a student balances the following redox reaction using half - reactions.\nal + mn^{2+}→al^{3+}+mn\nhow many…
a student balances the following redox reaction using half - reactions.\nal + mn^{2+}→al^{3+}+mn\nhow many electrons will be lost in all?\n1\n2\n5\n6
Answer
Explanation:
Step1: Write oxidation half - reaction
Al loses electrons to form Al³⁺. The oxidation half - reaction is Al → Al³⁺ + 3e⁻.
Step2: Determine total electrons lost
Since there are 2 Al atoms in the balanced overall reaction (to balance the charges and atoms), the total number of electrons lost is 2×3 = 6. The balanced overall reaction is 2Al + 3Mn²⁺ → 2Al³⁺+ 3Mn.
Answer:
6