Question:
Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2$ Faraday electricity through an aqueous solution of potassium succinate, the total volume of gases (at both cathode and anode) at STP ($1\, atm$ and $273\, K$) is :
Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing $0.2$ Faraday electricity through an aqueous solution of potassium succinate, the total volume of gases (at both cathode and anode) at STP ($1\, atm$ and $273\, K$) is :
Updated On: Jul 20, 2024
- $2.24\, L$
- $4.48\, L$
- $6.72\, L$
- $8.96\, L$
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The Correct Option is D
Solution and Explanation
Total equivalents of $C_{2}H_{4}+CO_{2}+H_{2} = 0.2+0.2+0.2 = 0.6$
Total moles of gases $= \frac{0.2}{2}+\frac{0.2}{1}+\frac{0.2}{2} = 0.4$
$v = \frac{nRT}{P} = \frac{0.4\times0.0821\times273}{1}$
$= 8.96\,L$
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Concepts Used:
Electrolysis
Electrolysis:
Electrolysis is the process by which an element is decomposed and undergoes some chemical change under the influence of any electric current. The first-ever electrolysis was executed out by Sir Humphrey Davey in the year 1808. Electrolysis can occur in both Galvanic cells and Electrolytic cells.
Applications of Electrolysis:
- Electrolytic cells are used for the production of Hydrogen and Oxygen gas from water.
- They are used for the large-scale production of pure metals like sodium, copper, magnesium, etc.
- They are used to extract Aluminium from Bauxite.
- Electrolytic cells are used for electroplating, a process by which a thin protective layer of one metal is formed over another metal, mostly for protection.
- Electrolysis is used for the electrorefining of non-ferrous metals.
Read More: Products of Electrolysis