asked by @juanj10 •
over 1 year ago •
Chemistry
• 5 pts

Estimate the free-energy change for the combustion of glucose at body temperature (37ºC) using the data given if the phosphorylation of one mole of ADP^3- involves free energy change of +30.5kJ, about how many moles of ATP^4- could be made from the combustion of one mole of C8H12O6, assuming no energy loss?

Susbtance Delta Hºf (Kj/mol) S^+(J/mol*K) C6H12O6(s) -1274.4 212.1 O2(g) 205.0 CO2(g) -393.5 213.8 H2O(l) -285.8 69.9

Hey! So this problem is a bit tricky. The first thing you have to do is find the balanced chemical equation. This will help you find Delta G. In order to find Delta G, you must find Delta H and Delta S of the reaction first. Find these two values as shown below. Then, you will plug them into the equation to find Delta G. Remember that the temperature is 37 degrees Celsius, but you must convert it to Kelvin, so you add 273 and get 310 degrees Kelvin. This is what you plug into the Delta G equation. Delta G should now give you -2882.031 kJ. The problem tells you that it takes 30.5 kJ to make 1 mole of ATP, so you just use a conversion factor to figure out how many moles of ATP you can make with the energy that you calculated (the -2882.031 kJ). We assume here a positive value so that we could have a positive number of moles of ATP (since a negative value wouldn't make sense). We end up getting 94.5 moles of ATP. Hope this helped!! Let us know if you have any other questions.

answered by @sabrina •
over 1 year ago

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