Given N2(g) + O2(g) â 2NO(g) Kc1 = 1.0 x 10-30 N2(g) + Br2(g) + O2(g) â 2NOBr(g) Kc2 = 2.0 x 10-27 (a) What is the Kc for the reaction: 2NO(g) + Br2(g) â 2NOBr (g)? ÎHo = â 47.14 kJ (b) If you start with [NO] = 5.0 x10-3 M, [Br2] = 1.9 x 10-3 M, and [NOBr] = 6.9 x 10-3 M, is the reaction at equilibrium? If not, predict the direction in which reaction will occur to reach equilibrium. (c) What is the ÎGo and ÎSo of the above reaction? Is the reaction spontaneous or nonspontaneous at 25oC (d) At what temperature in oC the spontaneity of the above reaction will shift? (i.e. spontaneous becomes non-spontaneous or vice versa)

Question

Given N2(g) + O2(g) â 2NO(g) Kc1 = 1.0 x 10-30 N2(g) + Br2(g) + O2(g) â 2NOBr(g) Kc2 = 2.0 x 10-27 (a) What is the Kc for the reaction: 2NO(g) + Br2(g) â 2NOBr (g)? ÎHo = â 47.14 kJ (b) If you start with [NO] = 5.0 x10-3 M, [Br2] = 1.9 x 10-3 M, and [NOBr] = 6.9 x 10-3 M, is the reaction at equilibrium? If not, predict the direction in which reaction will occur to reach equilibrium. (c) What is the ÎGo and ÎSo of the above reaction? Is the reaction spontaneous or nonspontaneous at 25oC (d) At what temperature in oC the spontaneity of the above reaction will shift? (i.e. spontaneous becomes non-spontaneous or vice versa)

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