At a certain temperature, the kp for the decomposition of h2s is 0.795.
h2s (g) > h2(g) + s(g)
initially, only h2s is present at a pressure of 0.203 atm in a closed container. what is the total pressure in the container at equilibrium?

The total pressure in the container at equilibrium is 0.37065 atm

Explanation:

Step 1: Data given

Kp for the decomposition of H2S is 0.795

Only H2S is present at a pressure of 0.203 atm

Step 2: The balanced equation

H2S (g) → H2(g) + S(g)

Step 3: Calculate partial pressure of H2 and S

Initially, there is no H2 and S, they have no pressure

There will react X

The pressure at the equilibrium we have:

H2: X

S: X

H2S: 0.203 - X

Kp = (pH2)(pS)/(pH2S)

0.795 = (x)(x)/(0.203 - X)

X = 0.16765

Step 4: Calculate total pressure at equilibrium:

Total pressure = the partial pressure of H2 + partial pressure of S + partial pressure of H2S

P = X + X + (0.203 - X)

P = 0.16765 + 0.16765 + (0.203 - 0.16765)

P =  0.37065 atm

The total pressure in the container at equilibrium is 0.37065 atm

answers: to make sure that all of the broken pieces of tablet were added to the water, to allow for fair comparison of all three trials, with different particle sizes to avoid experimental error