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The hydrogen used in the Haber process is made in the reaction shown below, which is an equitionum. C_(4)+(2)+H_(2)O(g)leftharpoons CO(g)+3H_(2)(g) Eoorgy change =+206kJ/mol a If the temperature of this equilibrium was increased what would happen to the equilibrium yield of hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yield of __ ii __ 5 Hydrogen can also be made in the reaction shown below. CO(g)+H_(2)O(g)leftharpoons CO_(2)(g)+H_(2)(g) Energy change=-42kJ/mol a If the temperature of this equilibrium was increased, what would happen to the equilibrium yield hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yie hydrogen? ii __

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The hydrogen used in the Haber process is made in the reaction shown below, which is an equitionum. C_(4)+(2)+H_(2)O(g)leftharpoons CO(g)+3H_(2)(g) Eoorgy change =+206kJ/mol a If the temperature of this equilibrium was increased what would happen to the equilibrium yield of hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yield of __ ii __ 5 Hydrogen can also be made in the reaction shown below. CO(g)+H_(2)O(g)leftharpoons CO_(2)(g)+H_(2)(g) Energy change=-42kJ/mol a If the temperature of this equilibrium was increased, what would happen to the equilibrium yield hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yie hydrogen? ii __

The hydrogen used in the Haber process is made in the reaction shown below, which is an equitionum. C_(4)+(2)+H_(2)O(g)leftharpoons CO(g)+3H_(2)(g) Eoorgy change =+206kJ/mol a If the temperature of this equilibrium was increased what would happen to the equilibrium yield of hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yield of __ ii __ 5 Hydrogen can also be made in the reaction shown below. CO(g)+H_(2)O(g)leftharpoons CO_(2)(g)+H_(2)(g) Energy change=-42kJ/mol a If the temperature of this equilibrium was increased, what would happen to the equilibrium yield hydrogen? ii __ b If the pressure of this equilibrium was increased, what would happen to the equilibrium yie hydrogen? ii __

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SonnyElite · Tutor for 8 years

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4a i) The equilibrium yield of hydrogen will increase.<br />ii) This is because the reaction is endothermic and absorbs heat. According to Le Chatelier's principle, increasing the temperature will shift the equilibrium to the side that absorbs heat, in this case, the product side.<br /><br />4b i) The equilibrium yield of hydrogen will decrease.<br />ii) This is because there are more moles of gas on the product side. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium to the side with fewer moles of gas, in this case, the reactant side.<br /><br />5a i) The equilibrium yield of hydrogen will decrease.<br />ii) This is because the reaction is exothermic and releases heat. According to Le Chatelier's principle, increasing the temperature will shift the equilibrium to the side that absorbs heat, in this case, the reactant side.<br /><br />5b i) The equilibrium yield of hydrogen will not change.<br />ii) This is because there are equal moles of gas on both the reactant and product sides. According to Le Chatelier's principle, increasing the pressure will not affect the equilibrium if the number of moles of gas is the same on both sides.

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## Step1: <br />The first question asks about the effect of increasing temperature on the equilibrium yield of hydrogen in the reaction:<br />\[<br />\mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}(g)+3 \mathrm{H}_{2}(g) \quad \text { Energy change }=+206 \mathrm{~kJ} / \mathrm{mol}<br />\]<br />This is an endothermic reaction, meaning it absorbs heat. According to Le Chatelier's principle, increasing the temperature will shift the equilibrium to the side that absorbs heat, in this case, the product side. Therefore, the equilibrium yield of hydrogen will increase.<br /><br />## Step2:<br />The second question asks about the effect of increasing pressure on the equilibrium yield of hydrogen in the same reaction. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium to the side with fewer moles of gas. In this reaction, there are 2 moles of gas on the reactant side and 4 moles of gas on the product side. Therefore, increasing the pressure will shift the equilibrium to the reactant side, decreasing the equilibrium yield of hydrogen.<br /><br />## Step3:<br />The third question asks about the effect of increasing temperature on the equilibrium yield of hydrogen in the reaction:<br />\[<br />\mathrm{CO}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \rightleftharpoons \mathrm{CO}_{2}(\mathrm{~g})+\mathrm{H}_{2}(\mathrm{~g}) \quad \text { Energy change }=-42 \mathrm{~kJ} / \mathrm{mol}<br />\]<br />This is an exothermic reaction, meaning it releases heat. According to Le Chatelier's principle, increasing the temperature will shift the equilibrium to the side that absorbs heat, in this case, the reactant side. Therefore, the equilibrium yield of hydrogen will decrease.<br /><br />## Step4:<br />The fourth question asks about the effect of increasing pressure on the equilibrium yield of hydrogen in the same reaction. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium to the side with fewer moles of gas. In this reaction, there are 2 moles of gas on both the reactant and product sides. Therefore, increasing the pressure will not affect the equilibrium yield of hydrogen.<br /><br />#
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