Can you please write the experimental question below using the results provided on the table Chemical Kinetics 2: Temperature of the reaction: Oxalic acid - potassium permanganate reaction system experiment The reaction rate for the oxidation - reduction between oxalic acid, H2C204 and potassium permanganate, KMnO4, is measured by recording the time elapsed for the purple colour of the permanganate ion, MnO4 to disappear in the reaction: 5H2C2O 4 (aq) + 2KMnO4 (aq) + 3H2SO4 (aq) -> 10CO2 (g) + 2MnSO4 (ag) + K2SO2 (ag) + 8H2O (1) The rate of discharge of the purple colour of MnO4, can thus be used as a measure of the rate of the reaction. Results Experiment Number| Temperature,T ( c) | Time, t (s)| Log t-1 (s-1) (T+273) -1 (K-1) 1|30| 190,21 0,43| 3,30 x 10-3 21 40 58,01 0,571 3, 19 x 10-3 3| 50| 22,91 0,761 3,096 x 10-34|60| 13,0 | 0,891 3,003 x 10-3 5 70| 10,65 0,971 2,91 x 10-3 Questions 2. Plot a graph of log t^ -1 versus (T+ 273)^-1 and draw the best straight line through the points. 3. If the rate of the reaction is k[MnO4] where k is the rate constant, what conclusion can be drawn about the order of the reaction with respect to the oxalate? 4. If the relationship between k and the absolute temperature (T+273)^-1 is log k/s^-1 = -0.0521 Ea (T+273)^-1/kJmol1 + constant, calculate the activation energy, Ea of the reaction from the graph taking k to be equal to t^ -15. Is the inorganic salt a catalyst or not Give reasons for your answer. 6. From your results, state the effect of increasing the temperature on the rate of the reaction and determine the factor by which the rate changes when the temperature changes by 10\deg C. Results and calculations Table \table[[\table[[Experiment], [number]], \table[[Temperature,], [T(c) 田 Results and calculations Table Experiment number 1 -23456 C C Temperature, Time, t(s) Logt (s1) T(C) (T+273) (k-1) 30 40 848828 190,2 0,43 3,30 x 10 58,0 0.57 3,19 x 103 50 22.9 0.76 3,096 x 103 60 13.0 0.89 3,003 x 10-3 70 10,65 0.97 2,91 x 10-3 21,46 0.75 3,096 x 10³
Can you please write the experimental question below using the results provided on the table Chemical Kinetics 2: Temperature of the reaction: Oxalic acid - potassium permanganate reaction system experiment The reaction rate for the oxidation - reduction between oxalic acid, H2C204 and potassium permanganate, KMnO4, is measured by recording the time elapsed for the purple colour of the permanganate ion, MnO4 to disappear in the reaction: 5H2C2O 4 (aq) + 2KMnO4 (aq) + 3H2SO4 (aq) -> 10CO2 (g) + 2MnSO4 (ag) + K2SO2 (ag) + 8H2O (1) The rate of discharge of the purple colour of MnO4, can thus be used as a measure of the rate of the reaction. Results Experiment Number| Temperature,T ( c) | Time, t (s)| Log t-1 (s-1) (T+273) -1 (K-1) 1|30| 190,21 0,43| 3,30 x 10-3 21 40 58,01 0,571 3, 19 x 10-3 3| 50| 22,91 0,761 3,096 x 10-34|60| 13,0 | 0,891 3,003 x 10-3 5 70| 10,65 0,971 2,91 x 10-3 Questions 2. Plot a graph of log t^ -1 versus (T+ 273)^-1 and draw the best straight line through the points. 3. If the rate of the reaction is k[MnO4] where k is the rate constant, what conclusion can be drawn about the order of the reaction with respect to the oxalate? 4. If the relationship between k and the absolute temperature (T+273)^-1 is log k/s^-1 = -0.0521 Ea (T+273)^-1/kJmol1 + constant, calculate the activation energy, Ea of the reaction from the graph taking k to be equal to t^ -15. Is the inorganic salt a catalyst or not Give reasons for your answer. 6. From your results, state the effect of increasing the temperature on the rate of the reaction and determine the factor by which the rate changes when the temperature changes by 10\deg C. Results and calculations Table \table[[\table[[Experiment], [number]], \table[[Temperature,], [T(c) 田 Results and calculations Table Experiment number 1 -23456 C C Temperature, Time, t(s) Logt (s1) T(C) (T+273) (k-1) 30 40 848828 190,2 0,43 3,30 x 10 58,0 0.57 3,19 x 103 50 22.9 0.76 3,096 x 103 60 13.0 0.89 3,003 x 10-3 70 10,65 0.97 2,91 x 10-3 21,46 0.75 3,096 x 10³
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![Can you please write the experimental question below using the results provided on the table Chemical Kinetics 2:
Temperature of the reaction: Oxalic acid potassium permanganate reaction system experiment The reaction rate for
the oxidation - reduction between oxalic acid, H2C204 and potassium permanganate, KMnO4, is measured by
recording the time elapsed for the purple colour of the permanganate ion, MnO4 to disappear in the reaction: 5H2C2O
4 (aq) + 2KMnO4 (aq) + 3H2SO4 (aq) -> 10CO2 (g) + 2MnSO4 (ag) + K2SO2 (ag) + 8H2O (1) The rate of
discharge of the purple colour of MnO4, can thus be used as a measure of the rate of the reaction. Results Experiment
Number| Temperature,T ( c) | Time, t (s)| Log t-1 (s-1)| (T+273) - 1 (K-1) 1| 30| 190,21 0,43| 3,30 x
10-3 21 40 58,01 0, 57| 3,19 x 10-3 3| 50| 22,9 0, 76| 3,096 x 10-3 4|60| 13,0 | 0,891 3,003 x
10-35 70 10,65 0,971 2,91 x 10-3 Questions 2. Plot a graph of log t^ -1 versus (T+ 273)^-1 and draw the best
straight line through the points. 3. If the rate of the reaction is k[MnO4] where k is the rate constant, what conclusion
can be drawn about the order of the reaction with respect to the oxalate? 4. If the relationship between k and the
absolute temperature (T+ 273)^-1 is log k/s^-1 = 0.0521 Ea (T+273) ^ -1/kJmol1 + constant, calculate the
activation energy, Ea of the reaction from the graph taking k to be equal to t^ -15. Is the inorganic salt a catalyst or not.
Give reasons for your answer. 6. From your results, state the effect of increasing the temperature on the rate of the
reaction and determine the factor by which the rate changes when the temperature changes by 10\deg C. Results and
calculations Table \table[[\table[[Experiment], [number]], \table[[Temperature,], [T(c)
Results and calculations
C
C
Table
Experiment
Temperature, Time, t(s)
Logt(s)
number
T(C)
(T+273)1
(k¹)
1
2
13456
40
898828
30
190,2
0.43
3,30 x 103
58.0
0.57
3,19 x 10
50
22,9
0.76
3,096 x 103
60
13.0
0,89
3,003 x 10-³
70
10.65
0,97
2,91 x 10-3
50
21,46
0.75
3,096 x 10³](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77ff2a96-543b-4770-bd8f-7777014afad2%2F52e64001-3895-47cb-8514-3fe5d36692b7%2Fprxblv3_processed.png&w=3840&q=75)
Transcribed Image Text:Can you please write the experimental question below using the results provided on the table Chemical Kinetics 2:
Temperature of the reaction: Oxalic acid potassium permanganate reaction system experiment The reaction rate for
the oxidation - reduction between oxalic acid, H2C204 and potassium permanganate, KMnO4, is measured by
recording the time elapsed for the purple colour of the permanganate ion, MnO4 to disappear in the reaction: 5H2C2O
4 (aq) + 2KMnO4 (aq) + 3H2SO4 (aq) -> 10CO2 (g) + 2MnSO4 (ag) + K2SO2 (ag) + 8H2O (1) The rate of
discharge of the purple colour of MnO4, can thus be used as a measure of the rate of the reaction. Results Experiment
Number| Temperature,T ( c) | Time, t (s)| Log t-1 (s-1)| (T+273) - 1 (K-1) 1| 30| 190,21 0,43| 3,30 x
10-3 21 40 58,01 0, 57| 3,19 x 10-3 3| 50| 22,9 0, 76| 3,096 x 10-3 4|60| 13,0 | 0,891 3,003 x
10-35 70 10,65 0,971 2,91 x 10-3 Questions 2. Plot a graph of log t^ -1 versus (T+ 273)^-1 and draw the best
straight line through the points. 3. If the rate of the reaction is k[MnO4] where k is the rate constant, what conclusion
can be drawn about the order of the reaction with respect to the oxalate? 4. If the relationship between k and the
absolute temperature (T+ 273)^-1 is log k/s^-1 = 0.0521 Ea (T+273) ^ -1/kJmol1 + constant, calculate the
activation energy, Ea of the reaction from the graph taking k to be equal to t^ -15. Is the inorganic salt a catalyst or not.
Give reasons for your answer. 6. From your results, state the effect of increasing the temperature on the rate of the
reaction and determine the factor by which the rate changes when the temperature changes by 10\deg C. Results and
calculations Table \table[[\table[[Experiment], [number]], \table[[Temperature,], [T(c)
Results and calculations
C
C
Table
Experiment
Temperature, Time, t(s)
Logt(s)
number
T(C)
(T+273)1
(k¹)
1
2
13456
40
898828
30
190,2
0.43
3,30 x 103
58.0
0.57
3,19 x 10
50
22,9
0.76
3,096 x 103
60
13.0
0,89
3,003 x 10-³
70
10.65
0,97
2,91 x 10-3
50
21,46
0.75
3,096 x 10³
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