In a research paper, (Orkin et al., J. Phys. Chem., 1997, 101: 174) rate constants were determined for the reaction between the hydroxyl radical and chlorobromomethane: OH• + CH2BrCI → products - Data that were obtained included the following values of the rate constant k for the following temperatures: T, K k, cm³/molecule•sec 1.11 x 10 13 298 313 1.34 x 10 13 330 1.58 x 10 13 Determine the Ea and the pre-exponential factor. E, = J/mol A = cm3/molecule sec

In a research paper, (Orkin et al., J. Phys. Chem., 1997, 101: 174) rate constants were determined for the reaction between the hydroxyl radical and chlorobromomethane: OH• + CH2BrCI → products - Data that were obtained included the following values of the rate constant k for the following temperatures: T, K k, cm³/molecule•sec 1.11 x 10 13 298 313 1.34 x 10 13 330 1.58 x 10 13 Determine the Ea and the pre-exponential factor. E, = J/mol A = cm3/molecule sec

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the reaction: NO(g) + C₂H₂(g) → HCN(g) + CO(g) + H(g), is The Arrhenius expression for the reaction is k(T) = 8.97 x 10-¹2 cm³ molec-¹ s¹ exp{-218 kJ mol-¹/RT} over the temperature range 1100 - 1500 K. Using transition state theory, calculate AH* and AS* for this reaction at 1300 K.
The rate law for the oxidation reaction 2CO(g) + O2(g) → 2CO2(g) assuming that the reaction occurs by the Langmuir -Hinshelwood mechanism. The over-all rate law for this mechanism is Rate = k3θCOθO2 ΘO2 = (KO2 [O2])1/2 and ΘCO = KCO [CO] --------------------------------- --------------------------------- 1+ (KO2[O2])1/2 + KCO[CO] 1+ (KO2[O2])1/2 + KCO[CO]
For an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 1
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1) The rate constant for the gas-phase reaction H2(g) + I2(g) → 2 HI(g) has the value 4.45 x 10-5 mol-1 dm³ s-1. What is the equivalent rate constant in units of molecule-1 cm³ s- 1? 2) The kinetics of the hydrolysis of methyl methanoate, CH3COOCH3, in aqueous solution were investigated by measuring the concentration of the ester after different time intervals. The reaction was found to be first order in the concentration of the ester. Use the data below to determine the rate constant for the reaction (must provide best fit graph). 3600 time, t/s 1800 5400 7200 9000 concentration, c/ (mol dm-3) 0.300 0.191 0.135 0.081 0.055 0.035
8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.
10. The rate of change in colour of iodide (yellow) can be measured as it reacts with colourless hypochlorite, OCI (ag): I (aq) + OCI(aq) I0- (aq) + Cl (aq) a. Different concentrations of reactants are combined at the same temperature and the rate of yellow colour disappearance were measured: Rate of colour Trial Initial [I] (mol/L) Initial [OCI(ag)) change (mol/(L s) 0.12 0.18 7.91 x 102 1 0.18 3.95 x 102 0.060 0.090 0.030 9.88 x 103 3 0.24 7.91 x 102 4 0.090 Using the data provided, calculate the value of the rate constant, including units b. Predict the rate of reaction if both reactants have an equal starting concentration of 0.10 mol/1.
Iodine is sparingly soluble in water but much more so in carbon tetrachloride. The equilibrium constant, also called the partition coefficient, for the distribution of I2 between these two phases I2(aq) =12(CCI4) is 83 at 20°C. (a) A student adds 0.028 L of CCI4 to 0.213 L of an aqueous solution containing 0.037 g I2. The mixture is shaken and the two phases are then allowed to separate. Calculate the fraction of I2 remaining in the aqueous phase. 4.0 (b) The student now repeats the extraction of I2 with another 0.028 L of CCI4. Calculate the fraction of I2 from the original solution that remains in the aqueous phase. 4.0 (c) Compare the result in (b) with a single extraction using 0.056 L of CCI4. Comment on the difference. After a single extraction using 0.056 L of CCI4, the fraction of I2 that remains in the aqueous phase is 40 This result is larger than the result in (b), which means that a single large extraction is not as efficient as two separate smaller extractions.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.
2C4H6(g) → C8H12(g) At high temperatures, the compound C4H6 (1,3-butadiene) reacts according to the equation above. The rate of the reaction was studied at 625 K in a rigid reaction vessel. Two different trials, each shown with a different starting concentration, were carried out. The data were plotted in three different ways, as shown below. (a) For trial 1, calculate the initial pressure, in atm, in the vessel at 625 K. Assume that initially all the gas present in the vessel is C4H6. (Hint-this is a gas law problem from chemistry last year) (b) Use the data plotted in the graphs to determine the order of the reaction with respect to C4H6. (c) The initial rate of the reaction in trial 1 is 0.0010 mol/(L *s). Calculate the rate constant, k, for the reaction at 625 K.
Consider the chemical reaction described by 2A(aq) ⇌ D(aq)with rate constants k1 and k-1. If the reaction is subject to a temperature jump, derive the equation for d[D]/dt in terms of a relaxation constant t.
In a study of the rearrangement of cyclopropane to propene at 500 °C (CH₂)3 CH3CH=CH₂ the concentration of (CH₂)3 was followed as a function of time. It was found that a graph of In[(CH₂)3] versus time in seconds gave a straight line with a slope of -9.38×104 s¹ and a y-intercept of -2.02. Based on this plot, the reaction is order in (CH₂)3 and the rate constant for the reaction is