The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr

Question

The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 15.9 L container at 298K contains NOBr at a pressure of 0.363 atm and NO at a pressure of 0.421 atm, the equilibrium partial pressure of Br2 is _______atm.

Consider the following reaction:

2NH3(g) N2(g) + 3H2(g) If 3.53×10-4 moles of NH3, 0.297 moles of N2, and 0.320 moles of H2 are at equilibrium in a 16.6 L container at 945 K, the value of the equilibrium constant, Kp, is .

Explanation / Answer

1.

The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 15.9 L container at 298K contains NOBr at a pressure of 0.363 atm and NO at a pressure of 0.421 atm, the equilibrium partial pressure of Br2 is _______atm.

Answer:

Given reaction at equilibrium is

2NOBr(g) = 2NO(g) + Br2(g)

pNOBr = 0.363 atm

pNO = 0.421 atm

pBr2 = unknown = x

and the equilibrium constant, Kp = 0.160

But for the given reaction

Kp = [(pNO)2 * (pBr2)]/ (pNOBr)2

0.160 = [(0.421)2 * (x)]/ (0.363)2

0.160 = [0.177241 * x]/ 0.131769

X = [0.131769 * 0.160]/ 0.177241

X = 0.118951 atm

Hence, the partial pressure of Br2 is 0.118951 atm

2.

Consider the following reaction:

2NH3(g) N2(g) + 3H2(g) If 3.53×10-4 moles of NH3, 0.297 moles of N2, and 0.320 moles of H2 are at equilibrium in a 16.6 L container at 945 K, the value of the equilibrium constant, Kp, is .

Answer:

For the given reaction,

2NH3(g) = N2(g) + 3H2(g)

The equilibrium constant, Kp is

Kp = [(pN2) * (pH2)3]/ (pNH3)2

When we consider concentration of reactants in terms of molarity then we can write

Kp = [N2] * [H2]3]/ [NH3]2

Where, [N2], [H2] and [NH3] are concentrations in terms of molarity per litters

Hence, [N2] = 0.297/ 16.6 = 0.017892 M

[H2] = 0.320/ 16.6 = 0.019277 M

[NH3] = 3.53×10-4/ 16.6 = 2.12651×10-5 M

Therefore,

Kp = [N2] * [H2]3]/ [NH3]2

Kp = [0.017892] * [0.019277]3]/ [2.12651×10-5]2

Kp = [0.017892] * [7.16339x10-6]/ [4.52204x10-10]

Kp = 0.128167x10-6/ [4.52204x10-10]

Kp = 2.8343x102

Hence, the equilibrium constant, Kp, is 2.8343x102

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