The standard Gibbs energy change at `300K` for the reaction `2AhArrB+C` is 2494. `2J`. At a given time, the composition of the reaction mixture is `[A]=1/2, [B]=2` and `[C]=1/2`. The reaction proceeds in the
`(R=8.314JK//"mol"e=2.718)`

Options

A. Forward direction because `Q gt K_(C)`
B. Reverse direction because`Q gt K_(C)`
C. Forward direction because `Q lt K_(C)`
D. Reverse direction because `Q lt K_(C)`

Answer

B

Explanation

`2A hArr B + C`
`Q = ([B][C])/([A]^2)`
`Q = (2 xx 1/2)/((1//2)^2) = 4`
`DeltaG = - RT ln K_c`
`2494.2 = - 8.314 xx 300 xx ln K_c`
`ln K_c = -1`
`K_c = C^(-1)`
` = 1//2.718` [Given e = 2.718]
`=0.36`
As `Q gt K_c`, reaction move in reverse direction.