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
[tex]2H_2(g)+O_2(g)\rightleftharpoons 2H_2O(g)[/tex]
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:
[tex]2H_2(g)+O_2(g)\rightleftharpoons 2H_2O(g)[/tex]
The expression for equilibrium constant will be;
[tex]K=\frac{[H_2O]^2}{[H_2]^2[O_2]}[/tex]
As per question, when [tex]H_2[/tex] and [tex]O_2[/tex] 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
