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If for the reaction, 2Mg((s)) + O(2(g)...

If for the reaction,
`2Mg_((s)) + O_(2(g)) to 2MgO_((s)), ` at `27^@C` `Delta r H = -1202kJmol^(-1)` and `Delta r S = -217kJ^(-1) mol^(-1)`. The total entropy change `(DeltaS)_T` and Gibb's energy change during the course of reaction `(Delta r G)` are respectively:

A

`3789.66 J mol^(-1), -1100 k J`

B

`3789.66 J mol^(-1), -1136.9 k J`

C

`-1136.9 kJ, 3789.66 J mol^(-1)`

D

`+1100 J , 3789.66 J mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
B
`:. DeltaG=DeltaH-TDeltaS`
`=-1202-(-217xx10^(-3)xx300)`
`=-1126.9 kJ`
Heat released will be absorbed by the surrounding to increase the entropy of surroundings
`DeltaS_("Surr.")=+(1202xx10^(3))/300=4006.67 J mol^(-1)`
`DeltaS_(T)=-217+4006.67=3789.66 J mol^(-1)`
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