A steady current of 1.5 A flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is 30 × 10-5 g C -1, the mass of copper deposited on the electrode will be

Question

A steady current of 1.5 A flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is 30 × 10-5 g C -1, the mass of copper deposited on the electrode will be (A) 0.40 g (B) 0.50 g (C) 0.67 g (D) 0.27 g

Tardigrade Admin · Accepted Answer

If m is the mass of a substance deposited or liberated at an electrode during electrolysis when a charge q passes through electrolyte, then according to Faraday's first law of electrolysis, m propto q or m=z q where z is a constant of proportionality and is called electrochemical equivalent (ECE) of the the substance. If an electric current I flows through the electrolyte, then q =I t ∴ m =z i t Here, i=1.5 A , t =10 min =10 × 60 s, z =30 × 10-5 gC -1 Hence, mass of copper deposited on the electrode m =30 × 10-5 × 1.5 × 10 × 60 =27 × 10-2=0.27 g

Q. A steady current of 1.5A flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is 30×10−5gC−1, the mass of copper deposited on the electrode will be

0.40 g

0.50 g

0.67 g

0.27 g

Q. A steady current of $1.5 A$ flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is $30 \times 1 0^{- 5} g C^{- 1}$ , the mass of copper deposited on the electrode will be