Give reason : Reduction of `Cr_(2) O_(3)` with `Al` is thermodynamically feasible, yet it does no occur at room temperature.

Why is O_2 inert at room temperature ?

The reaction 2 H_2(g) + O_2(aq) to 2 H_2 O(l) is thermodynamically feasible. How is that a mixture of hydrogen and oxygen kept at room temperature shows no tendency to form water?

The reactions between H_(2)(g) and O_(2)(g) is highly feasuble yet allowing the gases to stand at room tempertaure in the same vessel does not lead to the formation of water . Explain

The reaction Cr_2O_3+2AltoAl_2O_3+2Cr (triangleG^(ɵ)=-421kJ)) Is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

The reaction Cr_2O_3+2AltoAl_2O_3+2Cr (triangleG^(ɵ)=-421kJ)) Is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

At the points of intersection of Al_(2)O_(3) and MgO curves (A), DeltaG^(@) becomes zero for reaction, (2)/(3)Al_(2)O_(3) + 2Mg to 2MgO + 4/3 Al Above this point, magnesium can reduce alumina. Although thermodynamically feasible, Mg is not used to reduction of Al_(2)O_(3) because

Mg_3 N_2 on reaction with water gives off NH_3 , but MgCl_2 on reaction with water does not give HCl at room temperature.

Give two reasons to justify- (a) Water at room temperaure is a liquid (b) an iron almirah is a solid at room temperature.