Question

In: Chemistry

The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) ------CH4(g) +...

The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K.

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

Calculate the equilibrium concentrations of reactant and products when 0.321 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K.

[CH2Cl2] = ------------M

[CH4] = ------- M

[CCl4] = ------ M

Expert Solution

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

I 0.321 0 0

C -2x +x +x

E 0.321-2x +x +x

[CH2Cl2] = 0.321-2x/1 = 0.321-2x

[CH4] = x/1 = x

[CCl4] = x/1 = x

Kc = [CH4][CCl4]/[CH2Cl2]^2

10.5 = x*x/(0.321-2x)^2

10.5 = (x/0.321-2x)^2

3.24 = x/0.321-2x

3.24*(0.321-2x) = x

x= 0.139

[CH2Cl2] = 0.321-2x = 0.321-2*0.139 = 0.043M

[CH4] = x = 0.139 M

[CCl4] = x = 0.139 M

queen_honey_blossom answered 2 years ago

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