JEE Main 2014 · 12 Apr · Shift 1 · Chemistry Q36

← JEE Main 2014 · 12 Apr · Shift 1

ChemistrySingle correct+4 / -1Question 36 of 90

How many electrons would be required to deposit 6.35 g of copper at the cathode during the electrolysis of an aqueous solution of copper sulphate ? (Atomic mass of copper = 63.5 u, $N_A$ = Avogadro's constant) :

\dfrac{N_A}{20}

\dfrac{N_A}{10}

\dfrac{N_A}5

\dfrac{N_A}2

Answer and worked solution

Official answer: C

6.35 g is 0.1 mol Cu. $\ce{Cu^2+ + 2e- -> Cu}$ needs 0.2 mol electrons $=\dfrac{N_A}5$ .

Topics:Electrolysis and Faraday's laws

← Previous question Next question →

JEE Main 2014 · 12 Apr · Shift 1, Chemistry question 36