Question

Problem 12. The change in Gibbs energy that accompanies the oxidation of glucose to carbon dioxide and water vapor at 25.00℃ is −2808 kJ mol−1. How much glucose does a person of mass 89.43 kg need to consume to climb through 13.5m?

Answer 1

Assume that the "free energy" used by the person to climb (work) is that of the Gibbs free energy

Make an energy balance

Potential energy Etotal = mass * gravity * height

Potential energy Etotal = 89.43 kg * 9.8 m/s2 * 13.5 m = 11831.589 J

now...

from the combustion:

1 mol --> 2808 kJ

x mol --> 11831.589 J = 11.831 kJ

x = 11.831 /2808

x = 0.004213 mol of glucose required

mass = mol*MW = 0.004213*180

mass of glucose = 0.75834 g required to climb 13.5 m