Chapter 08
Chapter 09
Chapter 10
100
Write a balanced combustion reaction for n-propene, C3H6. How many molecules of O2 are required to combust six (6) molecules of n-propene?
A. 27
B. 18
C. 12
D. 9
A. 27
100
You find a penny (minted before 1982, when pennies were almost entirely copper) in the snow. How much heat is absorbed by the penny as it warms from the temperature of the snow, which is -8.0 °C, to the temperature of your body, 37.0 °C? Assume the penny is pure copper and has a mass of 3.10 g.
A. 34.6 J
B. 44.2 J
C. 53.7 J
D. 140 J
C. 53.7 j
100
The pressure exerted on a sample of a fixed amount of gas is doubled at constant temperature, and then the temperature of the gas in kelvins is doubled at constant pressure. What is the final volume of the gas?
a) The final volume of the gas is twice the initial volume.
b)The final volume of the gas is four times the initial volume.
c) The final volume of the gas is one-half the initial volume.
d) The final volume of the gas is one-fourth the initial volume.
e) The final volume of the gas is the same as the initial volume.
c) The final volume of the gas is one-half the initial volume.
200
Which of the following reactions is not a redox reaction?
A. H2(g) + Cl2(g) → 2 HCl(g)
B. 4 Al(s) + 3 O2(g) → 2 Al2O3(s)
C. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
D. 2 K2S(g) + 3 O2(g) → 2 K2O(s) + 2 SO2(g)
E. Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g)
C. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
200
Consider the following chemical equation:
What is Hrxn for the reaction 2 C — > 4 A + 2 B?
- 122 J
- -122 J
- 244 J
- -244 J
4. -224 J
200
Choose the best description as to how one could make a sample of H2(g) effuse at the same rate as Cl2(g).
A. Keep equimolar samples of H2 and Cl2 at the same temperature to ensure equal probability of effusion.
B. Keep the H2 sample at a significantly lower temperature than that of the Cl2 sample.
C. Keep the H2 sample at a significantly higher temperature than that of the Cl2 sample.
D. Keep the H2 sample at a significantly higher partial pressure than the Cl2 sample.
B. Keep the H2 sample at a significantly lower temperature than that of the Cl2 sample.
300
What reaction type best characterizes the following chemical reaction?
HNO3(aq) + NaHCO3(aq) → CO2(g) + NaNO3(aq) + H2O(l)
A. Acid-base
B. Redox
C. Combustion
D. Precipitation
A. Acid-base
300
When 1.010 g of sucrose (C,2H22°, ) undergoes combustion in a bomb calorimeter, the temperature rises from 24.92 °C to 28.33 °C. Find AE,n for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 4.90 kJ/°C.
(You can ignore the heat capacity of the small sample of sucrose because it is negligible compared to the heat capacity of the calorimeter.)
A. -5.66 x 10^3 kJ/mol
B. -16.7 kJ/mol
C. -3.41 x 10^3 kJ/mol
D. -5.72 x 10^3 kJ/mol
A. -5.66 x 10^3 kJ/mol
300
A container holds equal masses of CO2 and O2. Assume the container and its gases are at 25.0 °C. Which of the following statements is true?
A. The O2 molecules exert a higher partial pressure than the CO2 molecules.
B. The O2 molecules have a higher average kinetic energy than the CO2 molecules.
C. The CO2 molecules have a higher frequency of collisions with the container wall, compared to the O2 molecules.
D. The O2 molecules and the CO2 molecules exert equal partial pressures.
A. The O2 molecules exert a higher partial pressure than the CO2 molecules.
400
A 0.74 g sample of Ca(OH)2 requires 25.0 mL of aqueous HCl to react completely. What is the concentration of the HCl?
A. 1.0 × 10⁻³ M
B. 0.020 M
C. 0.40 M
D. 0.80 M
D. 0.80 M
400
Calculate ΔHrxn for the overall reaction below using the data given.
C6H4(OH)2(s) + H2O2(l) → C6H4O2(s) + 2 H2O(l) ΔHrxn = ?
Given Data:
a) C6H4O2(s) + H2(g) → C6H4(OH)2(s) ΔH = –177 kJ
b) 2 H2O2(l) → O2(g) + 2 H2O(l) ΔH = –188 kJ
c) 2 H2(g) + O2(g) → 2 H2O(l) ΔH = –572 kJ
A. –937 kJ
B. –583 kJ
C. –561 kJ
D. –365 kJ
E. –203 kJ
E. –203 kJ
400
Equal moles of H2 and Ne gases are combined in a sealed rigid vessel held at a constant temperature. Assume ideal gas conditions apply.
Which one of the following best describes the pressures of each of these gases?
A. The partial pressure of H2 is less than the partial pressure of Ne because the molar mass of H2 is less than the molar mass of Ne.
B. The partial pressure of H2 is greater than the partial pressure of Ne because H2 is a diatomic molecule while Ne is monatomic.
C. The partial pressures of H2 and Ne are equivalent because the volume of the rigid vessel is held constant.
D. The partial pressures of H2 and Ne are equivalent because the number of each gases' constituent particles is equivalent.
D. The partial pressures of H2 and Ne are equivalent because the number of each gases' constituent particles is equivalent.
500
Potassium arsenate has the formula K3AsO4. What would be the name of H3AsO3(aq)?
A. hydroarsenic acid
B. arsenous acid
C. arsenic acid
D. hypoarsenous acid
E. perarsenic acid
B. arsenous acid
500
A piece of titanium, Cs = 0.523 J/g·°C initially at 70.0 °C, is placed in a sample of water, Cs = 4.184 J/g·°C, initially at 50.0 °C. The piece of titanium and sample of water have the same masses. Select a true statement about the water-titanium mixture.
A. The temperature of the water will decrease, and the temperature of the titanium will increase.
B. The final temperature of the mixture will be 60.0 °C once thermal equilibrium has been reached.
C. The amount of heat transferred to the water will be equal to the amount of heat lost by the titanium.
D. The thermal energy of the water will decrease as the system approaches thermal equilibrium.
C. The amount of heat transferred to the water will be equal to the amount of heat lost by the titanium.
500
Choose the best description of the relationship between P and V when the amount of gas and temperature are held constant.
A. P vs. V yields straight line with a negative slope.
B. P vs. V yields a straight line with a positive slope.
C. P vs. 1/V yields a straight line with a negative slope.
D. P vs. 1/V yields a straight line with a positive slope.
D. P vs. 1/V yields a straight line with a positive slope.
600
When 145 mL of 1.20 M NaCl(aq) is added to 355 mL of 0.800 M CaCl2(aq), what is the final chloride ion concentration?
A. 0.742 M
B. 0.788 M
C. 0.916 M
D. 1.48 M
D. 1.48 M
600
Identify each process as endothermic or exothermic and indicate the sign of H.
- sweat evaporating from skin
- water freezing in a freezer
- wood burning in a fire
1. Endothermic
2. Exothermic
3 Exothermic
600
A. 0.852 g/L
B. 1.18 g/L
C. 2.71 g/L
D. 21.4 g/L
A. 0.852 g/L
700
Consider the following two-step process:
P4 + 10 Cl2 → 4 PCl5 6 PCl5 + P4O10 → 10 POCl3
4.00 moles P4 reacts with excess Cl2 producing PCl5 with 60.0% yield. The PCl5 is then isolated and reacted with excess P4O10 to form POCl3 with 80.0% yield. Determine the amount of POCl3 formed.
A. 9.60 mol
B. 12.8 mol
C. 16.0 mol
D. 20.4 mol
E. 26.6 mol
B. 12.8 mol
700
An LP gas tank in a home barbeque contains 13.2 kg of propane, CHg. Calculate the heat (in kJ) associated with the complete combustion of all of the propane in the tank.
C3H8(g) + 5O2(g) → > 3CO2(g) + 4H2O(g)
Hrxn = -2044 kJ
A. -6.12 x 10^5 kJ
B. -5.12 x 10^5 kJ
C. -2.70 x 10^4 kJ
D. -7.41 x 10^5 kJ
A. -6.12 x 10^5 kJ
700
A. 0.209 g
B. 0.449 g
C. 1.12 g
D. 0.0113 g
B) 0.449 g
800
Consider the oxidation of iron to produce iron(III) oxide:
4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)
2.00 mol of Fe is combined with 3.00 mol of O2. If the reaction proceeds with 80.0 % yield, how many moles of Fe2O3 were produced?
A. 2.00 mol
B. 1.60 mol
C. 1.25 mol
D. 1.00 mol
E. 0.800 mol
E. 0.800 mol
800
Consider the following reaction:
Cl2(g) + 3 F2(g) → 2 ClF3(g) ΔH = –810 kJ
Using the data from the reaction above and the following information, estimate the Cl—F bond energy.
Bond : Bond Energy (kJ/mol)
Cl—Cl : 243
F—F : 159
Cl—F : ?
A. 255 kJ/mol
B. 510 kJ/mol
C. 1.53 × 10³ kJ/mol
D. 4.59 × 10³ kJ/mol
A. 255 kJ/mol
800
A. X_He = 0.978, P_He = 11.8 atm; X_O2 = 0.022, P_O2 = 0.264 atm; P_total = 12.1 atm
B. X_He = 0.849, P_He = 10.3 atm; X_O2 = 0.151, P_O2 = 1.83 atm; P_total = 12.1 atm
C. X_He = 0.978, P_He = 14.5 atm; X_O2 = 0.022, P_O2 = 0.326 atm; P_total = 14.8 atm
D. X_He = 0.849, P_He = 11.8 atm; X_O2 = 0.151, P_O2 = 2.10 atm; P_total = 13.9 atm
A. X_He = 0.978, P_He = 11.8 atm; X_O2 = 0.022, P_O2 = 0.264 atm; P_total = 12.1 atm
900
The reaction between sodium phosphate and barium nitrate can be expressed according to the following balanced chemical equation where barium phosphate precipitates:
2 Na3PO4(aq) + 3 Ba(NO3)2(aq) → Ba3(PO4)2(s) + 6 NaNO3(aq)
If 20.0 mL of 0.300 M sodium phosphate is combined with 30.0 mL of 0.100 M barium nitrate, how many moles of the precipitate can be formed? Assume 100% yield.
A. 1.00 × 10⁻³ mol
B. 3.00 × 10⁻³ mol
C. 6.00 × 10⁻³ mol
D. 1.80 × 10⁻² mol
A. 1.00 × 10⁻³ mol
900
A. -463,000 J
B. -3,010 J
C. -441,000 J
D. -19,100 J
A. -463000 J
900
a) 152 m/s
b) 14.0 m/s
c) 482 m/s
d) 234 m/s
c) 482 m/s