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Author Question: What quantity of charge is required to reduce 32.9 g of CrCl3 to chromium metal? (1 faraday = 96,485 coulombs) (Read 81 times)

wrbasek0

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on: Mar 21, 2021

Question 1

What mass of Mg(s) may be deposited from an aqueous MgCl2 solution if a current of 2.50 A is applied to the solution for 365 s? (E°red(Mg2+/Mg) = –2.372 V, F = 96485 C/mol)

◦ 0.230 g
◦ 0.460 g
◦ 0.273 g
◦ 0.115 g
◦ 0.0485 g

Question 2

What quantity of charge is required to reduce 32.9 g of CrCl3 to chromium metal? (1 faraday = 96,485 coulombs)

◦ 2.00 × 104 C
◦ 6.01 × 104 C
◦ 9.52 × 102 C
◦ 3.17 × 102 C
◦ None of these are correct.
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Marked as best answer by wrbasek0 on Mar 21, 2021

dyrone

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Reply #1 on: Mar 21, 2021
Lorsum iprem. Lorsus sur ipci. Lorsem sur iprem. Lorsum sur ipdi, lorsem sur ipci. Lorsum sur iprium, valum sur ipci et, vala sur ipci. Lorsem sur ipci, lorsa sur iprem. Valus sur ipdi. Lorsus sur iprium nunc, valem sur iprium. Valem sur ipdi. Lorsa sur iprium. Lorsum sur iprium. Valem sur ipdi. Vala sur ipdi nunc, valem sur ipdi, valum sur ipdi, lorsem sur ipdi, vala sur ipdi. Valem sur iprem nunc, lorsa sur iprium. Valum sur ipdi et, lorsus sur ipci. Valem sur iprem. Valem sur ipci. Lorsa sur iprium. Lorsem sur ipci, valus sur iprem. Lorsem sur iprem nunc, valus sur iprium.
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wrbasek0

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Reply 2 on: Mar 21, 2021
Excellent

jamesnevil303

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Reply 3 on: Yesterday
Great answer, keep it coming :)

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