Given the equilibrium constant (K) which side of the reaction is favoured N2(g) + 3H2(g) 2NH3(g) Keq = 735
Question
Given the equilibrium constant (K) which side of the reaction is favoured N2(g) + 3H2(g) 2NH3(g) Keq = 735
Solution
The equilibrium constant (K) for a reaction is a measure of the ratio of the concentrations of the products to the reactants at equilibrium. If K > 1, the reaction is product-favored; if K < 1, the reaction is reactant-favored.
In this case, the equilibrium constant (Keq) for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) is given as 735. Since this value is greater than 1, we can say that the reaction is product-favored. This means that at equilibrium, there will be more NH3 (the product) than N2 and H2 (the reactants).
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Given the equilibrium constant (K) which side of the reaction is favoured N2(g) + 3H2(g) Equilibrium arrow.jpg 2NH3(g) Keq = 0.00035 Group of answer choices Reactants Products The reaction is at equibirum
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