A particular voltaic cell operates with the reaction: Zn (s) + Cl2 (g) - -->Zn^2 + (aq) + 2Cl^ - (aq) giving a cell potential of. 853 V. Calculate the amount of energy liberated from the cell when 20.0g of zinc metal is consumed?

Question

Nathan Blackburn

Chemistry

27 February, 02:02

A particular voltaic cell operates with the reaction: Zn (s) + Cl2 (g) - -->Zn^2 + (aq) + 2Cl^ - (aq) giving a cell potential of. 853 V. Calculate the amount of energy liberated from the cell when 20.0g of zinc metal is consumed?

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Answers (1)

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Angel Velasquez · Answer 1

The amount of energy liberated will be 49.38 J.

Explanation:

The amount of energy liberated (gibbs free energy) can be calculated using the following equation:

ΔG° = - nFε

n: amount of moles of electrons transfered

F: Faraday's constant

ε: cell potential

20.0 g of Zn is equal to 0.30 mol.

Two electrons are transfered during the reaction.

Therefore, n = 2x0.30 ∴ n = 0.60

ΔG° = - 0.60 x 96.485 x 0.853

ΔG° = 49.38 J