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Solution - 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 - Electrolytic Cells and Electrolysis - Introduction

Question

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 -

  1. 2098
  2. 96500
  3. 193000
  4. 4196

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?

APPEARS IN

2014-2015 (March)
Question 1.4 | 1 mark
Solution for question: 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 concept: Electrolytic Cells and Electrolysis - Introduction. For the courses HSC Science (Computer Science), HSC Science (Electronics), HSC Science (General)
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