AP EAMCET · Chemistry · Electrochemistry

$38.6$ amperes of current is passed for $100$ seconds through an aqueous ${CuSO}_{4}$ solution using platinum electrodes. The mass of copper consumed from the solution and volume of gas liberated at STP are respectively (molar mass of $Cu = 63.54 {gmol}^{- 1}$ )

A $26.37 g, 0.448 L$
B $0.63 g, 0.224 L$
C $1.27 g, 0.224 L$
D $4 g, 0.448 L$

Verified Solution

Answer & Solution

Correct Answer

(C) $1.27 g, 0.224 L$

Step-by-step Solution

Detailed explanation

Reduction potential of Cu2+ is higher than H+ hence Cu2+ will be reduced at cathode more easily. Reaction at the cathode: Cu+2+2e-→Cu Reaction at the Anode: 2H2O→O2+4H++4e- According to Faraday's first law W=Zit…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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38.6 amperes of current is passed for 100 seconds through an aqueous CuSO4 solution using platinum electrodes. The mass of copper consumed from the solution and volume of gas liberated at STP are respectively (molar mass of Cu=63.54 gmol-1)

Step-by-step Solution

$38.6$ amperes of current is passed for $100$ seconds through an aqueous ${CuSO}_{4}$ solution using platinum electrodes. The mass of copper consumed from the solution and volume of gas liberated at STP are respectively (molar mass of $Cu = 63.54 {gmol}^{- 1}$ )