Problem: At 1700°C, the equilibrium constant, Kc, for the following reaction is 4.10× 10–4.N2(g) + O2(g) ⇌ 2 NO(g)What percentage of O2 will react to form NO if 0.447 mol of N2 and 0.447 mol of O2 are added to a 0.619-L container and allowed to come to equilibrium at 1700°C?

FREE Expert Solution

We are being asked to determine the percentage of O2 that will react to form NO if 0.447 mol of N2 and 0.447 mol of O2 are added to a 0.619-L container and allowed to come to equilibrium at 1700°C.


We are going to do the following steps:

Step 1: Construct ICE Chart

Step 2: Determine the percentage of O2 reacted


95% (470 ratings)
View Complete Written Solution
Problem Details

At 1700°C, the equilibrium constant, Kc, for the following reaction is 4.10× 10–4.

N2(g) + O2(g) ⇌ 2 NO(g)

What percentage of O2 will react to form NO if 0.447 mol of N2 and 0.447 mol of O2 are added to a 0.619-L container and allowed to come to equilibrium at 1700°C?

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Mass Percent concept. You can view video lessons to learn Mass Percent. Or if you need more Mass Percent practice, you can also practice Mass Percent practice problems.