A student investigated the kinetics of the reaction between bromide ions, Br– , and bromate(V) ions, , in aqueous acid.
5Br–(aq) + Br(aq) + 6H+(aq) → 3Br2(aq) + 3H2O(l)
To determine the rate equation for the reaction, the student varied the concentration of bromide ions, bromate(V) ions and acid in turn.
The effect of the concentration of bromide ions was investigated first.
Procedure
Step 1 | Add 10.0 cm3 of 0.0050 mol dm–3 potassium bromate(V), 15.0 cm3 of acidified methyl orange indicator solution and 5.0 cm3 of 0.00010 mol dm–3 aqueous phenol to a beaker labelled P. |
Step 2 | Prepare the contents of beaker Q for Run 1 as specified in the table. |
Step 3 | Pour the contents of beaker Q into beaker P and start a timer. Pour the contents of beaker P back into beaker Q and place beaker Q on a white tile. |
Step 4 | Stop the timer as soon as the mixture turns colourless. Record the time, along with the temperature of the solution. |
Step 5 | Repeat Steps 1 to 4 for the remaining runs. |
Contents of beaker Q | ||
Run | Volume of 0.01 mol dm–3 KBr / cm3 | Volume of H2O / cm3 |
1 | 10.0 | 0 |
2 | 8.0 | 2.0 |
3 | 6.0 | 4.0 |
4 | 5.0 | 5.0 |
5 | 4.0 | 6.0 |
6 | 3.0 | 7.0 |
Give one reason why the contents of beaker P are poured back into beaker Q in Step 3.
Methyl orange indicator is bleached colourless by bromine.
Under the experimental conditions, the reciprocal of the time taken for the methyl orange to be bleached (1/t) is proportional to the initial rate.
(2)
(1)
(1)
The student’s results are shown.
Volume of KBr / cm3 | 10.0 | 8.0 | 6.0 | 5.0 | 4.0 | 3.0 |
Time, t / s | 23 | 24 | 32 | 39 | 48 | 64 |
(1/t) / s–1 | 0.043 | 0.042 | 0.031 | 0.026 | ||
Temperature / °C | 18 | 22 | 22 | 22 | 22 | 22 |
(1)
After investigating the effect on the rate of the concentration of bromate(V) ions and the concentration of hydrogen ions, the student obtained the graphs shown.
Deduce the rate equation for the reaction, using these data and your answer to (c)(iv).
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