Question

The equilibrium constant K_c for the reaction

H₂(g) + Br₂(g) ⇆ 2HBr(g)

is 2.180×10⁶ at 730°

C. Starting with

4.20 moles of HBr

in a 17.8−L reaction vessel, calculate the concentrations of H₂,Br₂, and HBr at equilibrium.

17. The equilibrium constant Kc for the reaction below is 0.00771 at a certain temperature. Br2(g) ⇌ 2Br(g) If the initial concentrations are [Br2] = 0.0433 M and [Br] = 0.0462 M, calculate the concentrations of these species at equilibrium. For the reaction H2(g) + CO2(g) ⇆ H2O(g) + CO(g) at 700°C, Kc = 0.534.

Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.690 mole of CO and 0.690 mole of H2O is heated to 700°C in a 20.0−L container. For the reaction H2(g) + CO2(g) ⇆ H2O(g) + CO(g) at 700°C, Kc = 0.534. Calculate the number of moles of H2 that are present at equilibrium if a mixture of 0.690 mole of CO and 0.690 mole of H2O is heated to 700°C in a 20.0−L container.

Answer 1