If 96500C of charge flows through a circuit for 10 seconds what is the amount of current in milli ampere ?
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Class 12
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>>A current of 10.0 A flows for 2.00 hrs t
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A current of 10.0 A flows for 2.00 hrs through an electrolytic cell containing a molten salt of metal X. This results in the decomposition of 0.250 mol of metal X at the cathode. The oxidation state of X in the molten salt is:(F=96500C)
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Correct option is C)
t=2×60×60=7200s
Charge = current time =10 A×7200 s=72000 C
According to the reaction: X
n+
(aq.)+ne
−
→X(s)
We require nF or n96500 C to deposit 1 mol of X.
For 0.25 mole of deposition we require n×24125 C.
Hence, n=
24125
72000
=3
Answer:
3
Explanation:
t=2×60×60=7200s
Charge = current time =10 A×7200 s=72000 C
According to the reaction: X
n+
(aq.)+ne
−
→X(s)
We require nF or n96500 C to deposit 1 mol of X.
For 0.25 mole of deposition we require n×24125 C.
Hence, n=
24125
72000
=3