CHEM: EQUILIBRIUM STUDY MODULE
At 298 K, Kc = 0.0142 for the following reaction. What is the value of Kp? 2 NOBr(g) ⇌ 2 NO(g) + Br2(g)
0.347 Kp= Kc(RT)^change in "n" Kp= 0.0142 (0.0821 * 298) ^(3-2) Kp= 0.347
What is the expression for Kp for the given reaction? 2 NO2(g) ⇌ N2O4(g)
Kp= PN2O4 / P^2NO2
What is the expression for Kp for the given reaction? N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Kp= [P^2NH3] / [PN2][P^3H2]
At 298 K, Kc = 1.2 × 10-3 for the following reaction. What is the value of Kp? CO(g) + Cl2(g) ⇌ COCl2(g)
4.9 × 10^-5
What is the equilibrium constant expression for the following reaction? 2 Fe(s) + 3 H2O(g) ⇌ Fe2O3(s) + 3 H2(g)
K= [H2]3 / [H2O]3
What is the equilibrium constant expression for the following reaction? H2(g) + Cl2(g) ⇌ 2 HCl(g)
K= [HCl]2 / [H2][Cl2]
What is the equilibrium constant expression for the following reaction? 3 O2(g) ⇌ 2 O3(g)`
K= [O3]2 / [O2]3
At 298 K, Kc = 18.3 for the following reaction. What is the value of Kp? C4(s) + 4 O2(g) ⇌ 4 CO2(g)
18.3 Kp= 18.3(0.0821 * 298) ^(4-4) Kp= 18.3
What is the equilibrium constant, K, for the following reaction, if the concentration of CO was measured to be 3.1 × 10-2 M, the concentration of O2 was measured to be 1.7 × 10-2 M, and CO2 was measured to be 1.452 × 10-1 M? 2 CO(g) + O2(g) ⇌ 2 CO2(g)
K = 1.3 × 10^3 K= [1.452e-1]2 / [3.1e-2]2[1.7e-2] K= 1.3e3
What is the equilibrium constant, K, for the following reaction, if the concentration of N2 was measured to be 0.521 M, H2 was measured to be 0.482 M, and NH3 was measured to be 3.17 M? N2(g) + 3 H2(g) ⇌ 2 NH3(g)
K = 172 K= [3.17]2 / [0.521][0.482]3 K= 172
What is the equilibrium constant, K, for the following reaction, if the concentration of N2O4 was measured to be 2.35 × 10-2 M, and NO2 was measured to be 1.3 × 10-2 M? N2O4(g) ⇌ 2 NO2(g)
K = 7.2 × 10-3 K= [1.3e-2]2 / [2.35e-2] K= 7.2 x 10^-3
What is the equilibrium constant expression for the following reaction? 2 H2(g) + O2(g) ⇌ 2 H2O(g)
K= [H2O]2 / [H2]2[O2]
Consider the following equilibrium reaction and equilibrium constant: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) K = 1.2 × 109 Is this equilibrium reaction a product favored equilibrium with mostly products, a reactant favored equilibrium with mostly reactants, or a true equilibrium with both reactants and products?
Product favored equilibrium with mostly products WHY? the equilibrium constant is a very large value. K= 1.2x10^9
Consider the following equilibrium reaction and equilibrium constant: N2(g) + O2(g) ⇌ 2 NO(g) K = 2 × 10-9 Is this equilibrium reaction a product favored equilibrium with mostly products, a reactant favored equilibrium with mostly reactants, or a true equilibrium with both reactants and products?
Reactant favored equilibrium with mostly reactants WHY? the equilibrium constant is a very small value. (K= 2e-9)
Consider the following equilibrium reaction and equilibrium constant: CO(g) + Cl2(g) ⇌ COCl2(g) K = 5.0 Is this equilibrium reaction a product favored equilibrium with mostly products, a reactant favored equilibrium with mostly reactants, or a true equilibrium with both reactants and products?
True equilibrium with both reactants and products WHY? the equilibrium constant is close to approximately 1. K= 5.0
Consider the following equilibrium reaction and equilibrium constant: 2 NH3(g) ⇌ N2(g) + 3 H2(g) K = 9.4 Is this equilibrium reaction a product favored equilibrium with mostly products, a reactant favored equilibrium with mostly reactants, or a true equilibrium with both reactants and products?
True equilibrium with both reactants and products WHY? the equilibrium constant is close to approximately 1. K= 9.4
What is the equilibrium constant, K, for the following reaction, if the concentration of PCl3 and Cl2 was measured to be 6.4 M, and PCl5 was measured to be 3.93 × 10-2 M? PCl3(g) + Cl2(g) ⇌ PCl5(g)
K = 9.6 × 10-4
What is the equilibrium constant expression for the given reaction? PCl3(l) + Cl2(g) ⇌ PCl5(s)
K= 1 / [Cl2]
What is the equilibrium constant expression for the given reaction? CO2(g) + H2(g) ⇌ CO(g) + H2O(l)
K= [CO] / [CO2][H2]
What is the equilibrium constant expression for the given reaction? CO2(g) + C(s) ⇌ 2 CO(g)
K= [CO]2 / [CO2]
What is the equilibrium constant expression for the given reaction? Fe3O4(s) + 4 H2(g) ⇌ 3 Fe(s) + 4 H2O(g)
K= [H2O]4 / [H2]4
What is the equilibrium constant expression for the following reaction? Si(s) + 2 Cl2(g) ⇌ SiCl4(g)
K= [SiCl4] / [Cl2]2
What is the concentration of CO, if the concentration of Cl2 was measured to be 0.75 M, COCl2 was measured to be 2.21 M, and the equilibrium constant, K, is 5.3? CO(g) + Cl2(g) ⇌ COCl2(g)
[CO] = 0.56 M 5.3 = [2.21] / [CO][0.75] [CO] = 0.56 M
What is the concentration of HCl, if the concentration of H2 was measured to be 3.8 × 10-5 M, the concentration of Cl2 was measured to be 4.6 × 10-6 M, and the equilibrium constant, K, is 2.5 × 1034? H2(g) + Cl2(g) ⇌ 2 HCl(g)
[HCl] = 2.1 × 10^12 M
What is the concentration of NOBr, if the concentration of NO was measured to be 0.89 M, Br2 was measured to be 0.562 M, and the equilibrium constant, K, is 1.3 × 10-2? 2 NO(g) + Br2(g) ⇌ 2 NOBr(g)
[NOBr] = 0.076 M
What is the concentration of NO, if the concentration of N2 and O2 were measured to be 152 M, and the equilibrium constant, K, is 2.0 × 10-9? N2(g) + O2(g) ⇌ 2 NO(g)
[NO] = 6.8 × 10-3 M 2.0x10^-9 = [NO]2 / [152][152] [NO] = 6.8 x10^-3 M
The equilibrium constant for the given reaction is 1.2 × 103 at 668 K. After 45 seconds, [CO] = 0.045 M, [Cl2] = 0.026 M, and [COCl2] = 1.4 M. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? CO(g) + Cl2(g) ⇌ COCl2(g)
The reaction is at equilibrium because Q = K. Q= [COCl2] /[CO][Cl2] Q= [1.4] / [0.045][0.026] Q= 1.2x10^3 Q is equal to K, so the reaction is at equilibrium.
The equilibrium constant for the given reaction is 14.5 at 483 K. After 30 seconds, [CO] = 0.25 M, [H2] = 0.30 M, and [CH3OH] = 0.75. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? CO(g) + 2 H2(g) ⇌ CH3OH(g)
The reaction will proceed to the left because Q > K. Q= [CH3OH] / [CO][H2]2 Q= [0.75] / [0.25][0.30]2 Q= 33 Q is greater than K, so the reaction will proceed to the left. As the concentration of the product decreases and the concentrations of the reactants increase, the value of Q will decrease until it reaches the value of K.
The equilibrium constant for the given reaction is 2.0 at 473 K. After 10 seconds, [COF2] = 0.050 M, [CO2] = 0.15 M, and [CF4] = 0.15 M. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 COF2(g) ⇌ CO2(g) + CF4(g)
The reaction will proceed to the left because Q > K. Q= [CO2][CF4] / [COF2]2 Q=[0.15][0.15] /[0.050]2 Q= 9.0 Q is greater than K, so the reaction will proceed to the left. As the concentrations of the products decrease and the concentration of the reactant increases, the value of Q will decrease until it reaches the value of K.
The equilibrium constant for the given reaction is 0.0142 at 298 K. After 20 seconds, [NOBr] = 0.15 M, [NO] = 0.020 M, and [Br2] = 0.010. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 NOBr(g) ⇌ 2 NO(g) + Br2(g)
The reaction will proceed to the right because Q < K. Q= [NO]2[Br2] / [NONr]2 Q= [0.020]2[0.010] / [0.15]2 Q= 1.8 x10^-4 so... Q is less than K, so the reaction will proceed to the right. As the concentrations of the products increase and the concentration of the reactant decreases, the value of Q will increase until it reaches the value of K.