If for the reaction at `300 K, 2 Mg _((s)) + O _(2 (g)) to 2 Mg O _((s)) , Delta _(r) H =- 1202 kJ mol ^(-1) , Delta , S=- 217 JK ^(-1) mol ^(-1).` The total entropychange `(Delta S)_(r)` and Gibbs energy change during the course of reaction`( Delta.G)` are respectivelv:

Options

A. `3.79 xx 10 ^(3) J , - 1136.9 J`
B. `3.79 xx 10^(3) J , + 1000 J`
C. `+ 1000 J, 3. 79 xx 10 ^(3) J`
D. `-1136.9 kJ , 3. 79 xx 10 ^(3) J`

Explanation

`Delta G = Delta H - T Delta S =- 1202 - (-2 17 xx 10 ^(-3) xx 300) =- 11 36 . 9 kJ`
Heat released will be absorbed by the surrounding to increase the entropy of surroundings.
`Delta S _("surr") =+ ( 1202xx 10 ^(3))/( 300) = + 4. 01 xx 10 ^(3) J mol ^(-1) therefore Delta S _("total") = - 217 + 4. 01 xx 10 ^(3) = + 3793 J mol ^(-1)`