Question

Which of the reactions are spontaneous (favorable)? DHAP − ⇀ ↽ − glyceraldehyde-3-phosphate Δ G = 3.8 kJ / mol DHAP↽−−⇀glyceraldehyde-3-phosphateΔG=3.8 kJ/mol C 4 H 4 O 5 ⟶ C 4 H 2 O 4 + H 2 O Δ G = 3.1 kJ / mol C4H4O5⟶C4H2O4+H2OΔG=3.1 kJ/mol C 2 H 4 + H 2 Rh ( I ) −−−→ C 2 H 6 Δ G = − 150.97 kJ / mol C2H4+H2→Rh(I)C2H6ΔG=−150.97 kJ/mol glutamate + NAD + + H 2 O ⟶ NH + 4 + α-ketoglutarate + NADH + H + Δ G = 3.7 kcal / mol glutamate+NAD++H2O⟶NH4++α-ketoglutarate+NADH+H+ΔG=3.7 kcal/mol L -malate + NAD + ⟶ oxaloacetate + NADH + H + Δ G = 29.7 kJ / mol -malate+NAD+⟶oxaloacetate+NADH+H+ΔG=29.7 kJ/mol C 6 H 13 O 9 P + ATP ⟶ C 6 H 14 O 12 P 2 + ADP Δ G = − 14.2 kJ / mol

Answer 1

Answer:

Explanation:

In spontaneous reaction , there is decrease in Gibb's free energy .( Δ G is negative ). Out of given reaction , following reactions have negative Δ G so they are spontaneous.

C ₂ H ₄ + H ₂ Rh ( I ) −−−→ C ₂ H ₆ ,  Δ G = − 150.97 kJ / mol

C ₆ H₁₃O₉ P + ATP ⟶ C ₆ H₁₄ O₁₂ P₂ + ADP ,  Δ G = − 14.2 kJ / mol