Question

3. Consider the equilibrium: CO (g) + H2 (g) \(\rightleftharpoons\) C (s) + H2O (g) \(\Delta H = -131\ kJ.mol^{-1}\) Explain how and why the equilibrium position and the concentration of H2 would change if: a) more carbon is added. b) the concentration of CO is increased. c) the pressure inside the container is increased.

          3. Consider the equilibrium:
CO (g) + H2 (g) \(\rightleftharpoons\) C (s) + H2O (g) \(\Delta H = -131\ kJ.mol^{-1}\)
Explain how and why the equilibrium position and the concentration of H2
would change if:
a) more carbon is added.

b) the concentration of CO is increased.
c) the pressure inside the container is increased.

3. Consider the equilibrium:
CO (g) + H2 (g) ⇌ C (s) + H2O (g) Δ H = -131 kJ.mol^-1
Explain how and why the equilibrium position and the concentration of H2
would change if:
a) more carbon is added.

b) the concentration of CO is increased.
c) the pressure inside the container is increased.

Added by Christopher B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ivan Kochetkov

07/11/2024

Step 1

Step 1: The reaction is exothermic because the enthalpy change is negative. Show more…

Show all steps

Thanks for your feedback!

3. Consider the equilibrium: CO (g)+ H2 (g) C (s) + H2O (g) ΔΗ = -131 kJ.mol-1 Explain how and why the equilibrium position and the concentration of H2 would change if: a) more carbon is added. I b) the concentration of CO is increased. c) the pressure inside the container is increased.