Iodine And Propanone Reaction Lab Report

TITLE OF EXPERIMENT: An investigation of the iodine/propanone reaction.

DATA COLLECTION AND PROCESSING :

Chemical Equation:

CH3COCH3 (aq) + I2 (aq) ( CH3COCH2I + H+ (aq) + I- (aq)

Rate of reaction:

R = V T

Concentration of reactant after dilution :

Volume of reactant x concentration of reactant
Total volume of mixture

Uncertainty for rate of reaction:

R =( V + t ) x R V t

Eg for Exp 1, run 1: R = ( 1 + 0.1 + 0.1 + 0.1 + 0.01 ) x 0.36 = +0.03cm3s-1 20 8 0 4 11.16

Experiment 1 (without starch solution) :
|
Of I2(aq)/Time) /cm3s-1 |0.11 (+0.01) |0.08 (+0.01) |0.07 (+0.01) |0.14 (+0.03) |

Table 6 shows the rate of reaction for each run with the presence of starch.

Experiment 1 (without starch solution) :

| |Run 1 |Run 2 |Run 3 |Run 4 |
|Concentration of HCl/moldm-3 |1.25 |0.625 |1.25 |1.25 |
|Concentration of propanone/moldm-3 |0.5 |0.5 |0.25 |0.5 |
|Concentration of Iodine/moldm-3 |0.00125 |0.00125 |0.00125 |0.000625 |

Table 7 shows the concentration of reactant for experiment 1.

Experiment 2 (with starch solution)
So, the rate law is given by:

Rate= k[ H+][CH3COCH3]

Rate constant, k = Rate [ H+][CH3COCH3]

| |Rate of reaction / dm3s-1 |[H+] / mol dm-3 |[CH3COCH] / mol dm-3 |k/ dm9 mol-2 s-1 |
|Run 1 |1.1x10-4 |1.08 |0.43 |4.4x10-5 |
|Run 2 |8.0x10-5 |0.54 |0.43 |6.4x10-5 |
|Run 3 |7.0x10-5 |1.08 |0.22 |1.4x10-5 |
|Run 4 |1.4x10-4 |1.08 |0.43 |5.6x10-5 |

Table 6 shows the rate constant for each run in experiment 2.

Average rate constant, k = 4.4x10-5+6.4x10-5+1.4x10-5+ 5.6x10-5 = 4.5x10-5 dm9 mol-2 s-1 4
→The overall order of the reaction is (1+1) = second order.

(ii) QUALITITATIVE