What effect does a) increasing the total pressure and b) increasing the temperature have on the equilibrium H2(g) CO2(g) D H2O(g) CO(g), DHo

d. a) no change in the equilibrium and

   b) equilibrium shifts towards products.

Explanation:

Hello.

In this case, for the reaction:

Which is endothermic due to the positive enthalpy of reaction. In such a way, based on the Le Chatelier's principle which states that increasing the temperature of an endothermic chemical reaction shifts the equilibrium towards products as heat is understood as a reactant, we can see, this is the case.

Moreover, since the change in the number of gaseous moles in the chemical reaction (coefficients balancing the reaction) is 0 (1+1-1-1), we can see that increasing the total pressure does not have any effect over equilibrium.

Therefore answer is d. a) no change in the equilibrium and b) equilibrium shifts towards products.

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