Regarding Textbook answers for Physical Chemistry for the Life Science (2nd edit

Question

Regarding Textbook answers for Physical Chemistry for the Life Science (2nd edition), Ch 2 Problem 9E, I do not understand why G is equal to -2,808kJ mol^-1? According to the Appendix 2A below, it's the H that is equal to -2,808 kJ mol^-1 rather than G! According to Appendix 2A, G is equal to -910kJ mol^-1. Can you explain that?

Here is the question:

Suppose when you exercise, you consume 100g of glucose and that all the energy released as heat remains at your body at 37°C. What is the change in entropy of your body?

Thanks,

Kate

Explanation / Answer

enthalpy of combustion of glucose = -2805 KJ/mol
molecular mass of glucose = 180g/mol
given mass = 100g
no. of moles = 100/180 = 0.556
energy released by given amount of glucose = 2805*0.556 = 1558.33
Temp of body = 273+37 = 310 K
Change in entropy = dQ/T = 1558.33/310 = 5.0269 KJ/K

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