Question

Nitrogen and water react to form nitrogen monoxide and hydrogen, like this: N2(g) + 2H2O(g) → 2NO(g) +2H2(g)Also, a chemist finds that at a certain temperature the equilibrium mixture of nitrogen, water, nitrogen monoxide, and hydrogen has the following composition: compound pressure at equilibrium N2 0.25 M H20 1.3 M NO 0.33 M H2 1.2 MCalculate the value of the equilibrium constant for this reaction. Round your answer to significant digits.

Answer 1

Answer: The value of the equilibrium constant for this reaction is 0.37

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_c$  

For the given chemical reaction:

$N_2(g)+2H_2O(g)\rightarrow 2NO(g)+2H_2(g)$

The expression for $K_c$ is written as:

$K_c=\frac{[NO]^2\times [H_2]^2}{[H_2O]^2\times [N_2]^1}$

$K_c=\frac{(0.33)^2\times (1.2)^2}{(1.3)^2\times (0.25)^1}$

$K_c=0.37$

Thus the value of the equilibrium constant for this reaction is 0.37