Answer to Question #154191 in General Chemistry for Popoy

Question

C = (°F – 32) *5/9 °F = °C * 9/5 + 32 K = °C + 273

G = H - T S (Gibbs Formula)

Where: Delta H is change in Enthalpy, T is temperature (in Kelvin), and Delta S is change in entropy

1. Calculate the Gibbs free energy change ( G ) for the following chemical reaction:

ATP ADP + Pi

The reaction occurs at 65 °F, the change in heat (H) = 18,180 cal, and the change in entropy (S) = 86 cal/K.

2. Calculate the Gibbs free energy change (G) for the following chemical reaction:

glutamate + NH3 glutamine + H2O

The reaction occurs at 68 °F, the change in heat (H) = 4113 cal, and the change in entropy (S) = 2.6 cal/K.

3. Would either of the reactions above occur spontaneously? If so, which one(s) and why?

4. How does the Gibbs free energy in each of the two reactions change if the temperature were raised to normal body temperature (92.8 °F)?

5. Does an increase in reaction temperature make each of these reactions more or less likely to occur spontaneously? Explain your answer.

Answer 1

Dear Popoy , your question requires a lot of work, which neither of our experts is ready to perform for free. We advise you to convert it to a fully qualified order and we will try to help you. Please click the link below to proceed: Submit order