Question

Consider the following reaction where Kc = 9.52×10-2 at 350 K.CH4(g) + CCl4(g) 2CH2Cl2(g)A reaction mixture was found to contain 2.18×10-2 moles of CH4(g), 3.79×10-2 moles of CCl4(g) and 1.09×10-2 moles of CH2Cl2(g), in a 1.00 liter container.Is the reaction at equilibrium?If not, what direction must it run in order to reach equilibrium?The reaction quotient, Qc, equals .The reactionA. must run in the forward direction to reach equilibrium.B. must run in the reverse direction to reach equilibrium.C. is at equilibrium.

Answer 1

The reaction is not at equilibrium and reaction must run in reverse direction.

Step-by-step explanation:

At the given interval, concentration of
`CH_(4)` =
`(2.18* 10^(-2))/(1)M=2.18* 10^(-2)M`

Concentration of
`CCl_(4)` =
`(3.79* 10^(-2))/(1)M=3.79* 10^(-2)M`

Concentration of
`CH_(2)Cl_(2)` =
`(1.09* 10^(-2))/(1)M=1.09* 10^(-2)M`

Reaction quotient,
`Q_(c)`, for this reaction =
`([CH_(2)Cl_(2)]^(2))/([CH_(4)][CCl_(4)])`

species inside third bracket represents concentrations at the given interval.

So,
`Q_(c)=((1.09* 10^(-2))^(2))/((3.79* 10^(-2))* (2.18* 10^(-2)))=1.44* 10^(-1)`

So, the reaction is not at equilibrium.

As,
`Q_(c)> K_(c)` therefore reaction must run in reverse direction to reduce
`Q_(c)` and make it equal to
`K_(c)`.