Consider the reaction at 500 ° C 500°C. N 2 (g) + 3 H 2 (g) - ⇀ ↽ - 2 NH 3 (g) K c = 0.061 N2 (g) + 3H2 (g) ↽--⇀2NH3 (g) Kc=0.061 If analysis shows that the composition of the reaction mixture at 500 ° C 500°C is 1.14 mol ⋅ L - 1 N 2 1.14 mol⋅ L-1N2, 5.52 mol ⋅ L - 1 H 2 5.52 mol⋅ L-1H2, and 3.42 mol ⋅ L - 1 NH 3 3.42 mol⋅ L-1NH3, what is the value of the reaction quotient Q Q?

Question

Chemistry

Alani Blackburn

24 January, 07:25

Consider the reaction at 500 ° C 500°C. N 2 (g) + 3 H 2 (g) - ⇀ ↽ - 2 NH 3 (g) K c = 0.061 N2 (g) + 3H2 (g) ↽--⇀2NH3 (g) Kc=0.061 If analysis shows that the composition of the reaction mixture at 500 ° C 500°C is 1.14 mol ⋅ L - 1 N 2 1.14 mol⋅ L-1N2, 5.52 mol ⋅ L - 1 H 2 5.52 mol⋅ L-1H2, and 3.42 mol ⋅ L - 1 NH 3 3.42 mol⋅ L-1NH3, what is the value of the reaction quotient Q Q?

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Answers (1)

Know the Answer?

Kolby Whitehead · Answer 1

Q = 0.061 = Kc

Explanation:

Step 1: Data given

Temperature = 500 °C

Kc=0.061

1.14 mol/L N2

5.52 mol/L H2

3.42 mol/L NH3

Step 2: Calculate Q

Q=[products]/[reactants]=[NH3]² / [N2][H2]³

If Qc=Kc then the reaction is at equilibrium.

If Qc
If Qc>Kc then the reaction will shift left to reach equilibrium.

Q = (3.42) ² / (1.14 * 5.52³)

Q = 11.6964/191.744

Q = 0.061

Q = Kc the reaction is at equilibrium.