## Trending News

Promoted

# chemistry equilibrium?

The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K:

2CH2Cl2(g) CH4(g) + CCl4(g)

Calculate the equilibrium partial pressures of all species when CH2Cl2(g) is introduced into an evacuated flask at a pressure of 0.847 atm at 350 K.

PCH2Cl2= ____atm

PCH4= ____ atm

PCCl4= _____atm

### 1 Answer

Relevance

- davidLv 71 month agoFavorite Answer
Kp = (P CH4)(P CCl4) / (P CH2Cl2)^2

10.5 = (x/2)^2 / (0.847 - x)^2 <<<< round

10.5 = (x/2)^2 / (0.847 )^2 <<<< solve

x = 5.489 << not small ,,, must solve as a quadrtic

10.5 = (x/2)^2 / (0.847 - x)^2

10.5(0.847 - x)^2 = x^2 /4

42(0.847 - x)^2 = x^2

x≈0.733776

x≈1.00154 <<< not possible .. x must be < 0.847

x = 0.734 atm

x/2 = p CH4 = p CCl4 = 0.367 atm

P CH2Cl2 = 0.847 - x = 0.113 atm

- Login to reply the answers

Still have questions? Get your answers by asking now.