accountant current of 30 ampere is passed through an aqueous solution of NaCl for a timer of 1 hour how many grams of NIOS 6 produce what is the volume of cl2 gas at STP produced
Answers
Vasudevan Ans, former Retired Professor of Chemistry at Chemistry Professor (1977-2014)
Answered Nov 12, 2018 · Author has 1.8k answers and 434k answer views
2NaCl ———Electrolysis —→2Na+ +2Cl-
At anode 2Cl- —-±>Cl2+2e-
At cathode 2Na+ +2e- ——-> 2Na.
So 2 Faraday of electricity is required to liberate 1 mole = 22.4 liters of Cl2 at STP.
Amount of current passed
= 30 x 60 x 60=108000 coulombs.
So 108000 coulombs will liberate =108000/(96500 x2) = 0.5596 moles Cl2.
No.of liters of Chlorine liberated at STP
= 0.5596 x 22.4 = 12.53 liters.
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OTHER ANSWERS
Prakash Kulkarni, lives in Savedi, Ahmednagar (1992-present)
Answered Jul 19, 2018 · Author has 544 answers and 134.1k answer views
First of all there will be no evolution of Cl2.
Instead for an aqeous solution evolved gas is O2.
according to Faradays first law
Volume (in L)= 8/96487 *30 *3600*22.4/32.
For the evolution of Cl2, one has to use molten/ fused NaCl as an electrolyte & appropriate experimental set- up.
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Rizul Thakur, Student at JEE Coaching (2017-present)
Answered Jul 21, 2018
2H+ + 2e === H2(g) Cathode
2Cl-=== Cl2(g) + 2e- Anode
2Faraday Charge Produces 22.4L Cl2
1 Faraday Produces 11.2L Cl2
30*60*60/96500 Faraday Charge Will Produce 12.53L Of Cl2 At STP!
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