Multiple ChoiceThe rate constant of a reaction at 32°C is 0.060/s. If the frequency factor is 3.1 × 1015 s–1, what is the activation barrier?7172Has a video solution.
Multiple ChoiceA reaction with an activation energy Ea = 55.00 kJ/mol is run at temperature of 30ºC. Determine the temperature required to increase the rate constant 3 times.7513Has a video solution.
Multiple ChoiceThe following data shows the rate constant of a reaction measured at numerous temperatures. Use the Arrhenius plot to determine the frequency factor for the reaction.24564Has a video solution.
Textbook Question(a) Based on the following energy profile, predict whether kf > kr or kf < kr. [Section 15.1] 189Has a video solution.
Textbook QuestionThe accompanying graph shows plots of ln k versus 1>T for two different reactions. The plots have been extrapolated to the y-intercepts. Which reaction (red or blue) has (b) the larger value for the frequency factor, A? [Section 14.5] 360Has a video solution.
Textbook QuestionThe accompanying graph shows plots of ln k versus 1>T for two different reactions. The plots have been extrapolated to the y-intercepts. Which reaction (red or blue) has (a) the larger value for Ea, 140Has a video solution.
Textbook QuestionCalculate the fraction of atoms in a sample of argon gas at 400 K that has an energy of 10.0 kJ or greater.961Has a video solution.
Textbook Question(a) The activation energy for the isomerization of methyl isonitrile (Figure 14.6) is 160 kJ>mol. Calculate the fraction of methyl isonitrile molecules that has an energy equal to or greater than the activation energy at 500 K. (b) Calculate this fraction for a temperature of 520 K. What is the ratio of the fraction at 520 K to that at 500 K?813Has a video solution.
Textbook QuestionThe activation energy of a reaction is 56.8 kJ>mol and the frequency factor is 1.5 * 1011> s. Calculate the rate constant of the reaction at 25 °C.1298Has a video solution.
Textbook QuestionThe rate constant (k) for a reaction was measured as a function of temperature. A plot of ln k versus 1>T (in K) is linear and has a slope of -7445 K. Calculate the activation energy for the reaction.3869Has a video solution.
Textbook QuestionThe temperature dependence of the rate constant for a reaction is tabulated as follows: Temperature (K) k 1M 1 s1 2 600 0.028 650 0.22 700 1.3 750 6.0 800 23 Calculate Ea and A.12641Has a video solution.
Textbook QuestionThe data shown here were collected for the first-order reaction: N2O( g)¡N2( g) + O( g) Use an Arrhenius plot to determine the activation barrier and frequency factor for the reaction. Temperature (K) Rate Constant (1 , s) 800 3.24 * 10- 5 900 0.00214 1000 0.0614 1100 0.955780Has a video solution.
Textbook QuestionThe tabulated data show the rate constant of a reaction measured at several different temperatures. Use an Arrhenius plot to determine the activation barrier and frequency factor for the reaction. Temperature (K) Rate Constant (1 , s) 300 0.0134 310 0.0407 320 0.114 330 0.303 340 0.7571485Has a video solution.
Textbook QuestionA reaction has a rate constant of 0.0117>s at 400.0 K and 0.689>s at 450.0 K. a. Determine the activation barrier for the reaction.14334Has a video solution.
Textbook QuestionA reaction has a rate constant of 0.000122>s at 27 °C and 0.228>s at 77 °C. b. What is the value of the rate constant at 17 °C?869Has a video solution.
Textbook QuestionConsider these two gas-phase reactions: a. AA( g) + BB( g)¡2 AB( g) b. AB( g) + CD( g)¡AC( g) + BD( g) If the reactions have identical activation barriers and are carried out under the same conditions, which one would you expect to have the faster rate?985Has a video solution.
Textbook QuestionWhich of these two reactions would you expect to have the smaller orientation factor? Explain. a. O( g) + N2( g)¡NO( g) + N(g) b. NO( g) + Cl2( g)¡NOCl( g) + Cl( g)643Has a video solution.
Textbook QuestionThe activation barrier for the hydrolysis of sucrose into glucose and fructose is 108 kJ>mol. If an enzyme increases the rate of the hydrolysis reaction by a factor of 1 million, how much lower must the activation barrier be when sucrose is in the active site of the enzyme? (Assume that the frequency factors for the catalyzed and uncatalyzed reactions are identical and a temperature of 25 °C.)951Has a video solution.
Textbook QuestionThe enzyme urease catalyzes the reaction of urea, 1NH2CONH22, with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 * 10-5 s-1 at 100 C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 * 104 s-1 at 21 C. (c) In actuality, what would you expect for the rate of the catalyzed reaction at 100 C as compared to that at 21 C?1327Has a video solution.
Textbook QuestionThe activation energy of an uncatalyzed reaction is 95 kJ>mol. The addition of a catalyst lowers the activation energy to 55 kJ>mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (b) 125 C?665Has a video solution.
Textbook QuestionThe activation energy of an uncatalyzed reaction is 95 kJ>mol. The addition of a catalyst lowers the activation energy to 55 kJ>mol. Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at (a) 25 C26541Has a video solution.
Textbook QuestionA certain first-order reaction has a rate constant of 1.0 * 10-3 s-1 at 25 °C. (b) What is the Ea (in kJ/mol) if the same temperature change causes the rate to triple?7441Has a video solution.
Textbook QuestionIf the rate of a reaction increases by a factor of 2.5 when the temperature is raised from 20 °C to 30 °C, what is the value of the activation energy in kJ/mol? By what factor does the rate of this reaction increase when the temperature is raised from 120 °C to 130 °C?506Has a video solution.
Textbook QuestionThe kinetics of this reaction were studied as a function of temperature. (The reaction is first order in each reactant and second order overall.) C2H5Br(aq) + OH- (aq)¡C2H5OH(l ) + Br - (aq) Temperature (°C) k (L,mol # s) 25 8.81 * 10- 5 35 0.000285 45 0.000854 55 0.00239 65 0.00633 b. Determine the rate constant at 15 °C.539Has a video solution.
Textbook QuestionThe reaction 2 N2O5¡2 N2O4 + O2 takes place at around room temperature in solvents such as CCl4. The rate constant at 293 K is found to be 2.35 * 10 - 4 s - 1, and at 303 K the rate constant is found to be 9.15 * 10 - 4 s - 1. Calculate the frequency factor for the reaction.666Has a video solution.
Textbook QuestionAt 28 C, raw milk sours in 4.0 h but takes 48 h to sour in a refrigerator at 5 C. Estimate the activation energy in kJ>mol for the reaction that leads to the souring of milk.1179Has a video solution.
Textbook QuestionEthyl chloride vapor decomposes by the first-order reaction: C2H5Cl¡C2H4 + HCl The activation energy is 249 kJ>mol, and the frequency factor is 1.6 * 1014 s - 1. Find the value of the rate constant at 710 K.115Has a video solution.
Textbook QuestionIn a hydrocarbon solution, the gold compound 1CH323AuPH3 decomposes into ethane 1C2H62 and a different gold compound, 1CH32AuPH3. The following mechanism has been proposed for the decomposition of 1CH323AuPH3: Step 1: 1CH323 AuPH3 Δ k1 k -1 1CH323Au + PH3 1fast2 Step 2: 1CH323 Au ¡k2 C2H6 + 1CH32Au 1slow2 Step 3: 1CH32Au + PH3 ¡k3 1CH32AuPH3 1fast2 (f) What would be the effect on the reaction rate of adding PH3 to the solution of 1CH323AuPH3?185Has a video solution.
Textbook QuestionEthyl chloride vapor decomposes by the first-order reaction: C2H5Cl¡C2H4 + HCl The activation energy is 249 kJ>mol, and the frequency factor is 1.6 * 1014 s - 1. What fraction of the ethyl chloride decomposes in 15 minutes at this temperature?10812Has a video solution.
Textbook QuestionThe reaction between ethyl iodide and hydroxide ion in ethanol 1C2H5OH2 solution, C2H5I1alc2 + OH- 1alc2 ¡ C2H5OH1l2 + I - 1alc2, has an activation energy of 86.8 kJ>mol and a frequency factor of 2.10 * 1011 M-1 s-1. (d) Assuming the frequency factor and activation energy do not change as a function of temperature, calculate the rate constant for the reaction at 50 C.309Has a video solution.
Textbook QuestionValues of Ea = 6.3 kJ>mol and A = 6.0 * 108>1M # s2 have been measured for the bimolecular reaction: NO1g2 + F21g2S NOF1g2 + F1g2 (a) Calculate the rate constant at 25 °C.280Has a video solution.
