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6. Use collision theory to calculate the theoretical value of the rate constant for the elementary...
Use collision theory to calculate the preexponential factor and the rate constant for the reactio...
Use collision theory to calculate the preexponential factor and
the rate constant for the reaction at 298 K. Compare your answer to
the experimental result of A = 2x1011 L mol-1
s-1.
3.13 The reaction F + HH HF is the rate-limiting elementary step in the overall reaction H2 + F2 → 2 HF. This latter process is the key reaction in the HF chemical laser. The reaction proceeds through a transition state: Suppose that the activated complex is linear....
a) Given these data for the reaction , write the rate-law expression. (Use k for the...
a) Given these data for the reaction , write the rate-law expression. (Use k for the rate constant.) Rate = _______ The specific rate constant = ___________ Expt. Initial [A] (M) Initial [B] (M) Initial Rate of Formation of C () 1 0.15 0.40 4x10^-5 2 0.15 0.80 1.6x10^-4 3 0.30 1.6 1.3x10^-3 b) The rate of the elementary reaction C2H2 + H2->C2H4 has been studied as a function of temperature between 300 and 2500 K. The following data were...
The rate of the elementary reaction C2H2 + O2C2H + HO2 has been studied as a...
The rate of the elementary reaction
C2H2 +
O2C2H
+ HO2
has been studied as a function of temperature between
300 and 2500 K. The following
data were obtained for the rate constant k:
Temperature (K)
k (L mol-1 s-1)
300
6.25×10-45
740
1.19×10-12
1180
1.91×10-4
1620
1.07
(a) Calculate the activation energy of this
reaction. kJ mol-1
(b) Calculate the factor A in the Arrhenius equation for the
temperature dependence of the rate constant. L
mol-1 s-1
12) The rate of the elementary reaction CS2 + O2 ---> CS + SO2 has been...
12) The rate of the elementary reaction CS2 + O2 ---> CS + SO2 has been studied as a function of temperature between 1500 and 2100 K. The following data were obtained for the rate constant k: Temperature (K) k (L mol-1 s-1) 1500 2.18×104 1620 4.82×104 1740 9.57×104 1860 1.74×105 (a) Calculate the activation energy of this reaction. ___ kJ mol-1 (b) Calculate the factor A in the Arrhenius equation for the temperature dependence of the rate constant. ___...
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for...
1) Calculate the activation energy in kJ/mol for the following reaction if the rate constant for the reaction increases from 93.5 M-1s-1 at 497.7 K to 1349.3 M-1s-1 at 636.7 K. do not include units, but make sure your answer is in kJ/mol! 2) A chemist constructs a plot of ln k vs. 1/T for a chemical reaction. The slope of the trendline for the data is -746 K. What is the activation energy for this reaction in kJ/mol? R...
Calculate the rate constant at 200.°C for a reaction that has a rate constant of 4.10...
Calculate the rate constant at 200.°C for a reaction that has a rate constant of 4.10 × 10−4 s−1 at 90.°C and an activation energy of 57.3 kJ/mol.
A reaction has a rate constant of 1.12x10-2 /s at 400. K and 0.684 /s at...
A reaction has a rate constant of 1.12x10-2 /s at 400. K and 0.684 /s at 450. K. Part A Determine the activation barrier for the reaction. VO AEO ? E = kJ/mol Submit Request Answer Part B What is the value of the rate constant at 425 K? ΟΙ ΑΣΦ ? k= Submit Request Answer Provide Feedback
23. The rate constant for a particular reaction is 27 activation energy for the reaction in...
23. The rate constant for a particular reaction is 27 activation energy for the reaction in kj/mol (R at 75 lut 25°C and 6 8.314 J/ mol.K) What is the 24. Initial rate data were obtained for the following reaction: A(g) + 2B(g) C + D(e) initial initial TA, mol/l. [B], molt initial rite Experiment 0.45 0.15 0.30 0.15 0.10 0.10 0.20 1.8 0.9 What are the rate law and k value for the reaction? 25. A mixture of 0.100...
The first order elementary reaction: A + B + C was carried out in a constant...
The first order elementary reaction: A + B + C was carried out in a constant volume batch reactor isothermally at 328 K. The concentrations of species A, CA, were recorded as a function of time, as given in the following table. The activation energy Ea=120 kJ/mol. 0.9 6 t (min) CA (mol/dm) 0 20 0.5 17.4 1.5 12.9 2.2 10.5 4 6.2 15.5 8.3 3.5 Based on integral method: b) Process the data using the above table and the...
Calculate the activation energy for the decomposition of hydrogen iodide (HI), if at 573K the rate...
Calculate the activation energy for the decomposition of
hydrogen iodide (HI), if at 573K the rate constant is 2.91E-6 M/s;
and at 773K the rate constant is 7.65E-2 M/s.
Note: answer should be 187.38 kJ/mol
Calculate the activation energy for the decomposition of hydrogen iodide (HI), if at 573 °K the rate constant is 2.91 x 106 M/s; and at 773 "K the rate constant is 7.65 x 102 M/s. a. -1.41 kJ/mol b. 187.38 kJ/mol c. 10.18 kJ/mol d....
Use collision theory to calculate the preexponential factor and
the rate constant for the reaction at 298 K. Compare your answer to
the experimental result of A = 2x1011 L mol-1
s-1.
3.13 The reaction F + HH HF is the rate-limiting elementary step in the overall reaction H2 + F2 → 2 HF. This latter process is the key reaction in the HF chemical laser. The reaction proceeds through a transition state: Suppose that the activated complex is linear....
A reaction has a rate constant of 1.12x10-2 /s at 400. K and 0.684 /s at 450. K. Part A Determine the activation barrier for the reaction. VO AEO ? E = kJ/mol Submit Request Answer Part B What is the value of the rate constant at 425 K? ΟΙ ΑΣΦ ? k= Submit Request Answer Provide Feedback
23. The rate constant for a particular reaction is 27 activation energy for the reaction in kj/mol (R at 75 lut 25°C and 6 8.314 J/ mol.K) What is the 24. Initial rate data were obtained for the following reaction: A(g) + 2B(g) C + D(e) initial initial TA, mol/l. [B], molt initial rite Experiment 0.45 0.15 0.30 0.15 0.10 0.10 0.20 1.8 0.9 What are the rate law and k value for the reaction? 25. A mixture of 0.100...
The first order elementary reaction: A + B + C was carried out in a constant volume batch reactor isothermally at 328 K. The concentrations of species A, CA, were recorded as a function of time, as given in the following table. The activation energy Ea=120 kJ/mol. 0.9 6 t (min) CA (mol/dm) 0 20 0.5 17.4 1.5 12.9 2.2 10.5 4 6.2 15.5 8.3 3.5 Based on integral method: b) Process the data using the above table and the...
Calculate the activation energy for the decomposition of
hydrogen iodide (HI), if at 573K the rate constant is 2.91E-6 M/s;
and at 773K the rate constant is 7.65E-2 M/s.
Note: answer should be 187.38 kJ/mol
Calculate the activation energy for the decomposition of hydrogen iodide (HI), if at 573 °K the rate constant is 2.91 x 106 M/s; and at 773 "K the rate constant is 7.65 x 102 M/s. a. -1.41 kJ/mol b. 187.38 kJ/mol c. 10.18 kJ/mol d....
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