Equilibrium constant Kc for the reaction: H2 (g) + CO2 (g) - H2O (g) + CO (g) a)

Question

Equilibrium constant Kc for the reaction: H2 (g) + CO2 (g) - H2O (g) + CO (g) a) in one experiment, a container is introduced in a mixture formed by the four shown in the reaction gases. their initial concentrations were: 0.248 M H2, CO2 0.439 M, 1.25M H2O and CO 0975 m. Chemical reaction will there be? What direction, clockwise or counterclockwise? b) In another experiment, placed only H2 and CO2 in the reaction vessel, and their initial concentrations are 0.500 M MY 0500, respectively, what is the concentration of CO in the container at equilibrium achieved?

Explanation / Answer

A)Kc = Kf/Kb =( 0.248*0.439 )/ (1.25*0.975) = 0.0893 since it is less than 1 ...Kb > Kf hence backward reaction is favored B) H2 (g) + CO2 (g) - H2O (g) + CO (g) initial 0.5 0.5 0 0 equilibrium 0.5-x 0.5-x x x Kc = (0.5-x)^2/x^2 = 0.0893 (0.5-x)/x = 0.3 hence , x = 0.3846 M

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