# chemistry

posted by .

I also had a problem with this type of questionthe initial pressure of NOCl(g) is 4.329 atm, calculate the % of NOCl(g) left over after the reaction reaches equilibrium according to the balanced equation. The value of Kp at 400.0 °C is 1.99. The initial pressure of the reaction products is 0 atm.

2NOCl(g) = 2NO(g)+Cl2(g)

• chemistry -

initial:
NOCl = 4.329
NO = 0
Cl2 = 0

change:
NOCl = -2x
NO = +2x
Cl2 = x

equilibrium:
NOCl = 4.329 - 2x
NO = 2x
Cl2 = x

Substitute into Kp and solve for x, multiply by 2 and subtract from original. That gives pressure of NOCl at equilibrium. I don't know if percent is to be based on pressure or not. I would think it would be based on grams but I don't see a way to quickly convert to grams.One way might be to convert Kp to Kc and find concns at equilibrium, then tak a liter.

• chemistry -

1.99 = (3x)/(4.329-2x)

8.615 - 3.98x = 3x
8.615 = 6.98x
x = 1.23

NO = 2.46 atm
Cl2 = 1.23 atm

The question now is, how to find the % NOCl left over?