What effect does a) increasing the total pressure and b) increasing the temperat

Question

What effect does a) increasing the total pressure and b) increasing the temperature have on the equilibrium H2(g)+ CO2(g) H2O(g) + CO(g),Ho= 41.2 kJ/mol. Can you please explain why?

A) a) equilibrium shifts towards products,

b) equilibrium shifts towards products.

B) a) equilibrium shifts towards reactants,

b) equilibrium shifts towards products.

C) a) equilibrium shifts towards products,

b) equilibrium shifts towards reactants.

D) a) no change in the equilibrium,

b) equilibrium shift toward products.

E) a) no change in the equilibrium,

b) equilibrium shifts towards reactants.

Explanation / Answer

Ans E) a) no change in the equilibrium

b) equilibrium shifts towards reactants

Since the number of gaseous species are same on both the sides of the reaction , there will be no effect of pressure on the equillibrium condition.

Since the reaction has positive enthalpy change , the reaction is endothermic , and the increase in temperature will cause the reaaction to move backward.

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