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 40.0 minutes? A)3.45 g B)6.15 g C)10.3 g D)31.0 g

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Quizplus · Accepted Answer

The amount of metal plated out is given by the equation:$$m = \frac{It}{nF}$$where:* m is the mass of metal plated out (in grams)* I is the current (in amperes)* t is the time (in seconds)* n is the number of electrons transferred per metal ion* F is the Faraday constant (96,485 C/mol)In this problem, we have:* I = 8.00 A* t = 40.0 min = 2400 s* n = 3 (for Cr³⁺)* F = 96,485 C/molSubstituting these values into the equation, we get:$$m = \frac{(8.00 A)(2400 s)}{(3)(96,485 C/mol)} = 3.45 g$$Therefore, the correct answer is A) 3.45 g.

How Many Grams of Chromium Metal Are Plated Out When