Consider the following reaction equation
N\(_{2}\)(g) + 3H\(_{2(g)}\) ⇌ 2NH3(g) ∆H = -92kJ
Increasing the temperature of the reaction would
shift the equilibrium to the right
increase the yield of ammonia
decrease the amount of hydrogen
decrease the yield of ammonia
Explanation
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Discussions (8)
The given reaction is the synthesis of ammonia, which is an exothermic reaction with a negative enthalpy change.
N2(g) + 3H2(g) ⇌ 2NH3(g) ∆H = -92kJ
Based on Le Chatelier's principle, we can predict the effect of changes in conditions on the equilibrium of the reaction.
A. To shift the equilibrium to the right, we need to increase the concentration of the reactants or decrease the concentration of the products. This means adding more N2 and H2 or removing some NH3 from the reaction mixture.
B. To increase the yield of ammonia, we need to shift the equilibrium to the right, as more product will form. This means increasing the concentration of the reactants or decreasing the concentration of the products.
C. To decrease the amount of hydrogen, we need to shift the equilibrium to the left, as more reactant will remain. This means increasing the concentration of NH3 or decreasing the concentration of N2 and H2.
D. To decrease the yield of ammonia, we need to shift the equilibrium to the left, as more reactant will remain. This means increasing the concentration of N2 and H2 or decreasing the concentration of NH3.
Therefore, the correct answer to this question is B. To increase the yield of ammonia, we need to shift the equilibrium to the right.
