Which of the reactions are spontaneous (favorable)? a. dhap↽−−⇀glyceraldehyde-3-phosphateδ =3.8 kj/mol b. c2h4+h2−→−−rh(i)c2h6δ=−150.97 kj/mol c. glutamate+nad++h2o⟶nh+4+α-ketogluta rate+nadh+h+δ=3.7 kcal/mol d. c6h13o9p+atp⟶c6h14o12p2+adpδ=−14.2 kj/mol e. l -malate+nad+⟶oxaloacetate+nadh+h+δ= 29.7 kj/mol

The spontaneous reactions are:

B. ; ΔG= −150.97 kJ/mol  

D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; ΔG = −14.2 kJ/mol  

Explanation:  

Gibbs free energy , denoted by ΔG, is the quantitative measure of the favorability or spontaneity of a given process or chemical reaction that is carried out at constant temperature (T) and pressure (P).

Therefore, Gibbs free energy in J: ΔG = ΔH - TΔS

Here, ΔH is the change in enthalpy and ΔS is the change in the entropy

For a given chemical reaction to be spontaneous or favorable, ΔG should be negative (ΔG < 0).

A. DHAP ⇌ glyceraldehyde-3-phosphate ; ΔG = 3.8 kJ/mol  

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

B. ; ΔG= −150.97 kJ/mol  

 The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.

C. glutamate + NAD⁺ + H₂O ⟶ NH⁴⁺ +α-ketoglutarate + NADH + H⁺ ; ΔG = 3.7 kcal/mol  

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; ΔG = −14.2 kJ/mol  

 The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.

E. L -malate + NAD⁺ ⟶ oxaloacetate + NADH + H⁺; ΔG = 29.7 kJ/mol

The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.

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