MCQ
How many faraday are needed to reduce a mole of $MnO_4^-$ to $Mn^{2+}$
- A$4$
- ✓$5$
- C$3$
- D$10$
$M n O_{4}^{-}+5 e^{-} \rightarrow M n^{2+}$
The oxidation number of $Mn$ in $MnO _{4}^{-}$ is $+7 .$
The oxidation number of $Mn$ in $M n^{2+}$ is $+2$.
The change in the oxidation number is $7-2=5$.
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(Assume $100\%$ ionization)
$A.$ $0.500\,M\,C _2 H _5 OH ( aq )$ and $0.25\, M\, KBr ( aq )$
$B.$ $0.100\,M\,K _4\left[ Fe ( CN )_6\right]$ (aq) and $0.100\, M$ $FeSO _4\left( NH _4\right)_2 SO _4$ (aq)
$C.$ $0.05 \,M\, K _4\left[ Fe ( CN )_6\right]( aq )$ and $0.25\, M\, NaCl$ (aq)
$D.$ $0.15\, M\, NaCl ( aq )$ and $0.1\, M BaCl _2$ (aq)
$E.$ $0.02\, M\, KCl\, MgCl _{2 .} 6 H _2 O ( aq )$ and $0.05\, M$ $KCl ( aq )$
$C{r_2}O_7^{2 - } + F{e^{2 + }} + {C_2}O_4^{2 - } \to C{r^{3 + }} + F{e^{3 + }} + C{O_2}$ (Unbalanced)