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5 marksElectrochemistry

CSEC Chemistry · May/June 2018 · Paper 2 · Question 4(c)

A sample of molten lead bromide, PbBr₂, is electrolysed for three minutes with a current of 6 amperes. Calculate the mass of lead that is deposited at the cathode, given that two moles of electrons are required to liberate one mole of lead as shown in the following equation: Pb²⁺(l) + 2e⁻ → Pb(l) [Q = It; RAM: Pb = 207; F = 96 500 C mol⁻¹]

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Other parts of this question

  1. 4(a)Define 'electrolysis'.[2 marks]
  2. 4(b)(i)Solid sodium chloride[2 marks]
  3. 4(b)(ii)1 mol dm⁻³ hydrochloric acid[2 marks]
  4. 4(b)(iii)Ethanol[2 marks]
  5. 4(b)(iv)A bar of lead touching the electrodes[2 marks]

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