Consider the following endothermic reaction: C(s) + H_2O(g) doubleheadarrow CO(g

Question

Consider the following endothermic reaction: C(s) + H_2O(g) doubleheadarrow CO(g) + H_2(g) Delta H = 131 KJ This reaction is allowed to reach equilibrium at 25 degree c. In which direction (shift to the products or to the right, shift to the reactants or to the left, or no change) will the, reaction proceed if the changes below are made. If more H_2O is added to the system Shifts to the right Shifts to the left Shifts to the right No Change If some C (s) is removed from the system Shifts to the left shifts to the right No Change C. If the volume of the container is increased Shifts to Shifts to the left the right No Change If the temperature of Shifts to the reaction is increased the left Shifts to the right If a catalyst is added to the reaction vessel Shifts to the left Shifts to the right consider the following chemical reaction

Explanation / Answer

Using Le Chatelier's principle:

A.- Shifts to the right

B.- Shifts to the left

C.- No change

D.- Shifts to the right (Endothermic reaction)

E.- No change

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