A current of 0.500 A is passed for 32 min 10 s through aqueous AgNO3 with platinum electrodes. Take F = 96500 C mol^-1, N_A = 6.02x 10^23, Ag = 108, Cu = 63.5, molar volume at STP = 22.4 L. Which statements are correct?

About 6.02x 10^21 electrons flow through the cell

The same charge passed through aqueous CuSO4 would deposit 0.3175 g of copper

The same charge passed through acidified water would liberate 224 mL of H2 at STP

About 6.02x 10^21 electrons flow through the cell

The same charge passed through aqueous CuSO4 would deposit 0.3175 g of copper

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3ec141

A current of $0.500 A$ is passed for $32 min 10 s$ through aqueous $AgNO X_{3}$ with platinum electrodes. Take $F = 96500 C mo l^{- 1}$ , $N_{A} = 6.02 \times 1 0^{23}$ , Ag = 108, Cu = 63.5, molar volume at STP $= 22.4 L$ . Which statements are correct?

A $1.08 g$ of silver is deposited
BThe same charge passed through acidified water would liberate $224 mL$ of $H X_{2}$ at STP
CAbout $6.02 \times 1 0^{21}$ electrons flow through the cell
DThe same charge passed through aqueous $CuSO X_{4}$ would deposit $0.3175 g$ of copper

Time

= 1930 s

, so

Q = 0.500 \times 1930 = 965 C = 0.0100 mol

of electrons

= 0.0100 \times 6.02 \times 1 0^{23} = 6.02 \times 1 0^{21}

electrons; (C) correct.

Ag X^{+} + e X^{-} Ag

0.0100 \times 108 = 1.08 g

; (A) correct.

Cu X^{2 +} + 2 e X^{-} Cu

0.00500 \times 63.5 = 0.3175 g

; (D) correct.

2 H X^{+} + 2 e X^{-} H X_{2}

0.00500 mol

H X_{2} = 112 mL

at STP, not

224 mL

; (B) wrong.