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At 25°C, AG° = +31.2 kJ for the reaction, Ag2CO3(s) → Ag20(s) + CO2(g). Is this reaction spontaneous at 25°C and a partial pressure of CO2 gas of 0.10 atm? Explain why or why not. No, it will not be spontaneous, since AG is negative. Yes, it will be spontaneous, since AG is negative. No, it will not be spontaneous, since the reaction is at equilibrium. No, it will not be spontaneous, since AG is positive.

At 25°C, AG° = +31.2 kJ for the reaction, Ag2CO3(s) → Ag20(s) + CO2(g). Is this reaction spontaneous at 25°C and a partial pressure of CO2 gas of 0.10 atm? Explain why or why not. No, it will not be spontaneous, since AG is negative. Yes, it will be spontaneous, since AG is negative. No, it will not be spontaneous, since the reaction is at equilibrium. No, it will not be spontaneous, since AG is positive.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter17: Spontaneity, Entropy, And Free Energy
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Problem 2RQ: What is the second law of thermodynamics? For any process, there are four possible sign combinations...
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At 25°C, AG° = +31.2 kJ for the reaction, %3D Ag2CO3(s) → Ag20(s) + CO2(g). Is this reaction spontaneous at 25°C and a partial pressure of CO2 gas of 0.10 atm? Explain why or why not. No, it will not be spontaneous, since AG is negative. Yes, it will be spontaneous, since AG is negative. No, it will not be spontaneous, since the reaction is at equilibrium. No, it will not be spontaneous, since AG is positive. Yes, it will be spontaneous, since AG is positive. Yes, it will be spontaneous, since AG° is positive. No, it will not be spontaneous, since AG° is positive.
Transcribed Image Text:At 25°C, AG° = +31.2 kJ for the reaction, %3D Ag2CO3(s) → Ag20(s) + CO2(g). Is this reaction spontaneous at 25°C and a partial pressure of CO2 gas of 0.10 atm? Explain why or why not. No, it will not be spontaneous, since AG is negative. Yes, it will be spontaneous, since AG is negative. No, it will not be spontaneous, since the reaction is at equilibrium. No, it will not be spontaneous, since AG is positive. Yes, it will be spontaneous, since AG is positive. Yes, it will be spontaneous, since AG° is positive. No, it will not be spontaneous, since AG° is positive.
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