1-Bromobutane was hydrolysed by an aqueous sodium hydroxide (NaOH) solution. CH3CH2CH2CH2Br + NaOH → CH3CH2CH2CH2OH + NaCl 1-Bromobutane Butan-1-ol During the reaction, the reactant sodium hydroxide is used up. Samples of the reaction mixture were drawn off at regular time intervals and analysed by titration with standard sulfuric acid to find out the concentration of sodium hydroxide. The results are given in the table below: Time / s Concentration of OH- / mol dm-3 0 0.500 100 0.350 200 0.250 300 0.180 400 0.125 500 0.090 600 0.063 700 0.040 800 0.030 Plot a ‘concentration of OH- (mol dm-3) against time (s)’ graph using the results given in the table above. Label the vertical and horizontal axes of the graph and include the unit/s. Select 4 suitable points along your graph [see part (a)] and draw tangents to find the rates. Construct a table of “Rate” against “Concentration” The rates need to be calculated and the calculations shown. From your graph drawn in part (c) make a deduction (deduce) the ‘order of reaction’ with respect to the concentration of OH-, hydroxide ions. Write a rate equation with respect to the concentration of hydroxide ions. Calculate the rate constant k from the gradient of the graph, drawn for part (c). All calculations must be shown.
URGENT HELP PLEASE
(this is not an exam question)
1-Bromobutane was hydrolysed by an aqueous sodium hydroxide (NaOH) solution.
CH3CH2CH2CH2Br + NaOH → CH3CH2CH2CH2OH + NaCl
1-Bromobutane Butan-1-ol
During the reaction, the reactant sodium hydroxide is used up. Samples of the reaction mixture were drawn off at regular time intervals and analysed by titration with standard sulfuric acid to find out the concentration of sodium hydroxide.
The results are given in the table below:
|
Time / s |
Concentration of OH- / mol dm-3 |
|
0 |
0.500 |
|
100 |
0.350 |
|
200 |
0.250 |
|
300 |
0.180 |
|
400 |
0.125 |
|
500 |
0.090 |
|
600 |
0.063 |
|
700 |
0.040 |
|
800 |
0.030 |
Plot a ‘concentration of OH- (mol dm-3) against time (s)’ graph using the results given in the table above. Label the vertical and horizontal axes of the graph and include the unit/s.
Select 4 suitable points along your graph [see part (a)] and draw tangents to find the rates. Construct a table of “Rate” against “Concentration” The rates need to be calculated and the calculations shown.
From your graph drawn in part (c) make a deduction (deduce) the ‘order of reaction’ with respect to the concentration of OH-, hydroxide ions.
Write a rate equation with respect to the concentration of hydroxide ions.
Calculate the rate constant k from the gradient of the graph, drawn for part (c). All calculations must be shown.
Trending now
This is a popular solution!
Step by step
Solved in 9 steps with 8 images
