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 [tex]K_p[/tex]
For the given chemical reaction:
[tex]H_2S(g)+I_2(g)\rightarrow S(g)+2HI(g)[/tex]
The expression for [tex]K_p[/tex] is written as:
[tex]K_p=\frac{(p_{HI})^2}{(p_{H_2S})^1}[/tex]
[tex]K_p=1.33\times 10^{-5}[/tex]
[tex]1.33\times 10^{-5}=\frac{p_{HI}^2}{p_{H_2S}^1}[/tex]
[tex]1.33\times 10^{-5}=\frac{(0.010\times p_{H_2S})^2}{p_{H_2S}^1}[/tex]
[tex]p_{H_2S}=0.133[/tex]
[tex]p_{HI}=0.010\times 0.133=0.0013[/tex]
Total pressure at equilibrium = [tex]p_{H_2S}+p_{HI}[/tex] = 0.133+0.0013 = 0.1343 atm
