Based on a Kc value of 0.170 and the data table given, what are the equilibrium conversations of XY, X, and Y, respectively? Calculating equilibrium concentrations when the net reaction proceeds in reverseConsider mixture C, which will cause the net reaction to proceed in reverse.– netConcentration (M) [XY[X]+ [Y]initial:0.2000.3000.300change:+xequilibrium:0.200 + x0.300 – x0.300 – xThe change in concentration, x, is positive for the reactants because they are produced and negative for the products becausethey are consumed.Part CBased on a K, value of 0.170 and the data table given, what are the equilibrium concentrations of XY, X, and Y,respectively?Express the molar concentrations numerically.

The reaction with ICE table given is, Given: Kc = 0.170

Calculating equilibrium concentrations when the net reaction proceeds in reverse Consider mixture C, which will cause the net reaction to proceed in reverse. + net Concentration (M) [XY] [X] + [Y] initial: 0.200 0.300 0.300 change: equilibrium: 0.200+x 0.300 – x 0.300 – x The change in concentration, x, is positive for the reactants because they are produced and negative for the products becaus they are consumed. Part C Based on a K, value of 0.170 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?

Calculating equilibrium concentrations when the net reaction proceeds in reverse Consider mixture C, which will cause the net reaction to proceed in reverse. + net Concentration (M) [XY] [X] + [Y] initial: 0.200 0.300 0.300 change: equilibrium: 0.200+x 0.300 – x 0.300 – x The change in concentration, x, is positive for the reactants because they are produced and negative for the products becaus they are consumed. Part C Based on a K, value of 0.170 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?