The reaction Cr2O3 + 2Al → Al2O3 + 2Cr (Δ G° = - 421 kj) is thermodynamically feasible due to -ve value of Δ G. Why does this reaction not take place at room temperature?

Question

The reaction Cr2O3 + 2Al → Al2O3 + 2Cr (Δ G° = - 421 kj) is thermodynamically feasible due to -ve value of Δ G. Why does this reaction not take place at room temperature? (A) Certain amount of activation energy is essential for thermodynamically feasible reactions also (B) Due to high melting point of chromium oxide the reaction does not take place (C) Overall value of Δ G for the net reaction becomes positive (D) Molecules of Cr2O3 and Al are not oriented properly

Tardigrade Admin · Accepted Answer

The spontaneous reaction also requires a certain amount of activation energy therefore heating is required.

Q. The reaction $C r_{2} O_{3} + 2 A l \to A l_{2} O_{3} + 2 C r (Δ G^{°} = - 421 kj)$ is thermodynamically feasible due to -ve value of $Δ G$ . Why does this reaction not take place at room temperature?

Certain amount of activation energy is essential for thermodynamically feasible reactions also

Due to high melting point of chromium oxide the reaction does not take place

Overall value of $Δ G$ for the net reaction becomes positive

Molecules of $C r_{2} O_{3}$ and $A l$ are not oriented properly

The spontaneous reaction also requires a certain amount of activation energy therefore heating is required.

Q. The reaction Cr2​O3​+2Al→Al2​O3​+2Cr(ΔG°=−421kj) is thermodynamically feasible due to -ve value of ΔG. Why does this reaction not take place at room temperature?

Certain amount of activation energy is essential for thermodynamically feasible reactions also

Due to high melting point of chromium oxide the reaction does not take place

Overall value of ΔG for the net reaction becomes positive

Molecules of Cr2​O3​ and Al are not oriented properly

The spontaneous reaction also requires a certain amount of activation energy therefore heating is required.

Q. The reaction $C r_{2} O_{3} + 2 A l \to A l_{2} O_{3} + 2 C r (Δ G^{°} = - 421 kj)$ is thermodynamically feasible due to -ve value of $Δ G$ . Why does this reaction not take place at room temperature?

Overall value of $Δ G$ for the net reaction becomes positive

Molecules of $C r_{2} O_{3}$ and $A l$ are not oriented properly