Question #44896

A non-aqueous electrolytic cell at $298 \text{ K}$ contains a solution of Uranium salts where the actinoid exists as a mixture of $U^{3+}$ and $U^{4+}$ ions in a $1:1$ molar ratio. A constant current of $19.3 \text{ A}$ is passed through the cell for $5000 \text{ s}$ to deposit solid Uranium ($\ce{U_{(s)}}$) at the cathode. Due to ion-pairing and solvent interactions in the non-aqueous medium, the current efficiency for the cathodic deposition is $75\%$. Assuming both $U^{3+}$ and $U^{4+}$ are reduced to $\ce{U_{(s)}}$ simultaneously at rates proportional to their bulk mole fractions, calculate the mass of Uranium deposited. \n\n(Given: Faraday's constant $F = 96500 \text{ C mol}^{-1}$, Atomic mass of $U = 238 \text{ g mol}^{-1}$)