chemistry final
What is the pressure today in atm if the weatherman says the current pressure today is 742 torr? 0.962 atm 18 atm 1.02 atm 1.00 atm 0.976 atm
0.976
How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H5 + 5 O2 → 3 CO2 + 4 H2O 1.5 3.0 5.0 6.0 18
1.5
How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H5 + 5 O2 → 3 CO2 + 4 H2O 6.0 3.0 5.0 1.5 18
1.5
What is the molarity of a solution prepared by dissolving 0.750 mol CaCl2 in enough water to make 0.500 L of solution 0.375 M 0.667 M 1.50 M 83.2 M 166.5 M
1.50 M
An imaginary element X consists of two isotopes having masses of 141.0 amu and 143.0 amu. A sample of X was found to contain 20.0% of the 141X isotope and 80.0% of the 143X. Calculate the atomic weight of X 141.2 amu 141.4 amu 142.0 amu 142.6 amu 143.0 amu
142.6 amu
How many mL of 0.360 M HNO3 are needed to neutralize a 22.5 mL sample of 0.240 M KOH 5.40 mL 15.0 mL 22.5 mL 33.8 mL 62.5 mL
15.0 mL
Atoms of a 35/17 Cl contain _____ protons and _____ electrons 17; 17 17; 18 18; 17 35; 18 35; 17
17; 17
How many grams of NaOH are needed to make 750 mL of a 2.5% (w/v) solution? 3.9 g 7.5 g 19 g 20 g 50 g
19 g
The number of grams in 7.00 moles of N2 is 4.21 x 10^24 14.0 28.0 98.0 196
196
What is the electron configuration of S? 1s2 2s2 2p2 1s2 2s2 2p6 3s2 3p2 1s2 2s2 2p6 3s2 3p4 1s2 2s2 2p6 3s2 3p6 1s2 2s2 2p6 3s2 3p6 4s2 3d1
1s2 2s2 2p6 3s2 3p4
Which of the following pH's corresponds to a strongly acidic solution? 11.5 2.1 6.9 7.4 4.3
2.1
In the reaction 2 C + O2 → 2 CO, how many moles of carbon are needed to produce 66.0 g of carbon monoxide? 0.424 1.18 2.36 4.71 28.3
2.36
How many moles of NaHCO3 are present in a 2.00 g sample? 2.38 x 10^-2 mol 1.27 x 10^-2 mol 2.00 mol 85.0 mol 168 mol
2.38 x 10^-2 mol
If the concentration of H3O+ is 3.5 x 10-3 M, the concentration of OH- is _____ M 2.9 x 10^-12 1.0 x 10^-12 1.0 x 10^-7 3.5 x 10^-11 10.5 x 10^-3
2.9 x 10^-12
In a reaction to produce chlorine gas, the theoretical yield is 25.6g. What is the actual yield of the reaction if the percent yield is 83.5%? 214 g 21.4 g 3.26 g 0.0326 g 2.56 g
21.4 g
How many mL of 16 M NH3 are needed to prepare 2.00 L of a 2.00 M solution 250 mL 125 mL 16 mL 8.0 mL 4.0 mL
250 mL
When the reaction shown is correctly balanced, the coefficients are: ___ HBr + ___Ca(OH)2 → ___CaBr2 + ___H2O 2; 1; 1; 1 1; 1; 1; 2 2; 1; 1; 2 2; 2; 1; 1 2; 1; 2; 2
2; 1; 1; 2
Consider the balanced equation shown and identify the statement that is not true Na2SO4(aq) + BaCl2(aq) → 2 NaCl(aq) + BaSO4(s) The coefficient of sodium sulfate is one Barium sulfate is produced in solid form Barium chloride is dissolved in water The products are barium sulfate and sodium chloride 2NaCl (aq) could also be correctly written as Na2Cl2 (aq)
2NaCl (aq) could also be correctly written as Na2Cl2 (aq)
What is the density of a substance with a volume of V=26.2 cm3 and a mass of 94.9 g?? 3.62 cm3/g 3.62 g3/cm 3.62 g/cm3 0.276 cm3/g 0.276 cm/g3
3.62 g/cm3
Which measurement represents the smallest quantity? 3740 nm 3.74 x 10-4 m 3.74 x 10^3 um 3.74 x 10-6 km 37.4 nm
3740 nm
The [H3O+] in a solution with pH = 6.35 is 7.65 M 6.35 M 4.5 x 10^-7 M 0.80 M 2.2 x 10^-8 M
4.5 x 10^-7 M
A sample of gas has a volume of 135 mL at 0.600 atm. What would be the volume if the pressure is decreased to 0.200 atm while temperature is held constant? 45.0 mL 180 mL 135 mL 405 mL 101 mL
405 mL
How many mL of 0.105 M AgNO3 are needed for an experiment that requires 0.00510 mol of AgNO3? 0.536 mL 17.8 mL 18.70 mL 20.6 mL 48.6 mL
48.6 mL
A sample of helium has a volume of 480 mL at 47.0 oC and 740 mm Hg. The temperature is lowered to 22.0 oC and the pressure to 625 mm Hg. what is the new volume? 616 mL 373 mL 266 mL 524 mL 1214 mL
524 mL
The molar mass of butane, C4H10, is _____ grams 22.01 49.05 52.08 58.12 68.24
58.12
How many electrons can occupy the 2p subshell? 1 2 6 8 10
6
Find the difference between two masses measured as 146.5 grams and 139.983 grams. Express the answer to the correct number of significant figures 6.5 grams 6.51 grams 6.517 grams 7.0 grams 7 grams
6.5 grams
A thimble of water contains 4.0 x 10^21 molecules. The number of moles of H2O is 2.4 x 10^45 6.6 x 10^-3 6.6 x 10^-23 2.4 x 10^23 2.4 x 10^-23
6.6 x 10^-3
Calculate the equilibrium constant for the reaction below if a tank was found to contain 0.355 M CO, 0.180 M O2m and 1,21 M CO2 2 CO(g) + O2 (g) → 2 CO2 (g) 5.23 x 10-2 1.55 x 10-2 18.9 64.5 22.9
64.5
Consider the reaction shown N2 + O2 → 2 NO ∆H = +43.2 kcal When 50.0 g of N2 react, _____ kcal will be _____ 2160; produced 2160; consumed 77.1; produced 77.1 consumed 43.2; produced
77.1; produced
What is 0.0970 written in scientific notation 970 x 10-4 97 x 10-3 9.7 x 10-2 97.0 x 10-2 0.97 x 10-1
9.7 x 10-2
Calculate the volume of a 3.50 mol sample of carbon dioxide at 35.0 oC and 0.900 atm 96.5 L 421 L 2.20 L 8.54 x 10-4 L 9.58 L
96.5 L
Which statement about solubility is not true? The solubility of gases decreases with increasing temperature The solubility of gases increases with increasing pressure The solubility of solids may increase or decrease with increasing temperature In a saturated solution, an equilibrium exists between dissolved and undissolved solute Additional solute added to a saturated solution will fully dissolve
Additional solute added to a saturated solution will fully dissolve
In the reaction below, the conjugate acid of CH3OO- is CH3COO- + H2CO3 → CH3OOH + HCO3- CH3COO- H2CO3 CH3COOH HCO3- H3O+
CH3COOH
What is the formula for the ionic compound formed between calcium and nitrate? Ca3N2 CaNO3 Ca2NO3 Ca(NO3)2 Ca2NO2
Ca(NO3)2
Identify the reactant(s) in the following equation Calcium carbonate → calcium oxide + carbon dioxide Calcium carbonate Calcium oxide + carbon dioxide Calcium carbonate + calcium oxide Carbon dioxide + calcium carbonate Calcium carbonate + calcium oxide + carbon dioxide
Calcium carbonate
The name of Cl- Chlorine ion Chloride ion Chlorate ion Chlorite ion Diatomic chlorine
Chloride ion
Which of the following is a non-metal Li Mg Cu Zn Cl
Cl
Which of the following is a non-metal? Li Mg Cu Zn Cl
Cl
Table salt (NaCl) is a(n) _____ and is found in the ____ phase Element; liquid Compound; solid Mixture; liquid Compound; gas Mixture; solid
Compound; solid
Adding one neutron to the nucleus of an atom Converts it to an isotope of the same element Converts it to an atom of a different element Increases its atomic number by one Increases its mass number by one Converts it to an ion with a positive charge
Converts it to an isotope of the same element
In the reaction shown, _____ is oxidized and becomes _____ Ni(s) + CuCl2(aq) → Cu(s) + NiCl2(aq) Ni; Ni+ Ni; Ni2+ Cu2+; Cu Cu+; Cu Cl; Cl-
Cu2+; Cu
Xylene, a compound with the formula C8H10, is composed of Any combination of atoms of carbon and hydrogen in a four to five ratio Eight atoms of carbon and ten atoms of hydrogen Eight atoms of calcium and ten atoms of helium Ten atoms of carbon and eight atoms of hydrogen Any combination of atoms of carbon and hydrogen that add up to 18
Eight atoms of carbon and ten atoms of hydrogen
Main group elements that are non-metals usually ____ one or more electrons to form ____, which have a _____ charge. Lose; anion; negative Lose; cation; negative Lose; cations; positive Gain; cations; positive Gain; anions; negative
Gain; anion; negative
What is they typical net ionic equation for an acid-base neutralization of KOH and HCl? HCl(aq) + KOH(aq) → H2O(l) + KCl(aq) KOH(aq) → K+(aq) + OH-(aq) H2O(l) → H+(aq) + OH-(aq) K+(aq) + OH-(aq) → KOH(aq) H+(aq) + OH-(aq) → H2O(l)
H+(aq) + OH-(aq) → H2O(l)
Rank the following in increasing order of boiling point: H2, NH3, CCl4, H2Se H2< CCl4<NH3<H2Se NH3<H2Se<H2<CCl4 NH3<H2Se<CCl4<H2 H2<CCl4<H2Se<NH3 H2Se<NH3<H2<CCl4
H2<CCl4<H2Se<NH3
Which reaction is an example of an acid-base reaction? H2CO3(aq) → H2O(l) + CO2(g) H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O 6 HCl(aq) + 2 Al(s) → 2 AlCl3(aq) + 3 H2(g) FeCl3(aq) + 3 KOH(aq) →Fe(OH)3(s) + 3 KCl(aq) 2 Hg(l) + O2(g) → 2 HgO(s)
H2SO4(aq) + Ca(OH)2(aq) → CaSO4(aq) + 2 H2O
Which of the following is the strongest acid? HCN (Ka = 4.9 x 10^-10) H2CO3 (Ka = 4.3 x 10^-7) HF (Ka = 3.5 x 10^-4) H3PO4 (Ka = 7.5 x 10^-3) Acid strength cannot be determined from the given information
H3PO4 (Ka = 7.5 x 10^-3)
Which element is most likely to have chemical properties similar to those of bromine? S Se Kr K I
I
According to Avogadro's Law, the volume of a gas will ____ as the ____ is increased while the ___ are held constant Increase; temperature; pressure and number of moles Increase; number of moles; pressure and temperature Increase; pressure; temperature and number of moles Decrease; pressure; temperature and number of moles Decrease; number of moles; pressure and temperature
Increase; number of moles; pressure and temperature
Which of the following is not soluble in water Potassium sulfide Iron (II) bromide Iron (III) hydroxide Iron (III) nitrate Ammonium sulfate
Iron(III) hydroxide
Which pair of elements is most likely to form an ionic compound if allowed to react together? Na and Al Fe and Ca C and F K and Br H and N
K and Br
The spectator ions in the reaction shown are 2 AgNO3(aq) + K2SO4(aq) → 2 KNO3(aq) + Ag2SO4(s) Ag+ and NO3- K+ and SO42- K+ and NO3- Ag+ and SO42- H+ and OH-
K+ and NO3-
Which one of the following will act as a strong electrolyte in an aqueous solution? KNO3 CH3OH CCl4 NH3 Glucose
KNO3
Which of the following is a strong base? HNO3 H3PO4 NH3 KOH H2O
KOH
Which symbol does not denote a compound? NH3 HBr Kr Na2S LiF
Kr
Which of the following elements is most likely to form an ion with a +2 charge? Mg Si S K Ti
Mg
The following equation represents the formation of nitrogen dioxide, a major component of smog, 2 NO + O2 → 2 NO2 If 0.68 mole of NO is reacted with 0.79 mole of O2 to produce NO2, the limiting reactant is Both NO and O2 NO O2 NO2 None of the above
NO
Of the following four substances, which would form a basic solution when dissolved in water: NH4Cl, Ba(NO3)2, K2CO3, NaF NH4Cl, Ba(NO3)2 K2CO3, NH4Cl NaF, K2CO3 NaF only None of them
NaF, K2CO3
Which of the following would be miscible with carbon tetrafluoride, CF4? H2O NaOH NH3 O2 CaF2
O2
Which of the following structures is likely to exist SH3 HBr4 CH20 OH2Cl2 None of the above
OH2CL2
Which of the following is an example of a molecular solid? Pd(s) CaF2(s) PCl5(s) K2S(s) Sr(s)
PCl5 (s)
Which of the following compounds can be most accurately described as a covalent molecule? AlF3 NaF CaF2 PF3 AgF
PF3
What is the formula of the phosphate ion? PO3- PO32- PO42- PO43- P3-
PO43-
Consider the pyramidal molecule NH3, in which the central atom has one lone pair of electrons. The electronegativities of H and N are 2.1 and 3.0, respectively. Based on these values and on consideration of molecular geometry, the H-N bond is _____ and the molecule is _____ 0 - 0.4 = non-polar covalent 0.5 - 1.9 = polar covalent 2.0 and above = ionic Polar; polar Nonpolar; nonpolar Polar; nonpolar Nonpolar; polar None of the above
Polar: polar
Protons possess a _____ charge, and neutrons possess a _____ charge. Negative; negative Negative; positive Positive; negative Positive; zero Zero; positive
Positive; zero
Which of the following conditions characterizes a system in a state of chemical equilibrium? Concentrations of reactants and products are equal Rate of forward reaction has dropped to zero Reactants are being consumed at the same rate they are being produced Reactants molecules no longer react with each other Product concentrations are greater than reactant concentrations
Reactants are being consumed at the same rate they are being produced
Which of the following conditions characterizes a system in a state of chemical equilibrium? Concentrations of reactatns and products are equal Rate of forward reaction has dropped to zero Product concentrations are greater than reactant concentrations Reactant molecules no longer react with each other Reactants are being consumed at the same rate they are being produced
Reactants are being consumed at the same rate they are being produced
Which statement about the system is not true? 2 SO2(g) + O2 (g) → 2 SO3 (g) + heat K = 4.8 x 1027 Removing O2 will cause an increase in the amount of SO3 At equilibrium, SO3 is the predominant substance Heating the system will cause a decrease in the amount of SO3 The large value of K means that the reaction essentially goes to completion Adding SO2 will cause an increase in the amount of SO3
Removing O2 will cause an increase in the amount of SO3
The classification of an acid or a base as weak or strong is determined by The solubility of the acid or base The extent of dissociation of the dissolved acid or base The concentrations of the acid or base The corrosiveness of the acid or base None of the above
The extent of dissociation of the dissolved acid or base
In forming covalent bonds where the octet rule is obeyed, oxygen usually forms _____ bonds and fluorine usually forms _____ bonds. One, one Two, two One, two Two, one Six, seven
Two, one
Which description best fits a gas? Definite volume; shape of container; moderate intermolecular attractions Volume and shape of container; no intermolecular attractions Definite volume; shape of container;weak intermolecular attractions Volume and shape of container; strong intermolecular attraction Definite shape and volume; strong intermolecular attractions
Volume and shape of container; no intermolecular attractions
Write the equilibrium expression for the following reaction: 2 BrF5(g) → Br2(g) + 5F2 (g) [Br2][F2] / [BrF5] [Br2][F2]^5 / [BrF5]^2 [BrF5]^2 / [Br2][F2]^5 2[BrF5] / [Br2] 5[F2] [BrF5] / [Br2][F2]
[Br2][F2]^5 / [BrF5]^2
Which of the following contains potential energy? A kid jumping rope Flowing water A book on a table A person riding a bike A bouncing ball
a book on a table
A necessary requirement for a Brosted-Lowry base is The presence fo water as a reaction medium The presence of hydroxide in its formula A lone pair of electrons in its Lewis dot structure The production of hydronium ion upon reaction with water The presence of a metal ion in its formula
a lone pair of electrons in its Lewis Dot Structure
Adding solute to a solution will increase which of the following Boiling point Freezing point Osmotic pressure Both A and B Both A and C
both A and C
Water can be used to dissolve which type of compound? Nonpolar compounds Polar compounds Ionic compounds Both A and B Both B and C
both B and C
When a liquid sample is taken from sea level to a higher elevation, what happens to the external (atmospheric) pressure on the liquid and the boiling point of the liquid? Both decrease Pressure goes up but boiling point goes down Both increase Pressure goes up but the boiling point remains unchanged Pressure goes down but boiling point goes up
both increase
All of the statements regarding "∆H" are correct except it Can be called the enthalpy change Can be called the heat of reaction Represents the difference between the energy used in breaking bonds and the energy released in forming bonds in a chemical reacion Has a negative value for an exothermic reaction Can be called the entropy change
can be called the entropy change
A positively charged particle formed by the loss of one or more electrons from an atom is called a(n) Anion Cation Isotope Nucleus Proton
cation
Which change to the system below would cause equilibrium to shift to the right? 4 NH3(g) + 3 O2 (g) → 2 N2 (g) + 6 H2O (g) ∆H = -1531 kJ Adding heat to the system Decreasing the reaction temperature Adding nitrogen to the equilibrium mixture Decreasing the concentration of oxygen Increasing the total pressure
decreasing the ratio temperature
In the reaction A + B → AB, which of the following will not increase the rate Adding A Adding a catalyst Adding B Increasing the temperature Decreasing the temperature
decreasing the temperature
In the reaction energy diagrams shown below, the reaction on the left is ___, and it occurs ____ the reaction on the right Exergonic; at the same rate as Endergonic; faster than Exergonic; faster than Endergonic; slower than Exergonic; slower than
exergonic; faster than
The amount of energy involved in melting a substance without changing its temperature is called the Joule Calorie Heat of vaporization Heat of combustion Heat of fusion
heat of fusion
What are the strongest intermolecular forces between C5H12 molecules London dispersion forces Ion-dipole Ionic bonds Hydrogen bonding Dipole-dipole
london dispersion forces
Which group contains only elements which normally exist as diatomic molecules Nitrogen, sulfur, bromine Helium, neon, argon Nitrogen, oxygen, fluorine Hydrogen, lithium, sodium Oxygen, phosphorus, germanium
nitrogen, oxygen, flourine
During the hydrolysis of water to form hydrogen and oxygen gases, there is an increase in entropy. This means the sign of ∆S is _____, and the randomness of the system ____ Positive; increases Undetermined; increases Negative; decreases Positive; decreases Negative; increases
positive; increase
For the process of vaporization, the sign of ∆H is _____ and the sign of ∆S is _____ Negative; negative None of the above Negative; positive Positive; Negative Positive; positive
positve: positve
A chemical bond formed when two atoms shar one pair of electrons is a _____ bons; it is best described as _____ Double; covalent Double; ionic Single; covalent Single; ionic Triple; covalent
single; covalent
Which of the following can affect the activation energy (Eact) of a reaction? Increase the concentration of reactants Temperature of the reaction Use of a catalyst Increase the concentration of products Surface area of reactants
use of a catalyst
If "A" contains 0.20 M NaCl and is separated by a semipermeable membrane from "B" which contains 1.0 M NaCl, which event will occur? NaCl will flow from "A" to "B" NaCl will flow from "B" to "A" Water will flow from "A" to "B" Water will flow from "B" to "A" None of the above
water will flow from "B" to "A"
Which is not an example of a solution? The mixture of gases in a SCUBA tank An alloy of nickel and copper Carbonated water Whole milk Salt brine used for pickling
whole milk
Although noble gases do not normally form covalent compounds, XeO3 has been prepared. The systematic name of this compound is Trioxy xenon Trixenon trioxide Xenon trioxide Xenon (III) oxide None of the above
xenon trioxide
Which solution has the greatest osmolarity 0.1 M NaCl 0.1 M AlCl3 0.1 M KF 0.1 M CaBr2 0.1 M KNO3
0.1 M AlCl2
A molecule in which the central atom forms two single bonds and has two lone pairs is said to have a _____ shape Bent Linear Planar Pyramidal Tetrahedral
bent
In a precipitation reaction the precipitate can be identified by the symbol (aq) (l) (g) (s) None of the above
(s)
Which of the following measurements has three significant figures? 1207 g 4.250 g 0.006 g 0.0250 g 0.03750 g
0.0250 g
The [OH-] and the pOH of 0.035 M KOH are respectively 0.035 M and 1.46 0.035 M and 12.54 2.9 x 10^-13 M and 1.46 2.9 x 10^-13 M and 9.59 2.9 x 10^-13 M and 12.54
0.035 M and 1.46
An increase in solution pH corresponds to An increase in hydronium ion concentration A decrease in hydronium ion concentration An increase in hydroxide ion concentration Both A and C Both B and C
an increase in hydronium ion concentration
