Question
2) The hydrogen used in the Haber process is made in the reaction shown below, which is an equilibrium. CH_(4)(g)+H_(2)O(g)leftharpoons CO(g)+3H_(2)(g) Delta H=+206kJ/mol If the temperature of this equilibrium was increased, what would happen to the yield of hydrogen? __ ii) Explain your reasoning ....11111111 ....iiii .... __ ...................................................................... -...iiii IIII aiiiiii a b) i) If the pressure of this equilibrium was increased, what would happen to the yield of hydrogen? __ ...................................................................... ................. ii) __ ".........-...............
Answer
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Kevin
Professional · Tutor for 6 years
Answer
a) i) If the temperature of this equilibrium was increased, the yield of hydrogen would increase.ii) This is because the reaction is endothermic (
). According to Le Chatelier's principle, an increase in temperature will shift the equilibrium to the right, favoring the products and thereby increasing the yield of hydrogen.b) i) If the pressure of this equilibrium was increased, the yield of hydrogen would decrease.ii) This is because there are more moles of gas on the product side of the reaction. According to Le Chatelier's principle, an increase in pressure will shift the equilibrium towards the side with fewer moles of gas, in this case, the reactants, thereby decreasing the yield of hydrogen.
Explanation
## Step 1: Understanding the effect of temperature on equilibriumThe reaction given is an endothermic reaction, as indicated by the positive enthalpy change (
). According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration of components, the system will shift its equilibrium position to counteract the effect of the disturbance. In the case of an endothermic reaction, increasing the temperature will shift the equilibrium to the right, favoring the products.## Step 2: Understanding the effect of pressure on equilibriumLe Chatelier's principle also applies to changes in pressure. For a reaction where the number of moles of gas is different on the reactant and product sides, an increase in pressure will shift the equilibrium towards the side with fewer moles of gas. In the given reaction, there are 2 moles of gas on the reactant side and 4 moles on the product side.