Consider the reaction
5Br(aq) + BrO3(aq) + 6H^+(aq)-> 3Br2(aq) + 3 H2O(l?
The average rate of consumption of Br- is 1.16×10-4 over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
To find the average rate of formation of Br2 during the same time interval, we need to determine the stoichiometric coefficient relationship between Br- and Br2 in the given balanced equation.
From the balanced equation: 5Br(aq) + BrO3(aq) + 6H^+(aq) -> 3Br2(aq) + 3H2O(l), we see that the stoichiometric coefficient of Br2 is 3.
Therefore, for every 3 moles of Br2 formed, a total of 5 moles of Br- must be consumed. This molar ratio allows us to relate the rates of consumption of Br- and formation of Br2.
Given that the average rate of consumption of Br- is 1.16×10-4 over the first two minutes, we can use this information to calculate the average rate of formation of Br2.
To do this, we can use the ratio of stoichiometric coefficients. The rate of formation of Br2 would then be (1.16×10-4 mol Br-/min) multiplied by the stoichiometric coefficient ratio of 3 Br2/5 Br-.
Therefore, the average rate of formation of Br2 during the same time interval is:
(1.16×10-4 mol Br-/min) * (3 Br2 / 5 Br-) = 6.96×10-5 mol Br2/min
So, the average rate of formation of Br2 during the same time interval is 6.96×10-5 mol Br2/min.
To determine the average rate of formation of Br2, we need to use the stoichiometry of the balanced chemical equation. From the given reaction:
5Br(aq) + BrO3(aq) + 6H+(aq) -> 3Br2(aq) + 3H2O(l)
We can see that the ratio of Br2 to Br- is 3:5. Therefore, for every 3 moles of Br2 formed, 5 moles of Br- are consumed.
Given that the average rate of consumption of Br- is 1.16×10-4 mol/min over the first two minutes, we can use this information to find the average rate of formation of Br2.
First, we calculate the moles of Br- consumed over the first two minutes:
Rate of consumption of Br- = 1.16×10-4 mol/min
Time interval = 2 minutes
Moles of Br- consumed = Rate of consumption of Br- × Time interval
= 1.16×10-4 mol/min × 2 min
= 2.32×10-4 mol
Now, using the stoichiometry of the reaction, we can determine the corresponding moles of Br2 formed:
Moles of Br2 formed = (5/3) × Moles of Br- consumed
= (5/3) × 2.32×10-4 mol
= 3.867×10-4 mol
Finally, we calculate the average rate of formation of Br2 over the first two minutes:
Average rate of formation of Br2 = Moles of Br2 formed / Time interval
= 3.867×10-4 mol / 2 min
= 1.9335×10-4 mol/min
Therefore, the average rate of formation of Br2 during the first two minutes is 1.9335×10-4 mol/min.