Question

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 ?

Answer 1

Answer:

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<Kc then the reaction will shift right to reach equilibrium.

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.