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(a) Steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes $FeSO_{4}$ and $ZnSO_{4}$ untill 2.8g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass Zn deposited at the cathode of cell Y.

(molar mass : Fe = 56 g mol^-1, Zn = 65.3 g mol^-1, 1F = 96500C mol^-1)

(b) In the plot of molar conductivity $(\wedge _{m})$ vs square root concentration $(c^{\frac{1}{2}})$ , following curves are obtained for two electrolytes A and B:

Answer the following:

(i) Predict the nature of electrolyte A and B.

(ii) What happens on extrapolation of $\wedge _{m}$ to concentration approaching zero for electrolytes A and B?

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