Balance the following redox equation and determine how many electrons were transferred. #Zn(s) + Ni^(3+) (aq) → Zn^(2+) (aq) + Ni(s)#?

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Answer 1 · 2018-01-31T00:05:11

Consider,

#Zn(s) + Ni^(3+)(aq) to Zn^(2+)(aq) + Ni(s)#

and its resolution into components,

#Zn(s) to Zn^(2+) + 2e^-#
#Ni^(3+) + 3e^- to Ni(s)#

In order "balance" this reduction-oxidation equation, the electrons oxidized and used by the oxidizing agent must be equal. Hence,

#3Zn(s) to 3Zn^(2+) + 6e^-#
#2Ni^(3+) + 6e^(-) to 2Ni(s)#

is equivalent to,

#3Zn(s) + 2Ni^(3+)(aq) to 3Zn^(2+)(aq) + 2Ni(s)#

Always think of the electrons. Always!