Respuesta :
Answer:
See explanation
Explanation:
We have to remember that for any equilibrium expression constant we can use the general reaction:
[tex]~aA~+~bB~<->~cC~+~dD[/tex]
With a equilibrium expression:
[tex]Keq~=~\frac{[C]^c[D]^d}{[A]^a[B]^b}[/tex]
We have to divide products by reagents and use the coefficient (in the balanced reaction) as exponents. So:
[tex]H_2_(_g_)~+~CO_2_(_g_)~->~H_2O_(_g_)~+~CO_(_g_)[/tex]
The reaction is already balanced. So, we can write the equilibrium expression:
[tex]Keq~=~\frac{[H_2O][CO]}{[H_2][CO_2]}[/tex]
In this case, all the compounds have gaseous state (g). So, we can change the concentration ([]) by the pressure of each compound:
[tex]Kp~=~\frac{P_H_2_O*P_C_O}{P_H_2*P_C_O_2}[/tex]
I hope it helps!
