We’re being asked to calculate for the time mass of nickel metal plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes.
NiCl2(aq) is subjected to electrolysis. It will break up in the solution:
NiCl2(aq) → Ni2+(aq) + 2 Cl-(aq)
Nickel metal are plated out:
Ni2+(aq) → Ni(s)
• Ni2+ needs to gain 2 electrons to become Ni(s):
Ni2+(aq) + 2 e- → Ni(s)
We can now calculate the mass of Ni(s) plated out.
How many grams of nickel metal are plated out when a constant current of 15.0 A is passed through aqueous NiCl2 for 60.0 minutes? Enter your answer with one decimal place and no units.
a. 0.3 g
b. 16.4 g
c. 0.5 g
d. 32.8 g
e. 65.7 g
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What scientific concept do you need to know in order to solve this problem?
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