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

Concentration (M)initial:change:equilibrium:[XY]0.500x0.500xnet[X]0.100+x0.100+x+[Y]0.100+x0.100+xnetConcentration (M)[XY][X]+[Y]initial:0.5000.1000.100change:x+x+xequilibrium:0.500x0.100+x0.100+x

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

Based on a KcKcK_c value of 0.170 and the given data table, what are the equilibrium concentrations of XYXY, XX, and YY, respectively?

Express the molar concentrations numerically.

Calculating equilibrium concentrations when the net reaction proceeds in reverse

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

Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+xnet[X]0.300x0.300x+[Y]0.300x0.300xnetConcentration (M)[XY][X]+[Y]initial:0.2000.3000.300change:+xxxequilibrium:0.200+x0.300x0.300x

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

Based on a KcKcK_c value of 0.170 and the data table given, what are the equilibrium concentrations of XYXY, XX, and YY, respectively?

Express the molar concentrations numerically.