At a certain temperature, the for the decomposition of h2s is 0.776. h2s(g)↽−−⇀h2(g)+s(g) initially, only h2s is present at a pressure of 0.200 atm in a closed container. what is the total pressure in the container at equilibrium?

0.365 atm is the total pressure in the container at equilibrium.

Explanation:

Given , equilibrium constant of the reaction in terms of partial pressure:

Initial Partial pressure of the hydrogen sulfide gas =

Let the partial pressure of hydrogen gas and sulfur gas at equilibrium be p.

Initially   0.200 atm

At eq'm  0.200-p           p   p

Solving the equation we will get two values of 'p' from which we will ignore the negative value.

p = 0.165 atm

Partial pressure of the hydrogen sulfide gas at equilibrium=

Total pressure in the container at equilibrium :

0.200-p + p + p =0.200 atm +p = 0.365 atm

the answer would be b i believe