Answer:
(i) Δ = <u>-4.07v</u>
(ii)Δ = <u>+785.510 KJ</u>
(iii)<u> The reaction is for an electrolytic cell</u>
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Explanation:
In this question, we are tasked with calculating Δ and Δ for the reaction and determine if the reaction is for a voltaic or electrolytic cell.
We proceed as follows;
Firstly, we write the complete equation of reaction as shown below;
+ → +
We can see that chlorine goes from a negative state to zero state. This is indicative of loss of electron which is defined as <u>oxidation</u>
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We can also see that sodium went from a positive state to zero state which is indicative of electron gain which is defined as <u>reduction</u>
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Mathematically, the value of Δ for the reaction can be calculated using the formula below;
Δ = Δ - Δ = -2.71v - 1.36v = -4.07V
The value of Δ can be calculated as follows;
Δ = -nFΔ
Where n = 2 and F is 96,500C . We plug these values to get;
Δ = -2 × 96,500C× -4.07V = 785,510J = 785.510KJ (1KJ = 1000J)
Now, we answer if this reaction is for a voltaic or an electrolytic cell;
It is for an <u>electrolytic cell </u>because electrons flow from cathode to anode as indicated by magnitude of the Δ(positive in value)