Suppose that 0.1000 mole each of H2and I2are placed in a 1.000-L flask, stoppered, and the mixture is heated to 425oC. At equilibrium, the concentration of I2is found to be 0.0210 M. Calculate Kcfor the following reaction at 425oC. H2(g) + I2(g) ⇄2 HI(g)

The value of equilibrium constant for the given reaction is 56.61

Explanation:

We are given:

Initial moles of iodine gas = 0.100 moles

Initial moles of hydrogen gas = 0.100 moles

Volume of container = 1.00 L

Molarity of the solution is calculated by the equation:

Equilibrium concentration of iodine gas = 0.0210 M

The chemical equation for the reaction of iodine gas and hydrogen gas follows:

Initial:                0.1    0.1

At eqllm:          0.1-x   0.1-x   2x

Evaluating the value of 'x'

The expression of for above equation follows:

Putting values in above expression, we get:

Hence, the value of equilibrium constant for the given reaction is 56.61

where is the following

explanation: