Problem: What is the ΔG (kJ/mol) for a reaction at 25 Celsius that is: Mg3(PO4)2 (s) → 3 Mg2+(aq) + 2 PO43− (aq)       ΔG° = 137.0 kJ/mol If there is initially 0.65 M Mg2+ (aq) and 0.43 M PO43−(aq) in solution? A. 129.6 B. 134.0 C. 137.0 D. 140.0 E. 144.4

FREE Expert Solution
100% (447 ratings)
Problem Details

What is the ΔG (kJ/mol) for a reaction at 25 Celsius that is:

Mg3(PO4)2 (s) → 3 Mg2+(aq) + 2 PO43− (aq)       ΔG° = 137.0 kJ/mol

If there is initially 0.65 M Mg2+ (aq) and 0.43 M PO43−(aq) in solution?

A. 129.6

B. 134.0

C. 137.0

D. 140.0

E. 144.4

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofWhat is the ΔG (kJ/mol) for a reaction at 25 Celsius that is...as high difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Dasha took 5 minutes and 59 seconds to solve this problem. You can follow their steps in the video explanation above.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Kautz's class at UNL.