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# Balancing a Redox Reaction Under Acidic Conditions

CHEM-MD@SB6

When the following redox reaction is balanced under acidic conditions, how many moles of ${H}_{2}O(l)$ will be produced per mole of $Mn{O}_{2}(s)$?

$$Mn{{O}_{4}}^{-}(aq)+{Br}^{-}(aq)\rightarrow Mn{O}_{2}(s)+Br{{O}_{3}}^{-}(aq)$$

A

$1/2$

B

$1$

C

$2$

D

$4$