How long (hrs) must a current of 2.5 amps flow to produce 10 g of Cu from a 0.15

Question

How long (hrs) must a current of 2.5 amps flow to produce 10 g of Cu from a 0.1500 M solution of CuCl2? 8.4 214 3.4 203 340 Identify the correct relationships. When K > 1, the reaction is spontaneous When AG 0, the reaction is spontaneous i and ii iii only i and iii ii only i, ii, and iii Which one of the following statements about electrochemical cells is correct? In a salt bridge, current is carried by cations moving toward the anode, and anions toward the cathode. In the external wire, elections travel from cathode to anode. The anode of a voltaic cell is labeled minus (-). Oxidation occurs at the cathode in an electrolytic cell. The change in free energy, delta G degree, is negative for an electrolytic cell.

Explanation / Answer

1) In CuCl2 , equivalent mass of Cu = molar mass/2   = 63.5/2 = 31.75 g   (as Cu exists as Cu2+)

Thus, number of equivalents of Cu in 10 g of it = 10/31.75 = 0.315

Now, as per faraday's law, charge in culombs required to deposit 1 equivalent of Cu2+ = 96500 C

thus, charge required to deposit 0.315 equivalent of Cu2+ = 0.315*96500 = 30393.7 C

Now, current = charge/time in sec

or, time in sec = charge/current = 30393.7/2.5 = 12157.48 sec

or, time in hours = time in sec/3600 = 3.377 hrs.

Thus, the correct option is C

2) All 3 statements are correct

So the correct option is E

3)The correct option is:- C

At anode oxidation occurs , so the electrons travels from anode to cathode

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