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 ?

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.  

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