Select the correct statement if: E0Mg2+/Mg=−2.4V,E0Sn4+/Sn2+=0.1V,E0MnO−4,H+/Mn2+=1.5V,E0I2/I−=0.5V
A
MnO−4 is the strongest oxidizing agent and Mg is the strongest reducing agent.
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B
Sn4++2I−→S2++I2 is a spontaneous reaction.
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C
Mg2++Sn2+→Mg+Sn4+ is a spontaneous reaction.
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D
Here, weakest oxidizing agent is Sn4+ and weakest reducing agent is Mn2+.
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Solution
The correct option is BMnO−4 is the strongest oxidizing agent and Mg is the strongest reducing agent. (A) E0MnO−4,H+/Mn2+=1.5 V is most positive. Hence, MnO−4, is the strongest oxidizing agent.
E0Mg2+/Mg=−2.4 V is most negative. Hence, Mg is the strongest reducing agent.
Hence, the statement (A) is correct.
(B) Sn4++2I−→S2++I2 is a non spontaneous reaction. Hence, the statement (B) is incorrect.
(C) Mg2++Sn2+→Mg+Sn4+ is a non spontaneous reaction. Hence, the statement (C) is incorrect.
(D) Here, the weakest oxidizing agent is Mg2+ and the weakest reducing agent is Mn2+.. Hence, the statement (D) is incorrect.