Question

Consider the following reaction where Kc = 154 at 298 K.2NO(g) + Br2(g) 2NOBr(g)A reaction mixture was found to contain 4.64×10-2 moles of NO(g), 4.56×10-2 moles of Br2(g) and 0.102 moles of NOBr(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 forward direction.

Step-by-step explanation:

At the given interval, concentration of NO =
`(4.64* 10^(-2))/(1)M=4.64* 10^(-2)M`

Concentration of
`Br_(2)` =
`(4.56* 10^(-2))/(1)M=4.56* 10^(-2)M`

Concentration of NOBr =
`(0.102)/(1)M=0.102M`

Reaction quotient,
`Q_(c)` , for this reaction =
`([NOBr]^(2))/([NO]^(2)[Br_(2)])`

species inside third bracket represents concentrations at the given interval.

So,
`Q_(c)=((0.102)^(2))/((4.64* 10^(-2))^(2)* (4.56* 10^(-2)))=106`

So, the reaction is not at equilibrium.

As
`Q_(c)< K_(c)` therefore reaction must run in forward direction to increase
`Q_(c)` and make it equal to
`K_(c)`.