One mole of N2( g) is mixed with 2 moles of H2( g) in a 4 litre vessel. If 50 % of N2( g) is con

step 1 In this problem, we have given that 1 mole of N2 gas is mixed with 2 moles of H2 gas in a 4 -lit

One mole of N2( g) is mixed with 2 moles of H2( g) in a 4...

One mole of $\mathrm{N}_2(\mathrm{~g})$ is mixed with 2 moles of $\mathrm{H}_2(\mathrm{~g})$ in a 4 litre vessel. If $50 \%$ of $\mathrm{N}_2(\mathrm{~g})$ is converted to $\mathrm{NH}_3(\mathrm{~g})$ by the following reaction: $$ \mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g}) $$ What will be the value of $\mathrm{K}_{\mathrm{c}}$ for the following equilibrium? $$ \mathrm{NH}_3(\mathrm{~g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{3}{2} \mathrm{H}_2(\mathrm{~g}) $$ (a) 256 (b) 16 (c) $\frac{1}{16}$ (d) None of these

One mole of $\mathrm{N}_2(\mathrm{~g})$ is mixed with 2 moles of $\mathrm{H}_2(\mathrm{~g})$ in a 4 litre vessel. If $50 \%$ of $\mathrm{N}_2(\mathrm{~g})$ is converted to $\mathrm{NH}_3(\mathrm{~g})$ by the following reaction:

$$
\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})
$$

What will be the value of $\mathrm{K}_{\mathrm{c}}$ for the following equilibrium?

$$
\mathrm{NH}_3(\mathrm{~g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{3}{2} \mathrm{H}_2(\mathrm{~g})
$$

(a) 256
(b) 16
(c) $\frac{1}{16}$
(d) None of these

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of the reactants and products over time.

Law of Mass Action

The Law of Mass Action states that at equilibrium, the rate of a chemical reaction is proportional to the product of the concentrations of the reactants each raised to the power of their respective stoichiometric coefficients. This law is the basis for writing the mathematical expression for the equilibrium constant.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, is a dimensionless value defined for a reversible reaction. It is calculated as the ratio of the product concentrations to the reactant concentrations, with each concentration raised to the power of its corresponding coefficient in the balanced chemical equation. Kc is specific to a given reaction at a particular temperature.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical equation. It is used to determine how the mole ratios of substances change as the reaction proceeds, which is crucial for calculating equilibrium concentrations and for understanding how much of each reactant is consumed or product formed.

Manipulation of Equilibrium Expressions

Manipulating equilibrium expressions involves mathematical adjustments when the form of the reaction is altered—for example, when a reaction is reversed or when the coefficients are multiplied or divided by a common factor. Reversing a reaction inverts the equilibrium constant, and scaling the stoichiometric coefficients results in the equilibrium constant being raised to a power corresponding to the scale factor.

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