Question

The equilibrium constant is given for one of the reactions below.

Determine the value of the missing equilibrium constant.
2 HD(g) ⇌ H2(g) + D2(g) Kc = 0.28
2 H2(g) + 2 D2(g) ⇌ 4 HD(g)

Answer 1

To find the missing equilibrium constant, we can use stoichiometry and the first given equilibrium constant. The missing equilibrium constant for the second reaction is the square of the given Kc value.

Step-by-step explanation:

To determine the missing equilibrium constant, you can use the concept of equilibrium constant expressions.

In the first reaction, 2 HD(g) ⇌ H2(g) + D2(g), the equilibrium constant is given as Kc = 0.28.

To find the value of the missing equilibrium constant for the second reaction, 2 H2(g) + 2 D2(g) ⇌ 4 HD(g), we can use the stoichiometry.

Since the equilibrium constant is a ratio of product concentrations to reactant concentrations, and the stoichiometric coefficients for the second reaction are all multiplied by 2 compared to the first reaction, the missing equilibrium constant would be the square of the given Kc value.

Therefore, the missing equilibrium constant is 0.28 squared, which is approximately 0.0784.

Answer 2

12.7551

Step-by-step explanation:

The given chemical equation follows:

`2HD(g)\rightarrow H_2(g)+D_2(g)`

The equilibrium constant for the above equation is 0.28.

We need to calculate the equilibrium constant for the reverse equation of above chemical equation, which is:

`2H_2(g)+2D_2(g)\rightarrow 4HD(g)`

The equilibrium constant for the reverse reaction will be the reciprocal of the initial reaction.

If the equation is multiplied by a factor of '2', the equilibrium constant of the reverse reaction will be the square of the equilibrium constant of initial reaction.

The value of equilibrium constant for reverse reaction is:

`K_(eq)'=((1)/(0.28))^2`

Hence, the value of equilibrium constant for reverse reaction is 12.7551.