The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is -
- 2098
- 96500
- 193000
- 4196
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Solution
(d) 4196
Moles of Na = 1.00/23.0 = 0.0435
Cathode-half reaction will be
Na+ + 1 e- → Na
It states that for every one Faraday consumed, one mole of Na is liberated.
This means to get 0.0435 moles, we need to use 0.0435 Faraday.
We know that
1 Faraday = 96500 coulomb
0.0435 Faraday = 4197.75 coulomb
So, the nearest option is 4196.
Is there an error in this question or solution?
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