Login or Sign Up
Menu
Ask a New Question

How many moles of ATP must be converted to ADP by the reaction

ATP(aq) + H2O ---> ADP(aq) + HPO4-2(aq) + 2H+(aq) delta-G*= -31 kJ

to bring about a nonspontaneous biochemical reaction in which delta-G*= +372 kJ?

I did my work out like this..:
372 kJ x 1 mol/-31 kJ = -12 mol
But how can I get negative moles?? Is there a different way to do this problem?


You cant get an endothermic reaction from a exothermic reaction. Your basic reaction is exothermic. You are trying to get a +G, endothermic. Not possible. If you try the math,you get negative matter (neg moles).

So as an answer would I just say that it's not possible?

Absolutely! It's like trying to find a serious clown or a high five from a jellyfish - it's just not possible. In this case, you can't magically make an exothermic reaction become an endothermic one. So the answer is that it's simply not possible to bring about a nonspontaneous biochemical reaction with a delta-G* of +372 kJ using the given exothermic reaction. Sometimes, chemistry likes to play hard to get.

Yes, based on the information you provided, it is not possible to convert a spontaneous reaction with a negative delta-G* value to a nonspontaneous reaction with a positive delta-G* value using the given reaction. Therefore, it is not possible to determine the number of moles of ATP that would need to be converted to ADP.

Yes, based on the information given, it is not possible to achieve a nonspontaneous biochemical reaction with a ΔG* of +372 kJ using the exothermic reaction you mentioned. The conversion of ATP to ADP is an exothermic reaction with a ΔG* of -31 kJ, indicating that it is spontaneous. It is not possible to obtain a positive value for ΔG* from an exothermic reaction. Therefore, the desired reaction with a ΔG* of +372 kJ cannot be achieved using the conversion of ATP to ADP.