Question

Refer to the given oxidation-reduction reaction, which takes place in acidic solution:
MnO4^-(aq) + Br^-(aq) --> MnO2(s) + BrO3^-(aq)
In the balanced equation, the coefficient for water is:

Answer 1

1

Answer 2

thank you, but can you elaborate on how you came up with this answer?

Answer 3

do you know the general rules to balance a redox reaction? do you need the rules or the specific for this particular reaction? can you figure out what are the oxidation states of the elements in the given reaction and separate the half equations?

Answer 4

I learned this a while ago and kinda forgot how to do it, but I took great notes so i should be fine. Thank you for your help :p

Answer 5

Balancing Redox Reactions
Balancing redox reactions is slightly more complex than balancing standard reactions, but still follows a relatively simple set of rules. One major difference is the necessity to know the half-reactions of the involved reactants; a half-reaction table is very useful for this. Half-reactions are often useful in that two half reactions can be added to get a total net equation. Although the half-reactions must be known to complete a redox reaction, it is often possible to figure them out without having to use a half-reaction table. This is demonstrated in the acidic and basic solution examples. Besides the general rules for neutral conditions, additional rules must be applied for aqueous reactions in acidic or basic conditions.

The method used to balance redox reactions is called the Half Equation Method. In this method, the equation is separated into two half-equations; one for oxidation and one for reduction.

Each equation is balanced by adjusting coefficients and adding H2O, H+, and e- in this order:

Balance elements in the equation other than O and H.
Balance the oxygen atoms by adding the appropriate number of water (H2O) molecules to the opposite side of the equation.
Balance the hydrogen atoms (including those added in step 2 to balance the oxygen atom) by adding H+ ions to the opposite side of the equation.
Add up the charges on each side. Make them equal by adding enough electrons (e-) to the more positive side. (Rule of thumb: e- and H+ are almost always on the same side.)
The e- on each side must be made equal; if they are not equal, they must be multiplied by appropriate integers (the lowest common multiple) to be made the same.
The half-equations are added together, canceling out the electrons to form one balanced equation. Common terms should also be canceled out.
(If the equation is being balanced in a basic solution, through the addition of one more step, the appropriate number of OH- must be added to turn the remaining H+ into water molecules.)
The equation can now be checked to make sure that it is balanced.

http://chemwiki.ucdavis.edu/Analytical_Chemistry/Electrochemistry/Redox_Chemistry/Balancing_Redox_reactions