Respuesta :
The value of ∆G° for 2Ag + Mn²⁺ ----- Mn + 2Ag⁺ is -79.1J. and for reaction Cl₂ + 2Br⁻ ----- Br₂ + 2Cl⁻ is -1.5 × 10^5J.
What is redox reaction?
The reaction in which both reduction and oxidation reaction take place simultaneously is known as redox reaction.
What is oxidation reaction?
The reaction in which a substance or compound or species looses its electron. In this reaction, oxidation state of an element increases.
What is reduction reaction?
The reaction in which a substance or compound or species accept thr electron. In this reaction, oxidation state of an element decreases.
Half cell reaction
at anode:
2Ag ----- 2Ag⁺ + 2e- E°(Al) = 0.80V
at cathode:
Mn²⁺ + 2e- ------ Mn E°(Cd) = -1. 19V
Multiplying equation (1) by 2 and equation second by 3, we get redox reaction
Redox reaction
2Ag + Mn²⁺ ----- Mn + 2Ag⁺
E° cell = E°(Al) - E°(Cd)
= -1.19 + 1.60
= 0.41V
∆G° = -2 × 96500 × 0.41
= -79.1kJ
b) at anode
Cl₂ ---- 2Cl⁻ + 2e- E°(I₂ ) = 1.36V
at cathode
2Br⁻ + 2e- ------- Br₂ E°(Br₂ ) = 1.07V
redox reaction:
Cl₂ + 2Br⁻ ----- Br₂ + 2Cl⁻
E° cell = E°(Br₂ ) - E°(I₂ )
= 2.14 - 1.36
= 0.78V
∆G° = -2 × 96500 × 0.78
= -1.5 × 10^5J
Thus, we calculated that ∆G° for 2Ag + Mn²⁺ ----- Mn + 2Ag⁺ is -79.1J. and for reaction Cl₂ + 2Br⁻ ----- Br₂ + 2Cl⁻ is -1.5 × 10^5J.
learn more about redox reaction:
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