Respuesta :
Answer:
The spontaneous reactions are:
B. [tex]C_{2}H_{4} + H_{2} \overset{Rh(I)}{\rightarrow}C_{2}H_{6}[/tex] ; 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. [tex]C_{2}H_{4} + H_{2} \overset{Rh(I)}{\rightarrow}C_{2}H_{6}[/tex] ; 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.
