Question

Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction 2H2(g)+O2(g)⇌2H2O(g) what is the likely magnitude of the equilibrium constant K?

Answer 1

This is an incomplete question, here is a complete question.

Hydrogen is used as a rocket fuel because it is very light and reacts explosively and completely with oxygen. For the combustion reaction

$2H_2(g)+O_2(g)\rightleftharpoons 2H_2O(g)$

what is the likely magnitude of the equilibrium constant K?

K < 10⁻³

10⁻³ < K < 10³

K = 0

K > 10³

Answer : The correct option is, K > 10³

Explanation :

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The given equilibrium chemical reaction is:

$2H_2(g)+O_2(g)\rightleftharpoons 2H_2O(g)$

The expression for equilibrium constant will be;

$K=\frac{[H_2O]^2}{[H_2]^2[O_2]}$

As per question, when $H_2$ and $O_2$ react completely then the reaction will be product favored that means the value of equilibrium constant will be high.

Hence, the correct option is, K > 10³