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

ID: 486206 • Letter: C

Question

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 +x -x -x

equilibrium 0.200+x 0.300x 0.300x

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

Part C

Based on a Kc value of 0.130 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

The Kc value for the reaction is:

Kc = ([X]*[Y])/[XY]

Putting values:

0.130 = ([0.3-x]*[0.3-x])/[0.2+x]

Solving we get:

x = 0.102

Thus,

[XY] = 0.302 M

[X] = 0.198 M

[Y] = 0.198 M

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.