QUESTION 10 The questions that follow are based on the reaction at equilibrium: C(s) + CO2(g) = 2C0(g) AH° = +172.5 kJ/mol What would be the effect on the preceding reaction of decreasing the volume to one-half its original value? The reaction would proceed to the reactant side. The position of the equilibrium would not change. The reaction would proceed to the product side. Additional information is needed to answer the question. 0000
QUESTION 10 The questions that follow are based on the reaction at equilibrium: C(s) + CO2(g) = 2C0(g) AH° = +172.5 kJ/mol What would be the effect on the preceding reaction of decreasing the volume to one-half its original value? The reaction would proceed to the reactant side. The position of the equilibrium would not change. The reaction would proceed to the product side. Additional information is needed to answer the question. 0000
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Chapter1: Chemical Foundations
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Transcribed Image Text:QUESTION 10
The questions that follow are based on the reaction at equilibrium:
C(s) + CO2(g)=2C0(g) AH° = +172.5 kJ/mol
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What would be the effect on the preceding reaction of decreasing the volume to one-half its original value?
O The reaction would proceed to the reactant side.
The position of the equilibrium would not change.
The reaction would proceed to the product side.
Additional information is needed to answer the question.
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Expert Solution
Step 1
When there is a decrease in volume, the equilibrium will shift to favor the direction that produces fewer moles of gas. When there is an increase in volume, the equilibrium will shift to favor the direction that produces more moles of gas.
For example, if the pressure in a system increases, or the volume decreases, the equilibrium will shift to favor the side of the reaction that involves fewer moles of gas.
So in the given reaction the number of gaseous product is greater than reactant. So with decreasing volume the equilibrium shifted to the more moles side
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