Question

Consider mixture B, which will cause the net reaction to proceed forward.

Concentration (M) [XY] ⇌ [X] + [Y]

Initial: 0.500 0.100 0.100

Change -x +x +x

Equilibrium 0.500-x 0.100+x 0.100+x

The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced.

Part B

Based on a Kc value of 0.180 and the given data table, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration (M) [XY] ⇌ [X] + [Y]

initial: 0.200 0.300 0.300

Change: +x -x -x

equilibrium:0.200+x 0.300-x 0.300-x

Part C

Based on a Kc value of 0.180 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Express the molar concentrations numerically.

XY(aq