For the reaction CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H2] = 0.045, [H2O] = 0.025, and [CH4] = 0.046M, in which direction will the reaction shift to attain equilibrium?

Question

Javon Strong

Chemistry

1 February, 11:26

For the reaction CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.025, [H2] = 0.045, [H2O] = 0.025, and [CH4] = 0.046M, in which direction will the reaction shift to attain equilibrium?

+1

Answers (1)

Know the Answer?

Jaden Hines · Answer 1

the reaction will shift to the left and produce more reactants

Explanation:

Step 1: data given

Kc = 190

Temperature = 1000 K

[CO] = 0.025 M

[H2] = 0.045 M

[H2O] = 0.025 M

[CH4] = 0.046 M

When Q=Kc, the system is at equilibrium and there is no shift to either the left or the right.

When Q
When Q>Kc, there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants

Step 2: The balanced equation

CO (g) + 3 H2 (g) ⇌ H2O (g) + CH4 (g)

Step 3: calculate Q

Q = [H2O][CH4] / [CO][H2]³

Q = (0.025*0.046) / (0.025*0.045³)

Q = 504.8

Q > Kc

This means there are more products than reactants. To decrease the amount of products, the reaction will shift to the left and produce more reactants