Question

Consider the following reaction where K-9.52x102 at 350 K. A reaction mixture was found to contain 2.09x10 moles of CH4(g CH,CI2(g), in a 1.00 liter container. ),3.83102 moles of CCl4(g) and 1,09-102 moles of Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Qe, equals A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium Retry Entire Group and Exit

Answer 1

ANSWER:

Given,

K_c = 9.52 x 10^-2

Temperature, T = 350 K

The given reaction is:

CH₄(g) + CCl₄(g) $\rightarrow$ 2 CH₂Cl₂(g)

Number of moles of CH₄ = 2.09 x 10^-2 moles

Number of moles of CCl₄ = 3.83 x 10^-2 moles

Number of moles of CH₂Cl₂ = 1.09 x 10^-2 moles

Volume of solution = 1 L

So, number of moles of each species is equal to its concentration.

Now,

Reaction quotient, Q = {[CH₂Cl₂]²}/{[CH₄] x [CCl₄]}

= {[1.09 x 10^-2 moles]²}/{[2.09 x 10^-2 moles][ x [3.83 x 10^-2 moles]}

= 14.8 x 10^-2

Here,

Since, Q is not equal to K_c so this reaction is not in equilibrium.

Q > K_c ; that means reaction system shift towards left to reach equilibrium.

The reaction quotient, Q = 14.8 x 10^-2

The reaction must run in the reverse direction to reach equilibrium.