at 500K, Kc for the reaction:H2 +D2 gives 2HD is 3.6 what is the value of Kc for 2HD gives H2 +D2

To determine the value of the equilibrium constant (Kc) for the reverse reaction, 2HD ⇌ H2 + D2, you can use the relationship between forward and reverse reactions and their respective equilibrium constants.

The equilibrium constant (Kc) is defined as the ratio of the product concentrations to the reactant concentrations at equilibrium, with each concentration raised to the power of its stoichiometric coefficient.

Given that Kc for the forward reaction, H2 + D2 ⇌ 2HD, is 3.6, we can use this information to find Kc for the reverse reaction.

The relationship between forward and reverse reactions is expressed as follows:

Kc (reverse) = 1 / Kc (forward)

Therefore, to find Kc for the reverse reaction, we take the reciprocal of Kc for the forward reaction:

Kc (reverse) = 1 / 3.6

Simplifying this expression gives:

Kc (reverse) ≈ 0.278

So, the value of Kc for the reverse reaction, 2HD ⇌ H2 + D2, is approximately 0.278.