Redox Reaction By Oxidation Number Method 01 Ques2
Question:
Which of the following is the correct balanced equation for the reaction between $MnO_4^- (aq)$ and $Fe^{2+} (aq)$ to form $Mn^{2+} (aq)$ and $Fe^{3+} (aq)$ in acidic medium?
Options:
A) $MnO_4^- + 5Fe^{2+} + 8H^+ \rightarrow Mn^{2+} + 5Fe^{3+} + 4H_2O$
B) $MnO_4^- + 4Fe^{2+} + 8H^+ \rightarrow Mn^{2+} + 4Fe^{3+} + 4H_2O$
C) $MnO_4^- + 6Fe^{2+} + 8H^+ \rightarrow Mn^{2+} + 6Fe^{3+} + 4H_2O$
D) $MnO_4^- + 5Fe^{2+} + 8H^+ \rightarrow Mn^{2+} + 5Fe^{3+} + 5H_2O$
Show Answer
Answer: a
Explanation:
A) Correct, this follows the oxidation number method correctly with charge balancing and atom balancing.
B) Incorrect, the ratio between $Fe^{2+}$ and $Fe^{3+}$ is not properly balanced.
C) Incorrect, $Fe^{2+}$ and $Fe^{3+}$ are not in the correct ratio as per oxidation states.
D) Incorrect, the number of water molecules is improperly balanced.
BETA
