Question

What is the equilibrium constant for the reaction
H2(g) CO2(9) = H2O(g) + CO(g)?

Answer 1

See explanation

Step-by-step explanation:

We have to remember that for any equilibrium expression constant we can use the general reaction:

`~aA~+~bB~<->~cC~+~dD`

With a equilibrium expression:

`Keq~=~([C]^c[D]^d)/([A]^a[B]^b)`

We have to divide products by reagents and use the coefficient (in the balanced reaction) as exponents. So:

`H_2_(_g_)~+~CO_2_(_g_)~->~H_2O_(_g_)~+~CO_(_g_)`

The reaction is already balanced. So, we can write the equilibrium expression:

`Keq~=~([H_2O][CO])/([H_2][CO_2])`

In this case, all the compounds have gaseous state (g). So, we can change the concentration ([]) by the pressure of each compound:

`Kp~=~(P_H_2_O*P_C_O)/(P_H_2*P_C_O_2)`

I hope it helps!