The negative Zn pole of Daniell cell, sending a constant current through a circuit, decreases in mass by 0.13 gin 30 min. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is

Question

The negative Zn pole of Daniell cell, sending a constant current through a circuit, decreases in mass by 0.13 gin 30 min. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is (A) 0.180 g (B) 0.141 g (C) 0.126 g (D) 0.242 g

Tardigrade Admin · Accepted Answer

According to Faradays law of electrolysis, m=zit (mZn/mCu)=(zZn/zCu) ∴ (0.13/mCu)=(32.5/31.5) mCu=0.126 g

Q. The negative Zn pole of Daniell cell, sending a constant current through a circuit, decreases in mass by 0.13 gin 30 min. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is

0.180 g

0.141 g

0.126 g

0.242 g

According to Faradays law of electrolysis, $m = z i t$ $\frac{m _{Z n}}{m _{C u}} = \frac{z _{Z n}}{z _{C u}}$ $∴$ $\frac{0.13}{m _{C u}} = \frac{32.5}{31.5}$ $m_{C u} = 0.126 g$

Q. The negative Zn pole of Daniell cell, sending a constant current through a circuit, decreases in mass by 0.13 gin 30 min. If the electrochemical equivalent of Zn and Cu are 32.5 and 31.5 respectively, the increase in the mass of the positive Cu pole in this time is

0.180 g

0.141 g

0.126 g

0.242 g

According to Faradays law of electrolysis, m=zit mCu​mZn​​=zCu​zZn​​ ∴ mCu​0.13​=31.532.5​ mCu​=0.126g

According to Faradays law of electrolysis, $m = z i t$ $\frac{m _{Z n}}{m _{C u}} = \frac{z _{Z n}}{z _{C u}}$ $∴$ $\frac{0.13}{m _{C u}} = \frac{32.5}{31.5}$ $m_{C u} = 0.126 g$