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jjaheimhicks3419
26.07.2019 •
Chemistry
How many grams of chromium metal are plated out when a constant current of 8.00 a is passed through an aqueous solution containing cr3+ ions for 160. minutes?
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Ответ:
Cr³⁺(aq) + 3e⁻ --> Cr(s)
This means that for every 3 moles of electron transferred, 1 mole of Chromium metal is plated. The molar mass of Cr: 52 g/mol. The solution is as follows:
Mass of Chromium metal = (8 C/s)(60 s/1 min)(160 min)(1 mol e⁻/96,500 C)(1 mol Cr/3 mol e)(52 g/mol)
Mass of Chromium metal = 13.79 g
Ответ: