Coal can be used to generate hydrogen gas (a potential fuel) by thefollowing endothermic reaction. C (s) + H2O (g) CO (g) + H2 (g) if this reaction mixture is at equilibrium, predict whether each ofthe following will result in the formation of additional hydrogengas, the formation of less hydrogen gas, or have no effect on thequantity og hydrogen gas. (a) adding more C to the reaction mixture (b) adding more H2O to the reaction mixture (c) raising the temperature of the reaction mixture (d) increasing the volume of the reaction mixture (e) adding a catalyst to the reaction mixture (f) adding an inert gas to the reaction mixture

Question

Chemistry

Titan

21 January, 07:31

Coal can be used to generate hydrogen gas (a potential fuel) by thefollowing endothermic reaction. C (s) + H2O (g) CO (g) + H2 (g) if this reaction mixture is at equilibrium, predict whether each ofthe following will result in the formation of additional hydrogengas, the formation of less hydrogen gas, or have no effect on thequantity og hydrogen gas. (a) adding more C to the reaction mixture (b) adding more H2O to the reaction mixture (c) raising the temperature of the reaction mixture (d) increasing the volume of the reaction mixture (e) adding a catalyst to the reaction mixture (f) adding an inert gas to the reaction mixture

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Jagger Gonzales · Answer 1

C (s) + H2O (g) CO (g) + H2 (g)

(a) adding more C to the reaction mixture

According to Le Chatelier's principle, adding additional reactant to a system will shift the equilibrium to the right, towards the side of the products - formation of additional hydrogen gas.

(b) adding more H2O to the reaction mixture

According to Le Chatelier's principle, adding additional reactant to a system will shift the equilibrium to the right, towards the side of the products - formation of additional hydrogen gas.

(c) raising the temperature of the reaction mixture

Since this reaction is endothermic, heat is a reactant. By Le Chatelier's principle, increasing the temperature will shift the equilibrium to the right, the formation of less hydrogen gas

(d) increasing the volume of the reaction mixture

When the volume of a system is increased (and the temperature is constant), the pressure will decrease. The equilibrium will shift in a direction that increases the number of gas molecules so that the pressure is also increased. A decrease in pressure will: Favour the reaction that increases the number of gas molecules. So formation of additional hydrogen gas

(e) adding a catalyst to the reaction mixture

- have no effect on the quantity of hydrogen gas. It must increases the rate at which the reaction is completed.

(f) adding an inert gas to the reaction mixture

- have no effect on the quantity of hydrogen gas.