Mg2+(aq) + 2e->(aq) → Mg(s)E°(volts) = 2.370
Zn2+(aq) + 2e->(aq) → Zn(s)E°(volts) = -0.763
Cds2+(aq) + 2e->(aq) → Cd(s)E°(volts) = 0.403
Cu2+(aq) + 2e->(aq) → Cu(s)E°(volts) = 0.340
In the electrochemical series above, the strongest reducing agents is?
Cu (s)
Cd(s)
Znsub>(s)
Mg(s)
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Discussions (13)
Yes A is the correct answer
HERE'S WHY 👇👇
That is the Standard Electrode potential values
The Mistake is from Myschool cuz those values aren't correct here's the correct value
Given Standard Electrode Potentials ( values):
Mg²⁺ + 2e⁻ → Mg (s) : -2.370V
Zn²⁺ + 2e⁻ → Zn (s) : -0.763V
Cd²⁺ + 2e⁻ → Cd (s) : -0.403 V
Cu²⁺ + 2e⁻ → Cu (s) : +0.340V
The more negative the value, the stronger the reducing agent because it readily donates electrons.
So Mg (s) has the most negative (-2.370 V), meaning it is the strongest reducing agent 👍✅
the answer should be cu ....because its has the lowest oxidation number......and not magnesium
Please @myschool make corrections the answer is supposed to be B
Ref. Page 222 in new school chemistry
In the given electrochemical series, the strongest reducing agent can be determined by looking at the standard reduction potential (E°) values. The more positive the reduction potential value, the stronger the reducing agent.
From the given values:
- Cu(s) has a reduction potential of 0.340 V
- Cd(s) has a reduction potential of 0.403 V
- Zn(s) has a reduction potential of -0.763 V
- Mg(s) has a reduction potential of 2.370 V
Among these options, Mg(s) has the highest reduction potential of 2.370 V. Therefore, Mg(s) is the strongest reducing agent among the given options. So, the correct answer is option D.
the answer is c o unless there is a mistake In magnesium and it has a negative sign
