Consider the following endothermic reaction that is used to generate Hydrogen ga

Question

Consider the following endothermic reaction that is used to generate Hydrogen gas from coal. C (s) + 2H2O (g) <------>CO (g) + H2 (g) How will the following changes affect the amount of H2 at equilibrium? In other words, Will the amount of H2 at equilibrium increase, decrease or stay the same?

1) Adding more C(s) to the reaction mixture

2) Adding more H2O(g) to the reaction mixture

3) Lowering the temperature of the reaction mixture

4) Decreasing the Volume of the container

5) Adding a catalyst

Explanation / Answer

apply Lechatelier concepts in equilibrium

1) Adding more C(s) to the reaction mixture --> no effect since it is a solid

2) Adding more H2O(g) to the reaction mixture --> adding reactants increases porducts, i..e H2 increases

3) Lowering the temperature of the reaction mixture --> this is combustion, so exothermic, will favour product formation, decreases H2

4) Decreasing the Volume of the container  --> increases P; favour least mol formation, since ratio is 2:2 no effect at all

5) Adding a catalyst --> no effect in equilibirum, only rate

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