The tarnish that forms on objects made of silver is solid silver sulphide. This can be removed by reacting it with aluminium met
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The of the voltaic cell is 0.743 V. The ΔG°of the given cell is -143.377 kJ and K is 1.35 × 10²⁵
A voltaic cell often called a galvanic cell, is an electrochemical device that produces electricity through spontaneous redox processes.
It is divided into two distinct half-cells. A half-cell is made up of an electrode (a metal strip, M) dissolved in a solution containing Mn⁺ ions. M can be any metal.
A wire from one electrode to the other connects the two half-cells. Additionally, a salt bridge links the two half-cells.
To solve the question, we need to write the equations of two half-cells
At the anode, oxidation occurs
E° = -0.403 V
At the cathode, reduction occurs
E° = 0.34 V
Overall reaction:
We know
= 0.34 -(-0.403) = 0.743 V
Also,
ΔG° = -nF
Where, n = no of electrons gained or lost
F = Faraday constant
= standard potential
ΔG° = -2×96485×0.743 = -143376.71 J = -143.377 kJ
Also,
ΔG° = -RTlnK
-143.377 = -8.314 × 10-3 × 298 × lnK
lnK = 57.87
K = 1.35 × 10²⁵
Hence, The of the voltaic cell is 0.743 V. The ΔG°of the given cell is -143.377 kJ and K is 1.35 × 10²⁵
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The percent yield is 71.3 %.
Explanation:
Percent yield is the measure to analyze the success percentage of any experiment .The percent yield of any experiment can be obtained by the ratio of actual or experimental value to expected or theoretical value multiplied with 100.
So, in the present problem, we have obtained 10.7 g of adamantium nitrate from Wolverine's 10 pound claws. So the actual value or the experimental value is the amount of adamantium nitrate obtained from Wolverine's claws.
Thus, the experimental outcome is 10.7 g. While we had expected to recover 15 g of adamantium nitrate. So the theoretical outcome is 15 g.
Thus, the percent yield is 71.3 %.