Question :
41) At a given temperature, K = 46.0 for the : 1282448
41) At a given temperature, K = 46.0 for the reaction
4 HCl (g) + O2 (g) 2 H2O (g) + 2 Cl2 (g)
At equilibrium, [HCl] = 0.150, [O2] = 0.395, and [H2O] = 0.625. What is the concentration of [Cl2] at equilibrium?
A) 1.26 M
B) 0.00653 M
C) 0.153 M
D) 0.438 M
42) If the K eq = 2.2 x 1012 then which of the following statements is true?
A) mostly products are present
B) mostly reactants are present
C) some of both reactants and products are present
D) none of the above
43) If the K eq = 5.6 x 10-10 then which of the following statements is true?
A) mostly products are present
B) mostly reactants are present
C) some of both reactants and products are present
D) none of the above
44) Sulfur combines with hydrogen to form hydrogen sulfide, a toxic gas that is a product of decay of organic material.
S (g) + H2 (g) H2S (g) K eq = 2.8 x 10-21
Which of the following statements is true concerning the equilibrium system?
A) Increasing the volume of the sealed reaction container would shift the equilibrium to the right.
B) Decreasing the concentration of H2 would shift the equilibrium to the right.
C) Decreasing the concentration of H2S would shift the equilibrium to the left.
D) Very little hydrogen sulfide gas is present in the equilibrium.
45) Hydrogen gas reacts with iron(III) oxide and produces iron metal which can be used to produce steel according to the reaction below. Choose the response that is incorrect concerning the equilibrium system.
Fe2O3 (s) + 3 H2 (g) + heat 2 Fe (s) + 3 H2O (g)
A) Lowering the reaction temperature will increase the concentration of hydrogen gas.
B) Increasing the pressure on the reaction chamber favors the formation of products.
C) Continually removing water from the reaction chamber increases the yield of iron.
D) Decreasing the volume of hydrogen gas will reduce the yield of iron.
46) CO2 and H2 are allowed to react until an equilibrium is established as follows:
CO2 (g) + H2 (g) H2O (g) + CO (g)
What will be the effect on the equilibrium after adding H2O to the equilibrium mixture?
A) The equilibrium will shift to the left.
B) H2 concentration will decrease and CO2 concentration will increase.
C) CO and CO2 concentrations will increase.
D) H2 concentration will decrease and H2O concentration will increase.
47) According to Le Chatelier’s principle, which of the following changes will shift to the left the position of the equilibrium to the left of the following reaction?
N2 (g) + 3 H2 (g) 2 NH3 (g) + Heat
A) Increase the concentration of N2.
B) Decrease the pressure on the system.
C) Decrease the temperature.
D) Increase the concentration of H2.
48) In which of the following equilibrium systems will the equilibrium shift to the left when the pressure of the system is increased?
A) N2 (g) + 3 H2 (g) 2 NH3 (g)
B) 4 NH3 (g) + 5 O2 (g) 4 NO (g) + 6 H2O (g)
C) 2 SO2 (g) + O2 (g) 2 SO3 (g)
D) H2 (g) + Cl2 (g) 2 HCl (g)
49) In which of the following reactions that are at equilibrium will a shift to the left occur when the pressure is decreased?
A) 2 HCl (g) H2 (g) + Cl2 (g)
B) 2 SO3 (g) 2 SO2 (g) + O2 (g)
C) N2 (g) + 3 H2 (g) 2 NH3 (g)
D) N2O4 (g) 2 NO2 (g)
50) The following reaction is exothermic. Which of the following will drive the reaction to the right (towards products)?
CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)
A) a decrease in temperature
B) an increase in temperature
C) the removal of CH4
D) the addition of CO2
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LeoSteve
