11. Consider the reaction, SnO2(s) + 2 CO(g) Sn(s) + 2CO2(g), at t = 500°C, where the reaction has an equilibrium constant K = 0.025. With the system at equilibrium, if the amount of Sn(s) is doubled, the partial pressure of CO(g) will A) increase. B) decrease. C) remain unchanged. D) change unpredictably. E) none of these

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Chapter1: Chemical Foundations
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reaction
A) will proceed by forming additional SO2(g) and O2(g).
B) will proceed by forming additional SO3(g).
C) is at equilibrium.
D) The direction of the reaction cannot be predicted from these data.
E) None of these is correct.
11. Consider the reaction, SnO2(s) + 2 CO(g) Sn(s) + 2CO2(g), at t= 500°C, where the
reaction has an equilibrium constant K = 0.025. With the system at equilibrium, if the amount of
Sn(s) is doubled, the partial pressure of CO(g) will
A) increase.
B) decrease.
C) remain unchanged.
D) change unpredictably.
E) none of these
500 ml of
12. When would the Kp and Ke for a reaction have the same value?
A) At low temperatures
ssures
Transcribed Image Text:reaction A) will proceed by forming additional SO2(g) and O2(g). B) will proceed by forming additional SO3(g). C) is at equilibrium. D) The direction of the reaction cannot be predicted from these data. E) None of these is correct. 11. Consider the reaction, SnO2(s) + 2 CO(g) Sn(s) + 2CO2(g), at t= 500°C, where the reaction has an equilibrium constant K = 0.025. With the system at equilibrium, if the amount of Sn(s) is doubled, the partial pressure of CO(g) will A) increase. B) decrease. C) remain unchanged. D) change unpredictably. E) none of these 500 ml of 12. When would the Kp and Ke for a reaction have the same value? A) At low temperatures ssures
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