For a reaction a A + bB cC + dD the equilibrium constant K is defined as the rat

Question

For a reaction a A + bB cC + dD the equilibrium constant K is defined as the ratio of products to reactants at equilibrium: K = [c]c[D]d/[A]a[B]b Because K represents the ratio of products to reactants, the magnitude of K is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium. 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? K

Explanation / Answer

The magnitude of equilibrium constant depends on the extent to which the reaction goes in the forward direction to completion.
Now, hydrogen reacts with oxygen almost completely. So, the denominator reduces to a great extent as compared to the numerator.
Hence k has a very large value for this reaction.

From the options, k > 103

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