Based on your energy level calculations, predict the photon energies that would be emitted by transitions between the hydrogen e
1 answer:
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Answer:
The spontaneous reactions are:
B. ; <u>ΔG= −150.97 kJ/mol </u>
D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; <u>ΔG = −14.2 kJ/mol </u>
Explanation:
Gibbs free energy , denoted by ΔG, is the <u>quantitative measure of the favorability or spontaneity</u> 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 <u>spontaneous or favorable</u>, ΔG should be negative (ΔG < 0).
A. DHAP ⇌ glyceraldehyde-3-phosphate ; <u>ΔG = 3.8 kJ/mol </u>
<u>The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.</u>
B. ; <u>ΔG= −150.97 kJ/mol </u>
<u>The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.</u>
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C. glutamate + NAD⁺ + H₂O ⟶ NH⁴⁺ +α-ketoglutarate + NADH + H⁺ ; <u>ΔG = 3.7 kcal/mol </u>
<u>The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.</u>
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D. C₆H₁₃O₉P + ATP ⟶ C₆H₁₄O₁₂P₂ + ADP; <u>ΔG = −14.2 kJ/mol </u>
<u>The value of ΔG is negative (ΔG < 0). Therefore, this reaction is spontaneous.</u>
<u />
E. L -malate + NAD⁺ ⟶ oxaloacetate + NADH + H⁺; <u>ΔG = 29.7 kJ/mol </u>
<u>The value of ΔG is positive (ΔG > 0). Therefore, this reaction is not spontaneous.</u>