0.164
0.164
0.082
0.246
are given below
(M)
0.15
0.45
0.45
0.15
Initial rate (Ms-1)
3.2 x 10-5
2.9 x 10-4
1.4 x 10-4
4.8 x 10-5
Determine the rate law and the rate constant for this reaction. If the rate of disappearance of
is 2.2 x 10-4Ms-1, what would be the rate of formation of CO2?
[Ans: 4.4 x 10-4]](https://image.slidesharecdn.com/initialratemethod-131202005326-phpapp02/85/Initial-rate-method-8-320.jpg)
![Initial rate method Question 5:
Experiment
[MnO4ˉ]/M
[ClO3ˉ]/M
[H+]/M
1
2
3
4
0.10
0.25
0.10
0.10
0.10
0.10
0.30
0.10
0.10
0.10
0.10
0.20
Determine the rate law and rate constant for the reaction.
Initial Rate/
M sˉ1
5.2 x 10-3
3.3 x 10-2
1.6 x 10-2
7.4 x 10-3
[Ans: 16.4]](https://image.slidesharecdn.com/initialratemethod-131202005326-phpapp02/85/Initial-rate-method-9-320.jpg)
![Initial rate method Question 6:
TABLE 1 shows the results obtain from the reaction
aX +
bY
cZ
at a specific temperature.
Experiment
1
2
3
4
Initial
X
Y
concentration (M)
1.0
1.0
2.0
2.0
1.0
3.0
3.0
2.0
Initial rate of formation
of Z
2.20 x 10-4
-1
(M x 10)
1.70min -3
6.60 x 10-4
3.96 x 10-3
Write the rate differential equation for the above reaction. What is the order of reaction with respect to
X and Y? Calculate the rate constant, k for the reaction.
[Ans:Rate constant, k = 2.2 10-4 M-2 min-1]](https://image.slidesharecdn.com/initialratemethod-131202005326-phpapp02/85/Initial-rate-method-10-320.jpg)
Initial rate method
- 1. Learning Outcomes: Determine the order of reaction using: (i) Initial rate method Initial rate method Example 1: O2(g) + Exp 1 2 3 4 5 2NO(g) 2NO2(g) Initial concentrations(molL-1) O2 NO -2 1.10 x 10 1.30 x 10-2 2.20 x 10-2 1.30 x 10-2 1.10 x 10-2 2.60 x 10-2 3.30 x 10-2 1.30 x 10-2 1.10 x 10-2 3.90 x 10-2 (a) Determine the order of reaction with respect to (i) O2 (ii) NO (b) Write the rate law (c) Determine the overall order of the reaction Initial rate (molL-1s-1) 3.21 x 10-3 6.40 x 10-3 12.8 x 10-3 9.60 x 10-3 28.8 x 10-3
- 2. SOLUTI ON: (a) Step 1: Write the rate law Let the rate law Compare experiment 2 with 1
- 3. Compare experiment 3 with 1 3.98
- 4. Initial rate method Question 1: The following of nitric oxide with hydrogen at 12800C is The following data was collected at this temperature : Exp 1 2 3 Initial concentrations(M) NO H2 -3 5.00 x 10 2.00 x 10-3 10.00 x 10-3 2.00 x 10-3 10.00 x 10-3 4.00 x 10-3 Initial rate (Ms-1) 1.25 x 10-5 5.00 x 10-5 10.00 x 10-5 Based on the data above, determine (a) rate law (b) rate constant (c) overall order of reaction (Answer: 2.5 x 102M-2s-1) TIPS: must write the unit
- 5. Initial rate method Question 2: The data below were obtained from the following reaction at 27 oC Exp NaOH 1 2 3 Initial concentrations(M) Reaction rate (M min-1) 0.25 0.50 0.25 3.0 x 10-3 6.0 x 10-3 9.0 x 10-3 0.15 0.15 0.45 (a) What is the order with respect to each reactant? (b) Write the rate equation
- 6. Initial rate method Chalenging Question 1: Exp 1 2 3 4 Initial concentrations(moldm-3) X Y 0.01 0.01 0.01 0.02 0.02 0.01 0.02 0.03 (a) State the order of reaction with respect to (i) X (ii) Y (b) State the overall order of reaction (c) Calculate the rate constant, k and state its unit (d) Determine the value of s Initial rate (mol dm-3min-1) 1.5 x 10-2 3.0 x 10-2 6.0 x 10-2 s
- 7. Initial rate method Question 3: Exp 1 2 3 4 5 6 Initial concentrations(mol dm-3) H2 NO -3 1.0 x 10 6.0 x 10-3 2.0 x 10-3 6.0 x 10-3 3.0 x 10-3 6.0 x 10-3 6.0 x 10-3 1.0 x 10-3 6.0 x 10-3 2.0 x 10-3 6.0 x 10-3 3.0 x 10-3 (a) Determine how the rate of reaction is affected by, (i) Concentration of H2 (ii) Concentration of NO (b) Write the rate equation for the reaction (c) State the overall order of reaction (d) Calculate the value of the rate constant, k Initial rate (mol dm-3s-1) 3.0 x 10-3 6.0 x 10-3 9.0 x 10-3 0.5 x 10-3 2.0 x 10-3 4.5 x 10-3
- 8. Initial rate method Question 4: The data for the initial rates of disappearance of Exp 1 2 3 4 ](M) 0.164 0.164 0.082 0.246 are given below (M) 0.15 0.45 0.45 0.15 Initial rate (Ms-1) 3.2 x 10-5 2.9 x 10-4 1.4 x 10-4 4.8 x 10-5 Determine the rate law and the rate constant for this reaction. If the rate of disappearance of is 2.2 x 10-4Ms-1, what would be the rate of formation of CO2? [Ans: 4.4 x 10-4]
- 9. Initial rate method Question 5: Experiment [MnO4ˉ]/M [ClO3ˉ]/M [H+]/M 1 2 3 4 0.10 0.25 0.10 0.10 0.10 0.10 0.30 0.10 0.10 0.10 0.10 0.20 Determine the rate law and rate constant for the reaction. Initial Rate/ M sˉ1 5.2 x 10-3 3.3 x 10-2 1.6 x 10-2 7.4 x 10-3 [Ans: 16.4]
- 10. Initial rate method Question 6: TABLE 1 shows the results obtain from the reaction aX + bY cZ at a specific temperature. Experiment 1 2 3 4 Initial X Y concentration (M) 1.0 1.0 2.0 2.0 1.0 3.0 3.0 2.0 Initial rate of formation of Z 2.20 x 10-4 -1 (M x 10) 1.70min -3 6.60 x 10-4 3.96 x 10-3 Write the rate differential equation for the above reaction. What is the order of reaction with respect to X and Y? Calculate the rate constant, k for the reaction. [Ans:Rate constant, k = 2.2 10-4 M-2 min-1]
- 11. Initial rate method Chalenging Question 2 : The reaction between C and D is represented as follows: The experiment results are shown in the table below: Exp 1 2 3 Initial concentrations(M) C D 0.10 0.10 0.05 1.00 2.00 1.00 Time interval (min) 30 30 120 The change in concentration of C (M) 2.5 x 10-3 1.0 x 10-2 5.0 x 10-3 (a) Calculate the rate of reaction for each experiment (b) Determine the order of reaction with respect to C and D write the rate law (c) State the effect on the reaction rate if the concentration of D is doubled but the concentration of C remains constant.