Consider the following reaction where Kc 952x102 at 350 K C

Consider the following reaction where Kc = 9.52x10-2 at 350 K: CH4(g)+ CCI4(g) 2CH2C12(8) A reaction mixture was found to contain 2.91x102 moles of CH(,4.152 moles of CCl4(8) and 1.22*102 moles of CH2Cl2(8), in a 1.00 Liter container Indicate True (T)0rFalseforeachofthefollowing; 1.In order to reach equilibrium CH2CI2(g) must be consumed. 2. In order to reach equilibrium Kc must increase 3.In order to reach equilibrium CH4 must be consumed 4.Qc is less than Kc 5. The reaction is at equilibrium. No further reaction will occur.

Solution

We have,

Concentration of CH₄ = No. of moles/Volume = 2.91 x 10^-2/1 = 2.91 x 10^-2 M

Concentration of CCl₄ = No. of moles/Volume = 4.15 x 10^-2/1 = 4.15 x 10^-2 M

Concentration of CH₂Cl₂ = No. of moles/Volume = 2 x 1.22 x 10^-2/1 = 2.44 x 10^-2 M

Therefore, Qc = [CH₂Cl₂]²/ ([CCl₄][CH₄]) = (5.9536 x 10^-4) / (12.0765 x 10^-4) = 0.493

Therefore, Qc > Kc, so the reaction tries to produce more reactant and reach equilibrium.

1) False. According to Le Chateliers principle, consuming CH2Cl2 will produce more product, and hence the system moves away from the equilibrium.

2) True. Kc<Qc, so it must increase.

3) True. According to Le Chateliers principle, consuming CH4 will produce more reactant, and hence the system moves towards the equilibrium.

4) False.

5) False. The system is not at equilibrium as Qc is not equal to Kc.