Calculate the charge passed when 0.200 A flows for 5.00 minutes.
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The Faraday constant is
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A current of 2.00 A passes through CuSO₄(aq) for 965 s. Calculate the mass of copper deposited (g). Cu 63.5, F = 96 500.
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Calculate the Avogadro constant (×10²³ mol⁻¹) from F = 96 500 C mol⁻¹ and e = 1.60 × 10⁻¹⁹ C.
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During electrolysis of concentrated NaCl(aq), the product at the cathode is
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During electrolysis of very dilute NaCl(aq), the main anode product is
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The same charge passes through Ag⁺(aq) and Cu²⁺(aq) cells in series. The ratio of moles Ag : Cu deposited is
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During electrolysis of CuSO₄(aq) with inert electrodes, the cathode product is
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To find L by electrolysis, you must measure
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How long (s) must a 0.500 A current flow to deposit 1.08 g of silver? ( Ag 108)
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What volume (cm³ at r.t.p.) of oxygen is produced at the anode when 0.400 A flows for 9650 s through dilute H₂SO₄?
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What mass (g) of aluminium is produced by 1.00 × 10⁵ C? ( Al 27.0)
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