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The number of Faradays (F) required to produce 20g of calcium from molten CaCl2 (Atomic mass of Ca = 40 g mol–1) is:
- a)3
- b)4
- c)1
- d)2
Correct answer is option 'C'. Can you explain this answer?
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The number of Faradays (F) required to produce 20g of calcium from mol...
EquivalentCa = Equivalentcurrent
⇒ No. of Faradays =
⇒ No. of Faradays = 1
⇒ No. of Faradays =
⇒ No. of Faradays = 1
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The number of Faradays (F) required to produce 20g of calcium from mol...
-1)
The balanced chemical equation for the electrolysis of molten CaCl2 is:
Ca2+ + 2e- → Ca
For every mole of Ca2+ ions reduced, 2 moles of electrons are required. The charge carried by 1 mole of electrons is 1 Faraday (F).
The molar mass of CaCl2 is 111 g mol-1, which means that 1 mole of CaCl2 contains 1 mole of Ca2+ ions. Therefore, the number of moles of Ca2+ ions required to produce 20 g of calcium is:
20 g / 40 g mol-1 = 0.5 mol
Since 1 mole of Ca2+ ions requires 2 moles of electrons, the total number of moles of electrons required is:
2 x 0.5 mol = 1 mol
The charge carried by 1 mole of electrons is 1 Faraday (F), so the number of Faradays required to produce 20 g of calcium is:
1 F/mol x 1 mol = 1 F
Therefore, 1 Faraday (F) is required to produce 20 g of calcium from molten CaCl2.
The balanced chemical equation for the electrolysis of molten CaCl2 is:
Ca2+ + 2e- → Ca
For every mole of Ca2+ ions reduced, 2 moles of electrons are required. The charge carried by 1 mole of electrons is 1 Faraday (F).
The molar mass of CaCl2 is 111 g mol-1, which means that 1 mole of CaCl2 contains 1 mole of Ca2+ ions. Therefore, the number of moles of Ca2+ ions required to produce 20 g of calcium is:
20 g / 40 g mol-1 = 0.5 mol
Since 1 mole of Ca2+ ions requires 2 moles of electrons, the total number of moles of electrons required is:
2 x 0.5 mol = 1 mol
The charge carried by 1 mole of electrons is 1 Faraday (F), so the number of Faradays required to produce 20 g of calcium is:
1 F/mol x 1 mol = 1 F
Therefore, 1 Faraday (F) is required to produce 20 g of calcium from molten CaCl2.
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The number of Faradays (F) required to produce 20g of calcium from molten CaCl2 (Atomic mass of Ca = 40 g mol–1) is:a)3b)4c)1d)2Correct answer is option 'C'. Can you explain this answer?
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