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Molten potassium chloride was electrolysed. at the end of the electrolysis, 7.8 g of potassium had been deposited at the cathode. what volume of chlorine gas was given off at the anode? ( k = 39 1 mole of any gas occupies 24 000 cm³)
Accepted Answer
Here's how to solve this problem:
1. Calculate moles of potassium:
Moles of potassium = mass / molar mass = 7.8 g / 39 g/mol = 0.2 mol
2. Stoichiometry:
The balanced chemical equation for the electrolysis of potassium chloride is:
2KCl(l) → 2K(l) + Cl₂(g)
The equation shows that 2 moles of potassium are produced for every 1 mole of chlorine gas.
3. Calculate moles of chlorine gas:
Moles of chlorine gas = (0.2 mol potassium) / 2 = 0.1 mol Cl₂
4. Calculate volume of chlorine gas:
Volume of chlorine gas = (0.1 mol Cl₂)
(24,000 cm³/mol) = 2400 cm³
Therefore, 2400 cm³ of chlorine gas was given off at the anode.
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