Moles of chromium would be electroplated by passing a current of 5.2 amperes through a solution of Cr2(SO4)3 for 45.0 minutes is 0.0484974 mole.
Divide the mass of the material via its molar mass. The molar mass of a substance is the mass in grams of 1 mole of that substance. This mass is given via the atomic weight of the chemical unit that makes up that substance in atomic mass units. One mole is defined as the quantity of substance containing as many primary entities (atoms, molecules, ions, electrons, radicals, and many others
Consider the reaction : Cr+3 (aq) + 3 e- =======> Cr (s)
3 moles of electrons are needed to electroplate 1 mole of chromium
= 3 ×96500 = 289500 C/mol
Quantity of electricity passed = i×t
= 5.2 ×45 min×60 sec = 14040 C
Hence, the number of mole of Cr deposited = 14040 C / 289500 C /mol = 0.0484974 mole
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