How is the equilibrium yield of C6H12O6 affected by each of the following? 6 CO2

Question

How is the equilibrium yield of C6H12O6 affected by each of the following? 6 CO2(g) + 6 H2O(l) + HEAT C6H12O6(s) + 6 O2(g) (a) increasing PCO2 increases decreases no effect (b) increasing temperature increases no effect decreases (c) removing CO2 increases no effect decreases (d) decreasing the total pressure (TRICKY!!) increases decreases no effect (e) removing part of the C6H12O6 (s), but still in excess no effect decreases increases (f) adding more C6H12O6 (s), even though it is in excess no effect decreases increases

Explanation / Answer

A) If the partial pressure of CO2 is increased, the equilibrium shifts to the right as the system tries to use up some of the added CO2 (LeChatelier's principle). The result is an increase in the C6H12O6 at the new equilibrium. B) Decreasing the total pressure will cause the equilibrium to shift to the right as the system tries to build the pressure back up. There is 1 mole of gas on the reactant side and 6 moles of gas on the product side. As the equilibrium shifts to the right, the pressure will build back up. The result is an increase in the equilibrium concentration of C6H12O6. C) If CO2 is removed, the equilibrium will shift to the left as the system tries to replace some of the CO2 being removed. The result will be less C6H12O6 at the new equilibrium. D) Adding a catalyst will not affect the equilibrium because it speeds up both the forward and reverse reactions. But, it doesn't have an effect on the equilibrium concentrations.

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