rate = k [CH3COCH3]m [I2 ]n [H+]p The rate is obtained by the following the disappearance of iodine using starch as an indicator. The following data are obtained: [CH3COCH3] [H+] [I2] Initial Rate (mol/L.s) 0.80 0.20 0.001 4.2 x 10-6 1.6 0.20 0.001 8.2 x 10-6 0.80 0.40 0.001 8.7 x 10-6 0.80
The equation for the iodination of acetone in acidic solution is
CH3 COCH3(aq) + I2(aq) → CH3 COCH2(aq) + H+(aq) + I- (aq)
The rate of the reaction is found to be dependent not only on the concentration of the reactants but also on the hydrogen ion centration. Hence the rate expression of this
rate = k [CH3COCH3]m [I2 ]n [H+]p
The rate is obtained by the following the disappearance of iodine using starch as an indicator. The following data are obtained:
|
[CH3COCH3] |
[H+] |
[I2] |
Initial Rate (mol/L.s) |
|
0.80 |
0.20 |
0.001 |
4.2 x 10-6 |
|
1.6 |
0.20 |
0.001 |
8.2 x 10-6 |
|
0.80 |
0.40 |
0.001 |
8.7 x 10-6 |
|
0.80 |
0.20 |
0.0005 |
4.3 x 10-6 |
1. What is the order of the reaction with respect to each reactant?
2. Write the rate expression for the reaction.
3. Calculate, K
4. What is the rate of the reaction when [H+]= 0.933 M and [CH3COCH3]= 3[H+]= 10[I-] ?
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