The equilibrium constant, Kc, for the following reaction is 9.52E-2 at 350 K. CH4 (g) CCl4 (g) 2 CH2Cl2 (g) Assuming that you start with equal concentrations of CH4 and CCl4 and no CH2Cl2 is initially present, describe the relative abundance of each species present at equilibrium. 1 [CCl4] 1 [CH4] 2 [CH2Cl2] 1) Lower 2) Higher 3) Can't tell

[CCl₄] = Lower.

[CH₄] = Lower.

[CH₂Cl₂] = Higher.

Explanation:

Based in the reaction:

CH₄ (g) + CCl₄ (g) → 2CH₂Cl₂ (g)

Kc is defined as:

Kc = 9.42x10⁻² = [CH₂Cl₂]² / [CCl₄] [CH₄]

Where the concentrations of the compounds are concentrations in equilibrium.

If you start with just CH₄ and CCl₄ the reaction will produce CH₂Cl₂ until the ratio of [CH₂Cl₂]² / [CCl₄] [CH₄] = Kc

That means CH₄ and CCl₄ will decrease in concentration and CH₂Cl₂ will increase its concentrations. Thus, in equilibrium the relative abundance of species are:

[CCl₄] = Lower.

[CH₄] = Lower.

[CH₂Cl₂] = Higher.