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Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g);...

Consider this reaction between solid carbon and carbon dioxide gas. C(s) + CO2(g) ⇌ 2 CO(g); ΔH = +172.5 kJ/mol Please explain the following: When chemical systems are subjected to stresses, the equilibrium position may shift toward the reactants or products, or it may be unaffected. How would each of the following changes affect this equilibrium? 1. decreasing the temp 2. increasing the CO2 3. increasing the volume of the container 4. adding C 5. adding a catlyst Options: Would #'s 1-5... a. shift the reaction towards the reactants, shift the reaction towards the products, or would the change not have any effect on the reaction at all?

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queen_honey_blossom answered 2 years ago
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