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?

Question

Chemistry

Kylan Hall

10 August, 05:42

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?

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Answers (1)

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Gibson · Answer 1

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