Answer: The value of [tex]K_p[/tex] for the net reaction is 1.94
Explanation:
The given chemical equations follows:
Equation 1: [tex]C(s)+2H_2O(g)\rightleftharpoons CO_2(g)+2H_2(g);K_{p1}[/tex]
Equation 2: [tex]H_2(g)+CO_2(g)\rightleftharpoons H_2O(g)+CO(g);K_{p_2}[/tex]
The net equation follows:
[tex]C(s)+CO_2(g)\rightleftharpoons 2CO(g);K_{p}[/tex]
As, the net reaction is the result of the addition of first equation and the twice of second equation. So, the equilibrium constant for the net reaction will be the multiplication of first equilibrium constant and the square of second equilibrium constant.
The value of equilibrium constant for net reaction is:
[tex]K_p=K_{p1}\times (K_{p2})^2[/tex]
We are given:
[tex]K_{p1}=3.09[/tex]
[tex]K_{p2}=0.793[/tex]
Putting values in above equation, we get:
[tex]K_p=3.09\times (0.793)^2=1.94[/tex]
Hence, the value of [tex]K_p[/tex] for the net reaction is 1.94
