Question

Consider the following reaction in aqueous solution. 5 Br−(aq) + BrO3−(aq) + 6 H +(aq) → 3 Br2(aq) + 3 H2O(l) If the rate of disappearance of Br−(aq) at a particular moment during the reaction is 3.4 ✕ 10−4 M·s−1, what is the rate of appearance (in M·s−1) of Br2(aq) at that moment?

Answer 1

Answer:

Rate of appearance of Bromine is 2.04 X 10-4 M·s−1

Explanation:

According to the balanced stoichiometric equation, for every 5 moles of Br- that react, 3 moles of Br2 is produced so they have the stoichiometric ratio of 5:3.

We can use this to calculate the rate of appearance of bromine since this is a direct relationship.

Br-                            :                Br2

5                               :                 3

3.4 ✕ 10−4 M·s−1     :                  x

5x = 1.02 X 10-3 M·s−1

x = 2.04 X 10-4 M·s−1