Standard entropies of` X_(2), Y,_(2) and XY_(3)` are 60,40 and 50`JK^(-1) mol^(-1)` respectively. For the reaction:
`(1)/(2) X ^(2) + (3)/(2) Y _(2) to XY _(3)`
`Delta H =- 30 kJ` to be at equilibrium, the temperature will be:

Options

A. 750 K
B. 1000 K
C. 1250 K
D. 500 K

Explanation

`Delta S = sum S _("Products") - sum S _("Reactants") = 50 - [ (1)/(2) xx 60 + (3)/(2) xx 40] =- 40 JK ^(-1) mol^(-1)`
At equilibrium, `Delta G = Delta H - T Delta S =0 i.e., Delta H - T Delta S,T = (DeltaH)/(DeltaS) = (- 30 xx 1000)/(-40) = 750 K`