Fe(s) + H2O(g)<-> FeO(s) + H2(g)

Calculate K for the above reaction, using the information which follows.
H2O(g) + CO(g)<-> H2(g) + CO2(g) K = 1.6
FeO(s) + CO(g)<-> Fe(s) + CO2(g) K = 0.67

Add equn 1 to the reverse of equation 2. K1 = 1.6

K2 for the reversed equation is 1/0.67
K for the reaction is K1K2

thanks, the answer worked

it was 2.4

To calculate K for the reaction Fe(s) + H2O(g) <-> FeO(s) + H2(g), we can use the known values of K for the following two reactions:

1. H2O(g) + CO(g) <-> H2(g) + CO2(g) K = 1.6
2. FeO(s) + CO(g) <-> Fe(s) + CO2(g) K = 0.67

Step 1: Write the balanced equation for the given reaction:
Fe(s) + H2O(g) <-> FeO(s) + H2(g)

Step 2: Use the given equations to construct the overall equation:

H2O(g) + CO(g) <-> H2(g) + CO2(g) (multiply equation by 2)
2H2O(g) + 2CO(g) <-> 2H2(g) + 2CO2(g)

FeO(s) + CO(g) <-> Fe(s) + CO2(g)

Overall equation: Fe(s) + H2O(g) + CO(g) <-> FeO(s) + H2(g) + CO2(g)

(Note: We multiplied the first equation by 2 to balance the number of H2O and H2 molecules.)

Step 3: Calculate the overall K value from the given K values:

K overall = (K1 * K2) / (K3)

where K1, K2, and K3 are the respective equilibrium constants of the three equations involved in the overall reaction.

K overall = (1.6 * 0.67) / (1)

K overall = 1.072

Therefore, K for the reaction Fe(s) + H2O(g) <-> FeO(s) + H2(g) is approximately 1.072.

To calculate the equilibrium constant (K) for the given reaction, we need to use the equilibrium constant expression and the information provided.

The balanced equation for the given reaction is:
Fe(s) + H2O(g) ⇌ FeO(s) + H2(g)

The equilibrium constant expression for this reaction is:
K = [FeO(s)] * [H2(g)] / [Fe(s)] * [H2O(g)]

To find the value of K for the given reaction, we can use the equilibrium constants of the two reactions provided. We need to manipulate the given reactions in order to match the overall reaction.

First, let's reverse the second reaction and multiply it by the stoichiometric coefficients to get the desired products on the right side:
Fe(s) + CO2(g) ⇌ FeO(s) + CO(g)

The equilibrium constant expression for the reversed second reaction is:
K2 = [FeO(s)] * [CO(g)] / [Fe(s)] * [CO2(g)]

Next, let's multiply the first reaction by the stoichiometric coefficients to balance the equation:
Fe(s) + H2O(g) ⇌ FeO(s) + H2(g)

The equilibrium constant expression for the first reaction is:
K1 = [FeO(s)] * [H2(g)] / [Fe(s)] * [H2O(g)]

Now, let's multiply the two equilibrium constant expressions to obtain the equilibrium constant expression for the overall reaction:
K = K1 * K2

Substituting the given equilibrium constants:
K = 1.6 * 0.67

Calculating this multiplication gives us the value of K for the overall reaction:
K = 1.072

Therefore, the equilibrium constant (K) for the given reaction is approximately 1.072.