Question

Which of the reactions are spontaneous (favorable)? C6H13O9P+ATP⟶C6H14O12P2+ADPΔ????=−14.2 kJ/mol C4H4O5⟶C4H2O4+H2OΔ????=3.1 kJ/mol DHAP↽−−⇀glyceraldehyde-3-phosphateΔ????=3.8 kJ/mol L-malate+NAD+⟶oxaloacetate+NADH+H+Δ????=29.7 kJ/mol C2H4+H2−→−−Rh(I)C2H6Δ????=−150.97 kJ/mol glutamate+NAD++H2O⟶NH+4+α-ketoglutarate+NADH+H+Δ????=3.7 kcal/mol

Answer 1

Answer : The two spontaneous chemical reactions are:

`C_6H_(13)O_9P+ATP\rightarrow C_6H_(14)O_(12)P_2+ADP,\Delta G=-14.2kJ/mol`

`C_2H_4+H_2\overset{Rh(I)}\rightarrow C_2H_6,\Delta G=-150.97kJ/mol`

Explanation :

Gibbs free energy : It is defined as the amount of energy that is available to do useful work.

A reaction to be spontaneous when
`\Delta G<0`

A reaction to be non-spontaneous when
`\Delta G>0`

For the reaction to be spontaneous, the Gibbs free energy of the reaction
`\Delta G` is negative or we can say that the value of
`\Delta G` is less than zero.

From the given chemical reactions we conclude that there are two reactions that are spontaneous (favorable).

The two spontaneous chemical reactions are:

`C_6H_(13)O_9P+ATP\rightarrow C_6H_(14)O_(12)P_2+ADP,\Delta G=-14.2kJ/mol`

`C_2H_4+H_2\overset{Rh(I)}\rightarrow C_2H_6,\Delta G=-150.97kJ/mol`