At 35°C, K = 1.6 ✕ 10^−5 for the following reaction.

2 NOCl(g) (equilibrium reaction arrow) 2 NO(g) + Cl2(g)

Calculate the concentrations of all species at equilibrium for each of the following original mixtures.

2.8 mol of NOCl, 2.8 mol of NO, and 1.4 mol of Cl2 in a 1.3-L flask.

So far what I did was make an ICE chart, for the E section, I got 2.15-2x, 2.15+2x, and 1.08+x for 2NOCL, 2NO, and Cl respectively.

Question

At 35°C, K = 1.6 ✕ 10^−5 for the following reaction.

 2 NOCl(g) (equilibrium reaction arrow) 2 NO(g) + Cl2(g) 

 Calculate the concentrations of all species at equilibrium for each of the following original mixtures. 

2.8 mol of NOCl, 2.8 mol of NO, and 1.4 mol of Cl2 in a 1.3-L flask.

So far what I did was make an ICE chart, for the E section, I got 2.15-2x, 2.15+2x, and 1.08+x for 2NOCL, 2NO, and Cl respectively.

anonymous · Answer

Not too sure what to do after the ice chart, and please correct me if my ICE is incorrect.