The Value of `DeltaG^(@)` for the formation of `Cr_(2)O_(3)` is `-"540 – InterviewSolution

1.	The Value of `DeltaG^(@)` for the formation of `Cr_(2)O_(3)` is `-"540KJ mol"^(-1)` and that of `Al_(2)O_(3)` is `-827"KJ mol"^(-1)`. Is the reduction of `Cr_(2)O_(3)` possible with Al ?
Answer» From the given data the following are the thermo chemical equations . `(4)/(3)Cr_((S))+O_(2_((g)))rarr(2)/(3)Cr_(2)O_(3(s)),DeltaG^(@)-540KJ" ...(1)"` `(4)/(3)Cr_(2)O_(3_((s)))+O_(2_((g)))rarr(2)/(3)Al_(2)O_(3_((s))),DeltaG^(@)-827KJ" ...(2)"` Equation (1)-Equation (2) `(2)/(3)Cr_(2)O_(3_((s)))+(4)/(3)Al_(s)rarr(2)/(3)Al_(2)O_(3_((s)))+(4)/(3)Cr_((s)),DeltaG^(@)-287KJ` .

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The Value of `DeltaG^(@)` for the formation of `Cr_(2)O_(3)` is `-"540KJ mol"^(-1)` and that of `Al_(2)O_(3)` is `-827"KJ mol"^(-1)`. Is the reduction of `Cr_(2)O_(3)` possible with Al ?
The reaction, `Cr_(2)O_(3)+2AlrarrAl_(2)O_(3)+2Cr(DeltaG^(Theta)=-421KJ)` is the thermodynamically feasible as is apparent from the Gibbs energy value . Why does it not take place at rom temperture?