Calculating equilibrium concentrations when the net reactionproceeds forward

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

Concentration(M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x

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

Part B

Based on a Kc value of 0.260 and the given data table,what are the equilibrium concentrations of  XY, X, and Y,respectively?

Express the molar concentrations numerically.

[XY], [X], [Y] =		  M Â

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Calculating equilibrium concentrations when the net reactionproceeds in reverse

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

Concentration(M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x

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

Part C

Based on a Kc value of 0.260 and the data table given,what are the equilibrium concentrations of  XY, X, and Y,respectively?

Express the molar concentrations numerically.

[XY], [X],  [Y] =		  M Â

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