol
An aluminum (Al) cube contains 2.68*10^23 atoms of Al. What is the edge length of the cube? The density of Al is 2.70 g/cm^3. Recall the Vcube=a^3 where a=edge length
1.64 cm
One way which the useful metal copper is produced is by dissolving the mineral azurite which contains copper (II) carbonate in a concentrated sulfuric acid. The acid reacts with copper (II) carbonate to produce a blue solution of copper (II) sulfate. Scrap iron is then added to the solution and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) ---> Cu (s) + FeSO4 (aq) Suppose an industrial quality-control chemist analyzes a sample from the copper processing plant in the following way: adds powered iron to a 200 mL of copper (II) sulfate sample from the plant until no more copper will precipitate, then washes, dried and weighs it. It has a mass of 132 mg. Calculate original concentration of copper (II) sulfate in mg/L
1.66 mg/L
A chemist prepares a solution of potassium permanganate (KMnO4) by measuring out 8.1 micromoles into a 450 mL flask. Calculate concentration in mmol/L
1.8 \*10^-2 mmol/L
A typical human body contains roughly 30 moles of calcium. Determine (a) the number of Ca atoms in 30.00 moles of calcium and (b) the number of moles of calcium in a sample containing 1.00*10^20 Ca atoms
1.807*10^25 atoms and 1.66^10^-4 moles
Determine the molarity of a solution formed by 0.874 g of MgCl2 in enough water to yield 5.00 mL of solution. The molar mass of MgCl2 is 95.21 g/mol. A. 0.00184 M B. 175 M C. 0.545 M D. 0.175 M E. 1.84 M
1.84 M
A chemist adds 1.95 L of a 9.8*10^-5 mmol/L silver (II) oxide (AgO) solution to a reaction flask. Calculate the micromoles added.
1.911*10^-1 micromol
The chemical formula for rubidium chloride is RbCl. A chemist determined by measurements that 0.085 moles of rubidium chloride participate in a chemical reaction. Calculate the mass of rubidium chloride that participates.
10 g
A chemistry student weighs out 0.196 g of chloroacetic acid (HCH2ClCO2) into a 250 mL flask and dilutes to the mark with water. He plans to titrate the acid with 0.1900 M NaOH solution. Calculate volume (in mL) of NaOH needed to reach equivalence point
10.9 mL
How many grams of lead (II) chloride (MW 278.1 g/mol) is produced if 13.87 g lead (II) nitrate (MW 331.22 g/mol) combines with excess hydrochloric acid to produce lead (II) chloride and nitric acid Pb(NO3)2 + 2HCl (aq) ---> PbCl2 (s) + 2HNO3 (aq) A. 11.65 g B. 14.33 g C. 0.086 g D. 5.82 g E. 16.52 g
11.65 g
Liquid Hexane (CH4(CH2)4CH3) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). Suppose 23.3 g of hexane is mixed with 41 g of oxygen. Calculate the minimum mass of hexane left over
12 g
This is the chemical formula for chromium (III) carbonate Cr2(CO3)3 Calculate the mass percent of carbon
13%
A chemist prepares a solution of sodium chloride (NaCl) by measuring out 3.6 mol of sodium chloride into a 250 mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in micromoles/L.
14 micro M
This is the chemical formula for diethyl ether (CH3CH2)2O Calculate mass percent of hydrogen
14%
A chemist must dilute 13.0 mL of 5.42 mM aqueous calcium sulfate (CaSO4) solution until the concentration falls to 4.00 mM. She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate the final volume in mL.
17.6 mL
Ammonium phosphate (NH4)3PO4 is an important ingredient in many fertilizers. It can be made by reacting phosphoric acid (H3PO4) with ammonia (NH3). What mass of ammonium phosphate is produced by the reaction of 6.0 g of ammonia
18 g
What is the molecular mass of H2O?
18.02 amu
N2O is commonly used as an anesthetic in dentistry. It is manufactured by heating ammonium nitrate. The balanced equation is: NH4NO3(s) ------> N2O (g) + 2H2O (g) Calculate the mass of ammonium nitrate that must be heated in order to produce 10.0 g of N2O Determine the corresponding mass of H2O produced in the reaction
18.2 g NH4NO3 and 8.19 g H2O
Calculate the percent composition by mass of lithium in lithium carbonate
18.78%
Ammonium perchlorate (NH4ClO4) is a powerful solid rocket fuel used in the Space Shuttle boosters. It decomposes into nitrogen (N2) gas, chlorine (Cl2) gas, oxygen (O2) gas and water vapor, releasing a great deal of energy. Caclulate the moles of water produced by the reaction of 1.00 moil of ammonium perchlorate.
2.00 mol
The density of water is 1.00 g/mL at 4 degrees C. How many water molecules are present in 6.25 mL of water at this temperature? Na=6.022*10^23 A. 3.76*10^24 molecules B. 2.09*10^23 molecules C. 6.02*10^23 molecules D. 0.347 molecules E. 6.26*10^23 molecules
2.09*10^23 molecules
If a 0.584 L of a 2.5 M soldium chloride solution was diluted to 700 mL, what is the molarity of the diluted sodium chloride solution? A. 2.1*10^-2 M B. 2.1 M C. 3.0*10^3 M D. 3.0 M E. 1.5 M
2.1 M
The chemical formula for potassium bromide is KBr. A chemist measured the amount of potassium bromide produced during an experiment. She finds 255 g of potassium bromide is produced. Calculate the number of moles
2.14 moles
A major component of gasoline is octane (C9H18). When octane is burned in air, it chemically reacts with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O) What mass of water is produced by the reaction of 5.5 g of oxygen gas.
2.2 g
A chemist adds 60.0 mL of a 1.9 M silver perchlorate (AgClO4) solution to a reaction flask. Calculate the mass in grams that has been added
2.4*10^1 g
Ammonia (NH3) chemically reacts with oxygen gas (O2) to produce nitric oxide (NO) and water (H2O). What mass of ammonium is consumed by the reaction of 5.86 g of O2?
2.49 g
Aqueous hydrochloric acid (HCl) will react to solid sodium hydroxide (NaOH) to produce aqueous sodium chloride and liquid water. Suppose 5.10 g of HCl mixed with 10 g NaOH. Calculate the maximum mass of H2O that could be produced
2.52 g
What volume (in mL) of 12.0 M HCl must be used to prepare 250 mL of 0.125 M HCl
2.60 mL
Urea is synthesized in the laboratory by the combination of ammonia and carbon dioxide according to the equation 2NH3 (g) + CO2 (g) -----> (NH2)2 CO(aq) + H2O(l) Calculate the amount of urea that will be produced by the complete reaction of 5.25 mol of ammonia. Determine the stoichiometric amount of CO2 required to react to 5.25 mol of ammonia
2.63 mol Urea and 2.63 mol CO2
Calculate volume in mL of a 1.9 M iron (III) bromide solution that contains 150 g.
2.7*10^2 mL
Wine goes bad soon after opening because of the ethanol (CH3CH2OH) in it reacts with oxygen gas (O2) from the air to form water (H2O) and acetic acid (CH3COOH), the main ingredients of vinegar
2.88 g
A chemist must prepare 775 mL of 5.00 M aqueous silver nitrate (AgNO3) working solution. He'll do this by pouring out some 13.4 M. Calculate volume in mL that should be poured out.
2.89 mL
Ammonium perchlorate (NH4ClO4) is a solid rocket fuel used by the US Space Shuttle. It reacts with itself to produce nitrogen gas (N2), chlorine gas (Cl2), oxygen gas (O2), water (H2O) and a great deal of energy. What mass of chlorine gas is produced by the reaction of 9.6 g of ammonium perchlorate?
2.9 g
Calculate the molecular mass of lithium hydroxide
23.95 amu
Calculate the molar mass of Ca(BO2)2 * 6H2O A. 143.71 g/mol B. 174.89 g/mol C. 183.79 g/mol D. 233.80 g/mol E. 273.87 g/mol
233.80 g/mol
A chemist must prepare 450 mL of 1.00 M aqueous barium acetate (Ba(C2H3O2)2) working solution. He'll do this by pouring out some 1.85 M aqueous barium acetate stack solution into a graduated cylinder and diluting with distilled water. Calculate volume in mL of barium acetate stock solution that the chemist should pour out.
243 mL
Liquid octane (CH3(CH2)6CH3) will react with gaseous oxygen (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). Suppose 19 g of octane is mixed with 129 g oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction
27 g
Aqueous sulfric acid (H2SO4) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium sulfate (Na2SO4) and liquid water (H2O). Suppose 76n g of sulfric acid is mixed with 87.4 g of sodium hydroxide. Calculate the maximum mass of water that could be produced by a chemical reaction
28 g
the following chemical reaction takes place in an aqueous solution: 2AgF (aq) + Na2CO3 (aq) ----> Ag2CO3 (s) + 2NaF (aq) Write the net ionic equation
2Ag^+ (aq) + CO3^2- (aq) ---> Ag2CO3 (s)
The following chemical equation takes place in aqueous solution: 2AgNO3 (aq) + (NH4)2S (aq) ---> Ag2S (s) + 2NH4NO3(aq) Write the net ionic equation
2Ag^+ (aq) + S^2- (aq) -----> Ag2S(s)
Balance this equation C4H10(g) + O2(g) ----> 4CO2(g) + 5H2O(l) What is this equation an example of?
2C4H10(g) + 13O2(g) ----> 8CO2(g) + 10H2O(l), combustion
Ca (s) + O2 (g) ---> ? Fill in products and balance. What type of reaction is this?
2Ca (s) + O2 (g)----> 2CaO (s) Redox
Aqueous cobalt (III) nitrate reacts with aqueous sodium sulfide. A. Write a balanced molecular equation for this reaction B. Write the complete ionic equation for this reaction C. Write the net ionic equation for this reaction D. List spectator ions
2Co(NO3)3 (aq) + 3Na2S (aq) ---> Co2S3 (s) + 6NaNO3 (aq) 2Co^3+ (aq) + 6NO3^- (aq) + 6Na^+ (aq) + 3S^2- (aq) ---> Co2S3 (s) + 6NO3^- (aq) + 6Na^+ (aq) 2Co^3+ (aq) + 3S^2- (aq) ---> Co2S3 (s) Na^+ and NO3^-
Which of the following is an acid-base reaction? A. C (s) + O2 (g) --> CO2 (g) B. Fe (s) + 2AgNO3 (aq) --> 2Ag (s) + Fe(NO3)2 (aq) C. 2HClO4 (aq) + Ca(OH)2 (aq) ---> 2H2O (l) + Ca(ClO4)2 (aq) D. MgSO4 (aq) + Pb(NO3)2 (aq) ---> Mg(NO3)2 (aq) + PbSO4 (s)
2HClO4 (aq) + Ca(OH)2 (aq) ---> 2H2O (l) + Ca(ClO4)2 (aq)
Predict the products of the reaction below. That is, complete the right hand side of the equation. Be sure the equation is balanced. HClO4 + Ca(OH)2 ---->
2HClO4 + Ca(OH)2 ---> Ca(ClO4)2 + 2H2O
Predict the products of the reaction below. That is, complete the right hand side of the chemical equation. Make sure it's balanced. HNO3 + Ca(OH)2 --->
2HNO3 + Ca(OH)2 ----> Ca(NO3)2 + 2H2O
Please identify the complete ionic equation for the reaction between aqueous sodium sulfide and aqueous copper (II) chloride resulting in precipitation reaction A. ZNa^+ (aq) + S^2- (aq) + Cu^2+ (aq) + Cl^- (aq) ---> CuS (s) + 2NaCl (s) B. Na2^2+ (aq) + S^2- (aq) + Cu^2+ (aq) + Cl^- (aq) ---> CuS (s) + Na^+ + Cl2^2- (aq) C. 2Na^+ (aq) + S^2- (aq) + Cu^2+ (aq) + Cl^2- (aq) ----> CuS (s) + 2Na^+ (aq) + 2Cl^- (aq) D. 2Na^+ (aq) + 2Cl^- (aq) ---> 2NaCl (s) E. Cu^2+ (aq) + S^2- (aq) ---> CuS (s)
2Na^+ (aq) + S^2- (aq) + Cu^2+ (aq) + Cl^2- (aq) ----> CuS (s) + 2Na^+ (aq) + 2Cl^- (aq)
Balance the chemical equation below using the smallest possible whole number coefficients. Si4H10(l) + O2(g) ---> SiO2(s) + H2O
2Si4H10(l) + 13O2(g) ----> 8SiO2 (s) + 10H2O(l)
What is the oxidation state of Fe in Fe2O3 (s)?
3+
Gaseous methane (CH4) reacts with gaseous O2 to produce gaseous CO2 and gaseous H2O. What is the theoretical yield of 1.4 g of methane and 8.1 g of oxygen?
3.1 g
A chemist prepares a solution of barium chloride (BaCl2) by measuring out 8.2 micromole into a 250 mL flask and filling to the mark with water. Calculate the concentration in mol/L
3.3*10^-5 mol/L
Using the balanced equation below, answer the following questions. 2Na3PO4 (aq) + 3CuCl2 (aq) ---> Cu3(PO4)2 (s) + 6NaCl (aq) A. If you react 63.2 mL of 0.54 M Na3PO4 with 84.9 mL of 0.32 M CuCl2. How many grams of Cu3(PO4)2 will you produce?
3.4 g
What volume of 0.584 M AgNO3 is required to react exactly with 0.745 L of 1.5 M Na2SO4 solution? 2AgNO3 + NaSO4 ---> 2NaNO3 + AgSO4 A. 0.58 L B. 0.29 L C. 0.0038 L D. 3.8 L E. 1.9 L
3.8 L
A chemist adds 430.0 mL of a 0.537 mol/L sodium thiosulfate (Na2S2O3) solution to a reaction flask. Calculate the mass in grams the chemist added.
36.5 g
Ca(OH)2 (aq) + FeCl3 (aq) ---> ? Fill in products and balance. What type of reaction is this?
3Ca(OH)2 (aq) + 2FeCl3 (aq) ---> 3CaCl2 (aq) + 2Fe(OH)3 (s) Precipitation
Hydrogen gas reacts with nitrogen gas to produce ammonia gas. Write a balanced chemical equation for this
3H2(g) + N2(g) ---> NH3(g)
Gaseous methane (CH4) will react with gaseous (O2) to produce gaseous CO2 and gaseous H2O. Suppose 12 g of methane is mixed with 25.5 g of oxygen. Calculate the minimum mass of methane that could be left over
4.6 g
Calculate the molecular mass of propane
44.094 amu
A 0.8633 g sample of an ionic compound containing chloride ions and an unknown metal cation is dissolved in water and treated with excess of AgNO3. If 1.5615 g of AgCl precipitate forms, what is the percent by mass of Cl in the original compound?
44.73%
What volume in mL of 0.203 M sodium hydroxide solution is needed to neutralize 25.0 mL of a 0.188 M sulfuric acid solution?
46.3 mL
This is the chemical formula for methyl acetate (CH3)2CO2 Calculate the mass percent of carbon
49%
The chemical formula for barium oxide is BaO. A chemist measured the amount of barium oxide produced during an experiment. She finds that 784 grams of barium oxide is produced. Calculate the number of moles
5.11 moles
Give the percent yield when 28.16 g of CO2 are formed from the reaction of 5.0 moles of C8H18 with 19 moles of O2. Molar mass of CO2 is 44.01 g/mol. A. 1.60% B. 10.6% C. 5.26% D. 52.6% E. 190%
5.26%
How many moles of KCl are contained in 10.0 mL of solution of 5.6 M KCl? A. 5.6 moles B. 0.56 moles C. 5.6*10^4 moles D. 5.6*10^-2 moles E. 5.6*10^3 moles
5.6*10^-2 moles
How many atoms of oxygen are contained in 3.04 g of Fe2(CO3)3? The molar mass is 291.72 g/mol A. 5.65*10^22 atoms B. 3.34*10^22 atoms C. 1.00*10^23 atoms D. 3.01*10^23 atoms E. 5.65*10^24 atoms
5.65*10^22 atoms
Green plants use light from the sun to drive photosynthesis. A chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the 2 simple glucose sugar (C6H12O6) and oxygen gas (O2) What mass of simple sugar glucose is produced by the reaction of 8.69 CO2
5.93 g
What is the percent carbon in CH3OH2OH? A. 35% B. 13% C. 26% D. 52%
52%
Calculate mass percent composition of oxygen in Al(NO2)3 A. 16.34% B. 58.17% C. 29.09% D. 19.39% E. 69.85%
58.17%
What does 1 mol equal?
6.022x10^23
Aqueous hydrobromic acid (HBr) reacts with sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water. What is the theoretical yield of water formed from 74.4 g of HBr and 1.4 g of NaOH?
6.31 g
Calculate volume in mL of a 0.35 M nickel (II) chloride solution that contains 225 mmol
6.4*10^2 mL
Suppose an EPA chemist test a 250 mL sample of groundewater that is known to be contaminated with nickel (II) chloride, which would react with silver nitrate NiCl2 (aq) + 2AgNO3 (aq) ---> 2AgCl (s) + Ni(NO3)2 (aq) The chemist adds 12.0 mM silver nitrate solution the sample. The silver nitrate weighs 3.6 mg. Calculate concentration (mg/L) of nickel (II) chloride in the original sample.
6.5 mg/L
An analytical chemist weighs out 0.146 g of an unknown monoprotic acid into a 250 mL flask and dilutes to the mark with water. He then titrates the solution with 0.0800 M NaOH solution. When it reaches the equivalence point, 30.4 mL of NaOH have been added. Calculate molar mass of unknown acid.
60.0 g/mol
The chemical formula for acetic acid is CH3COOH. Calculate the molar mass. Round to two decimal places
60.05 g*mol^-1
Suppose the combustion of 18.8 g of glucose produced 27.6 g of CO2 and 11.3 g of H2O. Calculate the mass of C and H in the original sample of glucose
7.53 g C and 1.26 g H
A chemist adds 485.0 mL of a 0.15 mol/L potassium iodide (KI) solution to a reaction flask. Calculate the mmoles of KI the chemist added to the flask.
72 mmol
Here is the chemical formula for hexanal CH3(CH2)4CHO Calculate the mass percent of carbon
72%
Gaseous ethane (CH3CH3) will react with gaseous O2 to produce gaseous CO2 and gaseous H2O. Suppose 25 g of CH3CH3 is mixed with 148 g of O2. Calculate the maximum mass of carbon dioxide that could be produced
73 g
Aspirin, acetylsalicylic acid (C9H8O4) is produced by the reaction of salicylic acid (C7H6O3) and acetic anhydride (C4H6O3) according to the following equation: C7H6O3+C4H6O3----->C9H8O4+HC2H3O2 In certain aspirin sythesis 104.8 g of salicylic acid and 110.9 g of acetic anhydride are combined. Calculate the percent yield of the reaction if 105.6 g of aspirin are produced
77.25%
The first step in the Ostwald process for producing nitric acid is 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g). If the reaction of 15.0 g of ammonia (17.04 g/mol) with 15.0 g of oxygen gas (32.0 g/mol) yields 8.70 g of nitric monoxide (30.01 g/mol) , what is the percent yield of this reaction? A. 61.8% B. 29.0% C. 32.9% D. 77.3% E. 49.5%
77.3%
A 0.1216 g sample of a monoprotic acid is dissolved in 25 mL water and the resulting solution is titrated with 0.1104 M NaOH solution. A 12.5 mL volume of the base is required to neutralize the acid. Calculate the molar mass of the acid in g/mol
88.1 g/mol
Aqueous hydrobromic acid (HBr) will react with solid sodium hydroxide (NaOH) to produce aqueous sodium bromide (NaBr) and liquid water (H2O). Suppose 23 g of hydrobromic acid is mixed with 3.71 g of sodium hydroxide. Calculate the maximum mass of sodium bromide that could be produced
9.54 g
An analytical chemist weighs out 0.193 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates the solution with 0.0600 M NaOH solution. Once the equivalence point is reached, 98.5 mL of NaOH have been added. Calculate molar mass
98.0 g/mol
A chemist must dilute 37.0 mL of 567 mM aqueous copper (II) sulfate (CuSO4) solution until the concentration falls to 213 mM. She'll do this by adding distilled water to the solution until it reaches a certain final volume. Calculate the final volume in mL.
98.5 mL
What is a complete ionic equation?
A complete ionic equation is separating the compounds of the reactants and products of a skeleton equation into separate elements -the exception is one can not separate the compounds of a solid compound product or a polyatomic
What is the percent composition by mass?
A list of the percent by mass of each element in a compound
What is combustion analysis?
A method to experimentally determine the empirical formula
What is an oxidation number?
A number assigned to an element in chemical combination that represents the number of electrons lost (or gained, if the number is negative) by an atom of that element in the compound.
What is a displacement reaction?
A reaction in which a more reactive element takes the place of a less reactive element in a compound
Choose the statement below that is true A. A weak acid solution consists of partially ionized acid molecules and is a strong electrolyte B. A strong electrolyte solution conducts electricity C. A strong acid solution consists of only partially ionized acid molecules D. An example of a weak electrolyte is glucose (C6H12O6) E. A molecular compound that doesn't ionize in solution is considered a strong electrolyte
A strong electrolyte solution conducts electricity
What is an acid-base titration?
A substance in a solution of known concentration is reacted with another substance in a solution of unknown concentration
What is an indicator?
A substance that changes color in the presence of an acid or a base
What is an Arrhenius base?
A substance that produces OH- in water
What is a redox titration?
A titration of a reducing agent by an oxidising agent (or vice versa)
Ac
Actinium
Based on the solubility rules, which of these compounds is insoluble in water? A. MgBr B. ZnCl2 C. AgBr D. NaCl E. FeCl2
AgBr
Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4)2(aq) + 2 Ag(s) A. AgClO4 B. NI C. NI(ClO4)2 D. Ag
AgClO4
Which one of the following compounds is soluble in water? A. AgNO3 B. AgCl C. AgC2H3O2 D. Both B and C E. All are soluble
AgNO3 and AgC2H3O2
Which one of the following compounds is insoluble in water? A. Na2SO4 B. KNO3 C. Sr(C2H3O2)2 D. NH4Cl E. All are soluble
All are soluble
Am
Americium
What is concentration?
Amount of solute dissolved in a solvent
What is an acid-base neutralization?
An acid base reaction where water and an ionic compound are produced as products
What is a polyprotic acid?
An acid that can donate more than one proton per molecule
What is gravimetric analysis?
An analytical technique that relies almost exclusively on mass measurements
What is a net ionic equation?
An equation for a reaction in solution that shows only those particles that are directly involved in the chemical change
What is a molecular equation?
An equation that shows the complete neutral formulas for each compound in the reaction as if they existed as molecules
What is an Arrhenius acid?
Any substance that produces hydrogen ions in water
Ar
Argon
As
Arsenic
At
Astatine
Which of the follwing is a redox reaction? A. HBr (aq) + NaOH (aq) ---> NaBr (aq) + H2O (l) B. Ba (s) + 2HCl (aq) --> BaCl2 (aq) + H2 (g) C. NaI (aq) + AgNO3 (aq) ---> AgI (s) + NaNO3 (aq) D. Pb (C2H3O2)2 (aq) + 2LiBr (aq) ---> PbBr2 (s) + 2LiC2H3O2 (aq)
Ba (s) + 2HCl (aq) --> BaCl2 (aq) + H2 (g)
Write and balance the chemical equation for the aqueous reaction of barium hydroxide and perchloric acid to produce aqueous barium perchlorate and water
Ba(OH)2 (aq) + 2HClO4(aq) ----> Ba(ClO4)2 (aq) + 2H2O(l)
barium hydroxide
Ba(OH)₂
Be
Beryllium
Bi
Bismuth
Bh
Bohrium
B
Boron
Hypobromite
BrO-
Bromite
BrO2-
Bromate
BrO3-
Perbromate
BrO4-
Br
Bromine
What is combustion?
Burning a compound in the presence of oxygen
Write out the chemical equation for solid graphite reacting with gaseous oxygen to form gaseous carbon dioxide
C (s) + O2 (g) -----> CO2(g)
The percent composition by mass of a compound is 76.0% C, 12.8% H and 11.2% O. The molar mass of this compound is 284.5 g/mol. What is the molecular formula? A. C18H36O2 B. C16H28O4 C. C10H6O D. C9H18O E. C20H12O2
C18H36O2
Acetate
C2H3O2-
A common hydrocarbon, contains only carbon and hydrogen, was found to have 82.6% carbon by mass and 17.4% hydrogen by mass A. Determine empirical formula B. Determine molecular formula if the molecular weight is 58.14 g/mol
C2H5, C4H10,
Measurements indicate that unknown compound X is composed of the following: Carbon-41.0% Hydrogen-4.58% Oxygen-54.6% Write the empirical formula
C3H4O3
Assuming the only products are CO2 and H2O write and balance the equation for the metabolism of butyric acid C4H8O2
C4H8O2(aq) + 5O2 -----> 4CO2 + 4H2O
Balance the following equation: C8H18O3 (l) + O2 (g) ---> H2O (g) + CO2 (g) A. 2C8H18O3 (l) + 17O2 (g) ---> 18H2O (g) B. 2C8H18O3 (l) + 22O2 (g) ---> 9H2O (g) + 16CO2 (g) C. C8H18O3 (l) + 13O2 (g) ---> 18H2O (g) + 8CO2 (g) D. C8H18O3 (l) + 11O2 (g) ---> 9H2O (g) + 8CO2 (g) E. C8H18O3 (l) + 8O2 (g) ---> 9H2O (g) + 8CO2 (g)
C8H18O3 (l) + 11O2 (g) ---> 9H2O (g) + 8CO2 (g)
Combustion of 5.50 g sample of benzene produces 18.59 g CO2 and 3.81 g H2O. Determine the empirical and molecular formula of benzene given that the molar mass is about 78 g/mol
CH and C6H6
Measurements show that unknown compound X has the following composition Carbon-74.8% Hydrogen-25.1%
CH4
Cyanide
CN-
Measurements show that unknown compound X has the following composition Carbon-42.9% Oxygen-57.2% Write the empirical chemical formula for X
CO
Carbonate
CO3 (2-)
calcium hydroxide
Ca(OH)₂
Measurements show that unknown compound X has the following composition: Calcium-38.8% Phosphorus-20.0% Oxygen-41.3% Write the empirical chemical formula for X
Ca3P2O8
Cd
Cadmium
Ca
Calcium
Cf
Californium
C
Carbon
Ce
Cerium
Cs
Cesium
Cl
Chlorine
Cr
Chromium
Hypochlorite
ClO-
Chlorite
ClO2-
Chlorate
ClO3-
Perchlorate
ClO4-
Co
Cobalt
H2(g)+Br2(g) ----> 2HBr(g) Is an example of what type of reaction?
Combination
NH3 (g) + HCl(g) ---> NH4Cl(s) Is an example of what type of reaction?
Combination
2HCO2H(l)+O2(g)---->2CO2(g)+2H2)(l) Is an example of what type of reaction?
Combustion
CH2O(l)+O2(g)---->CO2(g)+H2O(g) Is an example of what type of reaction?
Combustion
What is an acid?
Compound that dissolve in water to produce hydronium ion
What are Molecular bases?
Compounds that dissolve in water to produce hydroxide ions
Cn
Copernicum
Cu
Copper
Dichromate
Cr2O7 (2-)
Chromate
CrO4 (2-)
cesium hydroxide
CsOH
8Cu (s) + S8 (s) ---> 8CuS(s) Write the chemical formula for any reactants that will be oxidized and any reactants that will be reduced
Cu is oxidized and S8 is reduced
Cm
Curium
2KClO3(s) -> 2KCl(s) + 3O2(g) Is an example of what type of reaction?
Decomposition
CaCO3(s) --> CaO(s) + CO2(g) Is an example of what type of reaction?
Decomposition
How do you identify electrolytes?
Determine whether it is ionic or molecular, any ionic that dissolves in water is strong, for a molecular you need to determine if it is an acid or not
What are strong electrolytes?
Dissolves completely, strong acids, strong bases, soluble salts (ionic compounds)
What is a monoprotic acid?
Donates one proton when dissociating in aqueous solutions
What is a triprotic acid?
Donates three protons when dissociating in aqueous solutions
What is a diprotic acid?
Donates two protons when dissociating in aqueous solution
Dy
Dysprosium
Es
Einsteinium
What is the difference between an empirical formula and a molecular formula?
Empirical formula shows the simplest whole number ratio while molecular shows exact number of each type of atom
Er
Erbium
Eu
Europium
The spectator ion is always included in the net ionic equation. True or false?
False
Write the net ionic equation and indicate which element is oxidized and which is reduced: Fe(s) + PtCl2 (aq) --->
Fe (s) + PtCl2 ----> FeCl2 (aq) + Pt (s) Fe is oxidized Pt is reduced
4Fe (s) + 3O2 (g) ---> 2Fe2O3 (s) Write the chemical formula for any reactants that will be oxidized and any reactants that will be reduced
Fe is oxidized and O2 is reduced
Measurements show that within unknown compound X there is: Iron-69.9% Oxygen-30.0% Write the empirical formula
Fe2O3
Fm
Fermium
F
Fluorine
Fr
Francium
Gd
Gadolinium
What is reduction?
Gain of electrons
Ga
Gallium
Write out NH3(g) + HCl(aq) -----> NH4Cl(aq)
Gaseous ammonia and aqueous hydrogen chloride react to produce aqueous ammonium chloride
Ge
Germanium
Au
Gold
What compounds are soluble in water no matter what?
Group 1A, ammonium, nitrate ion, acetate ion or chlorate ion
Hydronium
H3O+
What is the percent mass of H2O2?
H=5.926% O=94.06%
hydrobromic acid
HBr (aq) (strong acid)
What is the ionization equation for hydrobromic acid?
HBr(aq) ----> H^+(aq)+Br^-(aq)
hypobromous acid
HBrO (aq)
bromous acid
HBrO₂ (aq)
bromic acid
HBrO₃ (aq)
hydrochloric acid
HCI (strong acid)
hydrocyanic acid
HCN (aq)
bicarbonate (hydrogen carbonate)
HCO3-
What is the ionization equation for hydrochloric acid?
HCl(aq) ---> H^+(aq) + Br^- (aq)
hypochlorous acid
HClO (aq)
What is the ionization equation for chloric acid?
HClO3(aq)---->H^+(aq)+ClO3^-(aq)
Predict the products of the reaction below. That is, complete the right-hand side of the chemical equation. Be sure it is balanced HClO4 + KOH ---->
HClO4 + KOH ---> KClO4 + H2O
What is the ionization equation for perchloric acid?
HClO4(aq)---->H^+(aq)+ClO4^-(aq)
chlorous acid
HClO₂ (aq)
chloric acid
HClO₃ (aq) (strong acid)
perchloric acid
HClO₄ (aq) (strong acid)
acetic acid
HC₂H₃O₂ (aq)
hydrofluoric acid
HF
hydroiodic acid
HI (aq) (strong acid)
What is the ionization equation for hydroiodic acid?
HI(aq)--->H^+(aq)+I^-(aq)
hypoiodous acid
HIO (aq)
iodous acid
HIO₂ (aq)
iodic acid
HIO₃ (aq)
periodic acid
HIO₄ (aq)
What is the ionization equation for nitric acid?
HNO3(aq) --->H^+(aq)+NO3^-(aq)
nitrous acid
HNO₂ (aq)
nitric acid
HNO₃ (aq) (strong acid)
Hydrogen Phosphite
HPO3 (2-)
Hydrogen Phosphate
HPO4 (2-)
Bisulfite (hydrogen sulfite)
HSO3-
bisulfate (hydrogen sulfate)
HSO4-
What is the net ionic equation if sodium sulfate is mixed with barium hydroxide? A. 2Na^+ (aq) + SO3^2- (aq) ---> Na2SO4 (s) B. Ba^2+ (aq) + 2OH^- (aq) ---> Ba(OH)2 (s) C. SO4^2- (aq) + 2Na^+ (aq) ---> Na2SO4 (aq) D. H^+ (aq) + OH^- (aq) ---> H2O (l) E. SO4^2- (aq) + 2Na^+ (aq) ---> Na2SO4 (s)
H^+ (aq) + OH^- (aq) ---> H2O (l)
Hf
Hafnium
Hs
Hassium
He
Helium
Ho
Holmium
What is a solution?
Homogeneous mixture of 2 or more substances
H
Hydrogen
hydrosulfuric acid
H₂S (aq)
sulfurous acid
H₂SO₃ (aq)
sulfuric acid
H₂SO₄ (aq) (strong acid)
phosphorous acid
H₃PO₃ (aq)
Iodite
IO2-
Iodate
IO3-
Periodate
IO4-
Compounds containing the sulfate ion are usually soluble. What are the exceptions?
If it is with Ag^+, H2^2+, Pb^2+, Ca^2+, Sr^2+ or Ba^2+
Compounds containing the chloride ion, bromide ion or iodide ion are typically soluble. What are the exceptions?
If it is with Ag^+, Hg2^2+ or Pb^2+
Compounds containing the hydroxide ion are typically insoluble. What are the excpetions?
If they contain Li^+, Na^+, K^+, Rb^+, Cs^+ or Ba^2+
Compounds containing the carbonate ion, phosphate ion, chromate ion or sulfide ion are typically insoluble. What are the excpetions?
If they contain Li^+, Na^+, K^+, Rb^+, Cs^+ or NH4^+
In
Indium
Is CaSO4 soluble or insoluble?
Insoluble
What is a precipitate?
Insoluble solid product that separates from solution
Is MgCl2 ionic, molecular, acid or base?
Ionic
Is Ba(OH)2 ionic, molecular, acid or base?
Ionic and base
What are spectator ions?
Ions that do not participate in a reaction
Ir
Iridium
Fe
Iron
Kr
Krypton
La
Lanthanum
Lr
Lawrencium
Pb
Lead
lithium hydroxide
LiOH
What are the strong bases?
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
Li
Lithium
What is oxidation?
Loss of electrons
Lu
Lutetium
Mg
Magnesium
Mn
Manganese
What is the formula for percent by mass?
Mass of element/mass of compound x 100
What is solubility?
Max amount of solute that will dissolve in a given quantity of solvent in a specific way
Mt
Meitnerium
What is always constant in dilution?
Moles
How do you calculate molarity?
Moles of solute/liters of solution
Mo
Molybdenium
Compound X has a molar mass of 104.01 grams per mol and the following composition: Nitrogen-26.13% Fluorine-73.07% Write the molecular formula
N2F4
Azide
N3-
Ammonium
NH4+
ammonia
NH₃ (weak base)
Determine the empirical formula of a compound that is 30.45% Nitrogen and 69.55% oxygen by mass
NO2
Nitrite
NO2-
Nitrate
NO3-
Based on the solubility rules, which of the following should be soluble in water? A. Hg2Cl2 B. BaCO3 C. Na2S D. Ag2CO3 E. Ag2S
Na2S
The mixing of which pair of reactants will result in a precipitation reaction? A. NH4I (aq) + NaOH (aq) B. HCl (aq) + Ca (OH)2 (aq) C. KNO3 (aq) + NH4F (aq) D. Na2SO4 (aq) + Ba(NO3)2
Na2SO4 (aq) + Ba(NO3)2
Give the spectator ions for the reaction that occurs when aqueous solutions of Na2S and CuCl2 are mixed to form aqueous NaCl and solid CuS. A. Na^+ and Cl^- B. Cu^2+ and S^2- C. S^2- and Cl^- D. Na^+ and Cu^2+ E. None
Na^+ and Cl^-
Nd
Neodymium
Ne
Neon
Np
Neptunium
Ni (s) + Cl2 (g) ---> NiCl2 (s) Write the chemical formula for any reactants that will be oxidized and any reactants that will be reduced
Ni is oxidized and Cl2 is reduced
Ni
Nickel
Nb
Niobium
N
Nitrogen
Does a precipitate form from zinc acetate and iron (II) chloride? If so, what is the empirical formula?
No
Is the below equation a redox reaction? If so, what is the reducing agent and oxidizing agent? HCl (aq) + NH3 (aq) ---> NH4Cl (aq)
No
No
Nobelium
Is methanol a non-electrolyte, a weak electrolyte or a strong electrolyte?
Non-electrolyte
What value remains constant in a dilution calculation? A. number of moles B. volume C. molarity D. number of moles and molarity E. number of moles and volume
Number of moles
What is the limiting reagent when 5 moles of C8H18 is reacted with 19 moles of O2? A. C8H18 B. CO2 C. O2 D. H2O E. There is no limiting reagent
O2
What is the oxidation state of each atom in SO2?
O2= -2 S= +4
What are the oxidation states of each atom in CO3^2-?
O= -2 C= +4
What is the oxidation state of each atom in N2O5?
O= -2 N= +5
Hydroxide
OH-
Os
Osmium
O
Oxygen
Compound X has a molar mass of 416.41 grams per mol and the following composition: Phosphorus-14.88% Chlorine-85.12% Find molecular formula
P2Cl10
Compound X has a molar mass of 283.89 grams per mol and the following composition: Phosphorus-43.64% Oxygen-56.36% Write molecular formula
P4O10
Compound X has a molar mass of 316.25 grams per mol and the following composition: Phosphorus-38.18% Sulfur-60.82% Write the molecular formula
P4S6
phosphite
PO3 (3-)
Phosphate
PO4 (3-)
Pd
Palladium
Write the molecular equation for the reaction that occurs when aqueous solutions of lead acetate (Pb(C2H3O2)2) and calcium chloride (CaCl2) are combined
Pb(C2H3O2)2 (aq) + CaCl2 (aq) ----> PbCl2 (s) + Ca (C2H3O2)2 (aq)
Write the complete ionic equation for the reaction that occurs when aqueous solutions of lead acetate (Pb(C2H3O2)2) and calcium chloride (CaCl2) are combined
Pb^2+ (aq) + 2C2H3O2^- (aq) + Ca^2+ (aq) + 2Cl^- (aq) ----> PbCl2 (s) + Ca^2+ (aq) + 2C2H3O2 (aq)
Write the net ionic equation for the reaction that occurs when aqueous solutions of lead acetate (Pb(C2H3O2)2) and calcium chloride (CaCl2) are combined
Pb^2+ (aq) + 2Cl^- (aq) ---> PbCl2 (s)
What is percent yield?
Percent the actual yield is of the theoretical yield
P
Phosphorus
Pt
Platinum
Pu
Plutonium
Po
Polonium
K
Potassium
Pr
Praseodymium
What is ionization?
Process by which a molecular compound forms ions when it dissolves
What are weak electrolytes?
Produces ions upon dissolving but exists in solution predominantly as molecules, weak acids and weak bases
Pm
Promethium
Pa
Protactinium
What is a Bronsted base?
Proton acceptor
What is a Bronsted acid?
Proton donor
Ra
Radium
Rn
Radon
rubidium hydroxide
RbOH
What is a chemical reaction?
Rearrangement of atoms in a sample of matter
Re
Rhenium
Rh
Rhodium
Rg
Roentgenium
Rb
Rubidium
Rf
Rutherfordium
What is the symbol for a solid?
S
Sulfate
SO4 (2-)
Sm
Samarium
Sc
Scandium
Sg
Seaborgium
Se
Selenium
Si
Silicone
Ag
Silver
The following chemical reaction takes place in aqueous solution: SnSO4 (aq) + K2S(aq) ---> SnS(s) + K2SO4 (aq) Write the net ionic equation
Sn^2+ (aq) _ S^2- (aq) ---> SnS (s)
Is K2CO3 soluble or insoluble?
Soluble
strontium hydroxide
Sr(OH)₂
Identify sulfuric acid A. strong electrolyte, weak acid B. weak electrolyte, weak acid C. strong electrolyte D. weak electrolyte E. nonelectrolyte
Strong electrolyte
Is sodium hydroxide a non-electrolyte, a weak electrolyte or a strong electrolyte?
Strong electrolyte
Sr
Strontium
What is a solvent?
Substance present in largest amount
What is a solute?
Substance present in smaller amount
What are electrolytes?
Substance that dissolves in water to yield a solution that conducts electricity
What are nonelectrolytes?
Substance that dissolves in water to yield a solution that doesn't conduct electricity
S
Sulfur
Ta
Tantalum
Tc
Technetium
Te
Tellurium
Tb
Terbium
Tl
Thallium
What is actual yield?
The amount of product actually obtained from a reaction
What is theoretical yield?
The amount of product that forms when all the limiting reactant reacts to form the desired product
What is a product?
The elements or compounds produced by a chemical reaction
What is molar mass?
The mass of one mole of a substance
What is a mole?
The number of atoms in 12 grams of carbon-12
What is Avogadro's number?
The number of atoms in 12g of carbon-12
What is molarity?
The number of moles of solute per liter of solution
What is dissociation?
The process in which an ionic compound separates into ions as it dissolves
What is dilution?
The process of lowering the concentration of a solution by adding more solvent
What is the excess reactant?
The reactant that is left over
What is a limiting reactant?
The reactant that runs out first
What is molecular mass?
The sum of the atomic masses of all the atoms in a molecule
What is formula mass?
The sum of the average atomic masses of all atoms represented in its formula
Th
Thorium
Tm
Thullium
Sn
Tin
Ti
Titanium
How do you convert between moles and particles?
To convert from moles to atoms multiply the molar amount by avogadro's number. To convert from atoms to moles divide the atom amount by avogadro's number
How do you convert between mass and moles?
To convert mass to moles divide the amount of grams by its molar mass, to convert moles to mass multiply the amount of moles by its molar mass
What is a redox reaction?
Transfer of one or more electrons from one reactant to another
W
Tungsten
What is a combination reaction?
Two or more reactants combine to form a single product
U
Uranium
How do you find the empirical formula from the percent composition?
Use experimentally determined percent composition to determine empirical formula
Is ethylamine a non-electrolyte, a weak electrolyte or a strong electrolyte?
Weak electrolyte
Identify acetic acid. A) strong electrolyte, weak acid B) weak electrolyte, weak acid C) strong electrolyte, strong acid D) weak electrolyte, strong acid E) nonelectrolyte
Weak electrolyte, weak acid
What is hydration?
When an ionic substance dissolves in water, the molecules remove individual ions from the solid structure and surround them
What is a decomposition reaction?
When something is broken down into smaller molecules
What is a precipitation reaction?
Where two solutions react and an insoluble solid forms in the solution
What is a reducing agent?
Whichever product is oxidized
What is oxidizing agent?
Whichever product is reduced
Xe
Xenon
Does a precipitate form from silver nitrate and potassium chloride? If so, what is the empirical formula?
Yes. AgCl
Is the below equation a redox reaction? If so, what is the reducing agent and oxidizing agent? C (s) + O2 (g) ---> CO2 (g)
Yes. C is the reducing agent and O2 is the oxidizing agent
Is the below equation a redox reaction? If so, what is the reducing agent and oxidizing agent? 3O2 (g) + 4Fe (s) ---> 2Fe2O3 (s)
Yes. Fe is the reducing agent and O is the oxidizing agent
Does a precipitate form from zinc chloride and ammonium sulfide? If so, what is the empirical formula?
Yes. ZnS
Y
Yttrium
Zn
Zinc
Zr
Zirconium
What is the symbol for gas?
g
What is the symbol for liquid?
l
Which term identifies the minority component of the solution? A. limiting reactant B. excess reactant C. solute D. solvent E. molarity
solute
What is an equivalence point?
the point in a titration where the acid has been completely neutralized
