CHEM: ADVANCED EQUILIBRIUM DYNAMIC STUDY MODULE

Given the following equilibrium reactions and constants, A + C ⇌ B + D K1 = 1.5 C ⇌ B K2 = 3.9 what is the equilibrium constant for the reaction A ⇌ D?

0.38

Given the following equilibrium reactions and constants, A + B ⇌ 2C K1 = 3.2 × 10-3 B + D ⇌ C K2 = 8.0 × 10-2 what is the equilibrium constant for the reaction A ⇌ B + 2D?

0.50 K1(1/K2)^2 = (3.2x10^-3)((1/8.0x10^-2)^2) = 0.50

A reaction mixture initially has [Br2] = 0.100 M and [Cl2] = 0.100. What is the equilibrium concentration of BrCl? Br2(g) + Cl2(g) ⇌ 2 BrCl(g) K = 1.45 × 10-4 at 150 K

1.19 × 10-3 M K= [BrCl]^2 / [Br2][Cl2] 1.45x10^-4 = (2X)^2 / (0.100) square root of: 1.45x10^-4 = square root of: (2X)^2 / (0.100) 1.20x10^-2 = (2X)/0.100 1.20x10^-3 = 2.01X X= 5.97x10^-4 [BrCl] = 2X soo... 2(5.97x10^-4) = 1.19 × 10-3 M

A reaction mixture initially has [H2S] = 0.100 M. What is the equilibrium concentration of H2? 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = 1.67 × 10-7 at 298 K

1.49 × 10-3 M 1.67x10^-7 = (2X)^2(X) / (0.100)^2 1.67x10^-7 = 4X^3 X= 7.47x10^-4 H2= 2X so.... 2(7.47x10^-4) = 1.49x10^-3

A reaction mixture initially has [SO3] = 0.150 M. What is the equilibrium concentration of SO2? 2 SO3(g) ⇌ 2 SO2(g) + O2(g) K = 1.6 × 10-10 at 350 K

1.9 × 10-4 M K=[SO2]^2[02] / [SO3]^2 1.6x10^-10 = (2X)^2(X) / (0.150)^2 3.6X10^-12 = 4X^3 X= 9.7x10^-5 SO2 = 2X soo.... 2(9.7x10^-5) = 1.9 × 10-4 M

Given the following equilibrium reactions and constants, A ⇌ 2 B K1 = 2.4 × 102 B ⇌ C K2 = 0.35 what is the equilibrium constant for the reaction A ⇌ 2 C?

29

A reaction mixture initially has [CH3OH] = 0.500 M. What is the equilibrium concentration of CO? CH3OH(g) ⇌ CO(g) + 2 H2(g) K = 4.42 × 10-7 at 125 K

3.81 x 10-3 M K= [CO][H2]^2 / [CH3OH] 4.42 × 10-7 = (X)(2X)^2/ (0.500) 2.21x10^-7 = 4X^3 X= 3.81x10^-3 M

A reaction mixture initially has [H2S] = 0.100 M. What is the equilibrium concentration of S2? 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = 1.67 × 10-7 at 298 K

7.47 × 10-4 M K= [H2]^2[S2] / [H2S]^2 1.67x10-7 = (2X)^2(X) / (0.100)^2 1.67x10^-7 = 4X^3 X= 7.47x10^-4 M

A reaction mixture initially has [CH3OH] = 0.500 M. What is the equilibrium concentration of H2? CH3OH(g) ⇌ CO(g) + 2 H2(g) K = 4.42 × 10-7 at 125 K

7.62 x 10-3 M K= [CO][H2]^2 / [CH3OH] 4.4x10^-7 = (X)(2X)^2 / (0.500) 2.21x10^-7 = 4X^3 X= 3.81x10^-3 H2= 2X sooo.... 2(3.81x10^-3) = 7.62 x 10-3 M

Given the following equilibrium reactions and constants, A + B ⇌ C K1 = 0.392 B + D ⇌ C K2 = 0.0483 what is the equilibrium constant for the reaction A ⇌ D?

8.12 K1 * 1/K2 = (0.392) (1/0.0483) = 8.12

A reaction mixture initially has [NO2] = 0.100 M and [ClNO] = 0.100 M. What is the equilibrium concentration of NO? NO2(g) + ClNO(g) ⇌ ClNO2(g) + NO(g) K = 7.7 × 10-5 at 298 K

8.8 × 10-4 M

If the volume of the reaction vessel is decreased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? Br2(g) + Cl2(g) ⇌ 2 BrCl(g)

No shift

If a catalyst is added to the following equilibrium system, in which direction will the reaction shift to relieve the stress? 3 O2(g) + heat ⇌ 2 O3(g)

No shift Why? When a catalyst is added to the equilibrium system, there is no effect on the equilibrium system.

If the concentration of O2 is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g)

Shift to the products

If the temperature is decreased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? H2(g) + Cl2(g) ⇌ 2 HCl(g) + heat

Shift to the products

If the temperature is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? C(s) + H2O(g) + heat ⇌ CO(g) + H2(g)

Shift to the products

If the volume is decreased, resulting in an increase in pressure in the equilibrium system, in which direction will the reaction shift to relieve the stress? C2H2(g) + 2 H2(g) ⇌ C2H6(g)

Shift to the products

If the volume is increased, resulting in a decrease in pressure in the equilibrium system, in which direction will the reaction shift to relieve the stress? 2 NOCl(g) ⇌ Cl2(g) + 2 NO(g)

Shift to the products

If the volume of the reaction vessel is decreased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? CO2(g) + H2(g) ⇌ CO(g) + H2O(l)

Shift to the products

If the volume of the reaction vessel is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? C(s) + CO2(g) ⇌ 2 CO(g)

Shift to the products

If the volume of the reaction vessel is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? CaCO3(s) ⇌ CaO(s) + CO2(g)

Shift to the products

If the concentration of Br2 is decreased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? Br2(g) + Cl2(g) ⇌ 2 BrCl(g)

Shift to the reactants

If the concentration of H2 is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? 2 CH4(g) ⇌ C2H2(g) + 3 H2(g)

Shift to the reactants

If the temperature is decreased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? N2(g) + O2(g) + heat ⇌ 2 NO(g)

Shift to the reactants

If the temperature is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? C2H2(g) + 2 Cl2(g) ⇌ C2H2Cl4(g) + heat

Shift to the reactants

If the temperature is increased in the following equilibrium system, in which direction will the reaction shift to relieve the stress? H2(g) + Cl2(g) ⇌ 2 HCl(g) + heat

Shift to the reactants

A reaction mixture initially has PN2 = 0.750 atm and PO2 = 0.750 atm. What is the equilibrium pressure of NO? N2(g) + O2(g) ⇌ 2 NO(g) Kp = 4.1 × 10-31 at 298 K

4.8 × 10-16 atm K= [NO]^2/ [N2][02] 4.1x10^-31 = (2X^2) / (0.750 - X)^2 square root of: 4.1x10^-31 = square root of: (2X^2) / (0.750)^2 6.4x10^-16 = 2X/0.750 4.8x10^-16 = 2X X= 2.4x10^-16 NO = 2X soo... 2(2.4x10^-16) = 4.8x10^-16 M

A reaction mixture initially has [CO2] = 0.200 M and 10.0 grams of Ni. What is the equilibrium concentration of CO? Ni(s) + CO2(g) ⇌ NiO(s) + CO(g) K = 2.5 × 10-4 at 1500 K

5.0 × 10-5 M K= [CO] / [CO2] 2.5x10^-4 = (X) / (0.200) 5.0x10^-5 = X

Given the following equilibrium reactions and constants, A + B ⇌ C K1 = 1.3 × 103 2C ⇌ B + D K2 = 4.3 × 105 what is the equilibrium constant for the reaction A + C ⇌ D?

5.6 × 10^8 K1 * K2 = (1.3 × 103)(4.3 × 105) = 5.6 × 10^8

A reaction mixture initially has [SO3] = 0.150 M. What is the equilibrium concentration of O2? 2 SO3(g) ⇌ 2 SO2(g) + O2(g) K = 1.6 × 10-10 at 350 K

9.7 × 10-5 M K= ([SO2]3[02]) / ([SO3]2 1.6x10^-10 = (2X)^2 (X)/ (0.150)^2 3.6x10^-12 = 4X^3 X= 9.7x10^-5 M