(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO₄and ZnSO₄ until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y. (Molar mass: Fe = 56 g mol^–1 Zn = 65.3 g mol^–1, 1F = 96500 C mol^–1)

(b) In the plot of molar conductivity (𝛬_m) vs square root of concentration (c^1/2), following curves are obtained for two electrolytes A and B

Question

(a) A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO₄and ZnSO₄ until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y. (Molar mass: Fe = 56 g mol^–1 Zn = 65.3 g mol^–1, 1F = 96500 C mol^–1)

(b) In the plot of molar conductivity (𝛬_m) vs square root of concentration (c^1/2), following curves are obtained for two electrolytes A and B

Infinity Learn · Accepted Answer

(a) I =2 Ampere56 g of Fe requires =2× 96500 C∴2.8 g will require =2.8×2×9650056=9650 CQ=Itt=QI=96502=4825 sUsing Faraday's second law of electrolysisw1w2=E1E2Where w1 = mass of Fe and w2= mass of Zn2.8w2=562×265.3w2=3.265g(b) (i) A is a strong electrolyte and B is a weak electrolyte. (ii) For B, 𝛬m value at zero concentration cannot be obtained by extrapolation as it is a weak electrolyte. For A, the intercept will give the 𝛬m value at zero concentration.

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