The dimerization of butadiene, , to form 1,5-cyclooctadiene is a second-order process that occurs when the diene is heated. In an experiment, a sample of 0.0083 mol of was heated in a 1.0-L flask. After 660. seconds, 15% of the butadiene had dimerized. Calculate the rate constant for this reaction. Rate constant =
we have:
[A]o = 0.0083 M
15% has dimerized. So, remaining is 85 %
[A] = 85 % of 0.0083 M = 0.007055 M
t = 660.0 s
use integrated rate law for 2nd order reaction
1/[A] = 1/[A]o + k*t
1/(0.007055) = 1/(0.0083) + k* 660.0
1.417*10^2 = 1.205*10^2 +k*6.6*10^2
k*6.6*10^2 = 21.26
k = 3.221*10^-2 M-1.s-1
Answer: 3.22*10^-2 M-1.s-1
The dimerization of butadiene, , to form 1,5-cyclooctadiene is a second-order process that occurs when the...
7. The gas-phase conversion of 1,3-butadiene to 1,5-cyclooctadiene, 2C4H6 → C3H12 was studied, providing data for the plot shown, of 1/[butadiene] versus time. 1/[butadiene] (L/mol) 0 500 1000 time (s) 1500 2000 a. Explain how this plot confirms that the reaction is second order. b. Calculate the second-order rate constant, k. c. Determine the initial concentration of 1,3-butadiene in this experiment.
The decomposition of 1,3-butadiene represents a second order process. 2 1,3-butadiene - (2,2)-15-Cyclooctadiene Answer the following questions about the decomposition of 1,3-butadiene. Report all answers to three significant figures. 1. The initial concentration of 1,3-butadiene is 1.945x10-2 M, however after 1.63 h the concentration decreases to 7.780x10- M. Calculate the rate constant (in /M hr) for this process. Submit Answer Tries 0/5 2. If the initial concentration of 1,3-butadiene is 1.945x10M, calculate the concentration (in M) of 1,3- butadiene after...
Butadiene (C4H6)reacts with itself to form a dimer with the formula C8H12. The reaction is second order in C4H6. Assume the rate constant at a particular temperature is 4.0×10−2M−1s−1 and the initial concentration of C4H6 is 0.0230 MM. What is its molarity after a reaction time of 1.30 hh? What is the time (in hours) when the C4H6 concentration reaches a value of 0.0023 M?
9) Butadiene can undergo the following reaction to form a dimer (two butadiene molecules hooked together). 2C4H3(g) → C8H12(g) The half-life for the reaction at a given temperature is 5.92 x 10-2 sec. The reaction kinetics are second order. a) If the initial concentration of C&His 0.5 M, what is the rate constant for the reaction? b) If the initial concentration of C4H8 is 0.1 M. what will be the concentration of the C4H8 after 3.6 x 102 sec?
3. Butadiene (C4H) reacts with itself at 250 °C to form a dimer with the formula CxH12. 2 C.H. (g) →C3H12 (1) The reaction is second order in C4H. mC4H16. a) What is the rate law for the reaction? b) If initial concentration of C.H. is 0.400 M, what is the concentration of C&H, after 25 min if the rate constant is 4.0 x 10-2 M's?
Butadiene (C4H6) reacts with itself to form a dimer with the formula C8H12. The reaction is second order in C4H6. Assume the rate constant at a particular temperature is 4.0×10−2M−1s−1 and the initial concentration of C4H6 is 0.0250 M. A)What is its molarity after a reaction time of 1.10 h? B)What is the time (in hours) when the C4H6 concentration reaches a value of 0.0025 M?
The initial concentration of N O 2 in the second-order reaction 2N O 2 →2NO+ O 2 is 0.621 mol/L . After 20 seconds, the concentration of N O 2 is 0.583 mol/L . W hat is the rate constant for the reaction?
Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second-order reaction: N2O4(g) → 2NO2(g) At 400.0 K, the rate constant for this reaction has been measured to be 2.9 × 108 L/(mol • s). Suppose 0.222 mol of N2O4(g) is placed in a sealed 41.7-L container at 400.0 K and allowed to react. What is the total pressure inside the vessel after 32.9 ns has elapsed? (R = 0.0821 (L • atm)/(K • mol)) a. 0.183 atm b. 0.175 atm...
1a. At 573 K, gaseous NO2 decomposes, forming NO(g) and O2. If a vessel containing NO2(g) has an initial concentration of 0.056 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant, and the rate constant for this reaction, at 573 K, is 1.1 L/mol · s. = ___ s 1b. The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction....
A gas decomposes to form O2 and two other products, in a first-order reaction, with rate constant k = 6.95 x 10 –4/s at 40oC. If the initial gas concentration = 4.80 x 10 –2 mol/L, what is the concentration (M) after 250 seconds have passed?