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Calculate the standard free-energy change at 25°C for the following reaction.
3Cu(s) + 2NO3(aq) + 8H+ (aq) 3Cu²+ (aq) + 2NO(g) + 4H₂O(1).
Use standard reduction electrode potentials.

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From the calculation, the standard free energy of the system is -359kJ.

What is the standard free-energy?

The  standard free-energy is the energy present in the system. We have to first obtain the cell potential using the formula;

Ereduction - E oxidation = 0.96 V - 0.34 V = 0.62 V

Using the formula;

ΔG = -nFEcell

ΔG =-(6 * 96500 * 0.62)

ΔG =-359kJ

Learn more about free energy:https://brainly.com/question/15319033

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