Calculate the numerical Kc value for the following reaction if the equilibrium mixture contains 0.51 M CO2 , 0.30 M H2 , 1.8 M CH4 , and 2.0 M H2O.

CO(g) + 3H2 (g) ⇌ CH4 (g) + H2O (g

The answer to your question is   Kc = 260.86

Explanation:

Balanced chemical reaction

                CO + 3H₂   ⇔   CH₄  +  H₂O

Process

1.- Write the equilibrium constant for the reaction

              Kc =

2.- Substitute values in the formula

               Kc =

3.- Simplification

              Kc =

4.- Result

              Kc = 260.86

The equilibrium constant for this reaction is 261.4

Explanation:

Step 1: Data given

The equilibrium mixture contains:

0.51M CO  

0.30M H2

1.8M CH4

2.0 M H2O

Step 2: The balanced equation

CO(g) + 3H2 (g) ⇌ CH4 (g) + H2O (g)

For 1 mol CO we need 3 moles H2 to produce 1 mol CH4 and 1 mol H2O

Step 3: Calculate Kc

Kc = [CH4]*[H2O] / [CO]*[H2]³

⇒with [CH4] = 1.8 M

⇒with [H2] = 0.30 M

⇒with [H2O] = 2.0 M

⇒with [CO] = 0.51 M

Kc = (1.8*2.0) / (0.51*0.30³)

Kc = 261.4

The equilibrium constant for this reaction is 261.4

answer: h+ its less than oh

explanation: