The standard Gibbs energy change at 300 K for the reaction `2A hArr B +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=8.314 J//K//"mol", e=2.718]`

Options

A. forward direction because `Q lt K_(e )`
B. reverse direction because `Q lt K_(e )`
C. forward direction because `Q gt K_(e )`
D. reverse direction because `Q gt K_(e )`

Answer

D

Explanation

`DeltaG^(@)=2494.2J`
`2A hArr B+C`
`R=8.314 J//K"mol"`.
e= 2.718
`[A]=(1)/(2), [B]=2, [C]=(1)/(2)`
`Q=([B][C])/([A]^(2))=(2xx1//2)/((1)/(2))^(2)=4`
`Delta G^(@)= - 2.303 " RT log " K_(e)`
`2494.2J= - 2.303xx(8.314 J//K//"mol")xx(300K)log K_(e )`
`implies " log " K_(e )= -(2494.2 J)/(2.303xx8.314 J//K//"mol" xx300K)`
`implies log K_(e )= -0.4341`
`K_(e )=0.37`
`Q gt K_(e )`