Question

For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5 at 333 K. What will be the total pressure of the gases above an equilibrium mixture if, at equilibrium, PHI = 0.010 × PH2 S?

Answer 1

Answer: The total pressure of the gases above an equilibrium mixture is 0.1343 atm

Explanation:-

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as
`K_p`

For the given chemical reaction:

`H_2S(g)+I_2(g)\rightarrow S(g)+2HI(g)`

The expression for
`K_p` is written as:

`K_p=((p_(HI))^2)/((p_(H_2S))^1)`

`K_p=1.33* 10^(-5)`

`1.33* 10^(-5)=(p_(HI)^2)/(p_(H_2S)^1)`

`1.33* 10^(-5)=((0.010* p_(H_2S))^2)/(p_(H_2S)^1)`

`p_(H_2S)=0.133`

`p_(HI)=0.010* 0.133=0.0013`

Total pressure at equilibrium =
`p_(H_2S)+p_(HI)` = 0.133+0.0013 = 0.1343 atm