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Pari A The following table lists concentrations (A) versus time for a certain reaction in which...
44) Which of the following represents the integrated rate law for a first-order reaction? A) In...
44) Which of the following represents the integrated rate law for a first-order reaction? A) In Alt E-kt TA) B) 1 . 1 .kt Alt Alo C) [Alt-[Al= kt D) k = Ae(Ea/RT) E) IN (1+ Ina 45) Which of the following represents the integrated rate law for a second-order reaction? A) ISAI. -- - B) TÁL TAL. - Lt C) [A]o - [A] =-kt D) k = Ac(Ea/RT) E 1). Ina 46) Which of the following represents the integrated...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of...
The integrated rate law allows
chemists to predict the reactant concentration after a certain
amount of time, or the time it would take for a certain
concentration to be reached. The integrated rate law for a
first-order reaction is: [A]=[A]0e−kt Now say we are particularly
interested in the time it would take for the concentration to
become one-half of its initial value. Then we could substitute
[A]02 for [A] and rearrange the equation to: t1/2=0.693k This
equation calculates the time...
The following data were obtained for the concentration vs. time for a certain chemical reaction. Values...
The following data were obtained for the concentration vs. time for a certain chemical reaction. Values were measured at 1.00 s intervals, beginning at 0.00 and ending at 20.00 s. Concentrations in mM are: 10.00, 6.91, 4.98,4.32, 3.55, 3.21, 2.61, 2.50, 2.22, 1.91, 1.80, 1.65, 1.52, 1.36, 1.42, 1.23, 1.20, 1.13, 1.09, 1.00, and 0.92. A. Decide whether the data best fits zero-order, first-order, or second-order rate kinetics. Make sure to calculate the rate coefficients (with units) for the reaction...
Most of the time, the rate of a reaction depends on the concentration of the reactant....
Most of the time, the rate of a reaction depends on the
concentration of the reactant. In the case of second-order
reactions, the rate is proportional to the square of the
concentration of the reactant.
Select the image to explore the simulation, which will help you
to understand how second-order reactions are identified by the
nature of their plots. You can also observe the rate law for
different reactions.
In the simulation, you can select one of the three different...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg of 238U to decay to 2.5 kg. What mass of 206Pb is produced? (5 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ ΔGIRT Ke=e AGⓇ = -nF8° Units/Constants: Volt: 1 V=1/C Faraday: 1 F -96,485 C/mol e Arrhenius Equation: k = Ae Ea/RT R= 8.314 J/mol K Integrated Rate...
help!! (CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time...
help!!
(CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time (s) 0.600 0 0.424 10.0 0.300 20.0 0.212 30.0 0.150 40.0 Determine the rate law for this reaction and calculate the rate constant. (20 points) E (V) Thermodynamics: AGº - AH-TAS Nernst Equation: 8 = 8°-(RT/nF)InQ AGⓇ--RTINK At 25°C: 8-6° -0.0591/n)logQ AG RT K-e AG° = -nF8° Units/Constants: Volt: 1 V-1 JC Faraday: 1 F -96,485 C/mole Ea/RT Arrhenius Equation: k = Ae R-8.314...
7. Using the following reaction progress diagram, answer the questions below: wiring Energy A G Rxn....
7. Using the following reaction progress diagram, answer the questions below: wiring Energy A G Rxn. a. How many steps are in the reaction? How do you know? (4 points) b. Which letter corresponds to the rate-determining-step? Explain your choice. (6 points) c. Is the reaction exothermic or endothermic? How do you know? (4 points) d. If the energy at point B is lowered, what will happen to the rate of the reaction will it increase, decrease, or stay the...
5. How much faster would a reaction be if a catalyst is used that lowers the...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
helpp 3. For the hypothetical reaction A+B → C the following rate data (with and without...
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
75 To stop a car, first you require a certain reaction time to be 2The psition...
75 To stop a car, first you require a certain reaction time to be 2The psition of a particle moving along the x sxis depends on gin braking: then the car slows at a constant rate. Suppose that the the time according to the equationxbP, where a is in me total distance moved by your car during these two phases is 56.7 m lers and rin secondh What are the units of (a) constant e and (b) con- when its...
44) Which of the following represents the integrated rate law for a first-order reaction? A) In Alt E-kt TA) B) 1 . 1 .kt Alt Alo C) [Alt-[Al= kt D) k = Ae(Ea/RT) E) IN (1+ Ina 45) Which of the following represents the integrated rate law for a second-order reaction? A) ISAI. -- - B) TÁL TAL. - Lt C) [A]o - [A] =-kt D) k = Ac(Ea/RT) E 1). Ina 46) Which of the following represents the integrated...
The integrated rate law allows
chemists to predict the reactant concentration after a certain
amount of time, or the time it would take for a certain
concentration to be reached. The integrated rate law for a
first-order reaction is: [A]=[A]0e−kt Now say we are particularly
interested in the time it would take for the concentration to
become one-half of its initial value. Then we could substitute
[A]02 for [A] and rearrange the equation to: t1/2=0.693k This
equation calculates the time...
Most of the time, the rate of a reaction depends on the
concentration of the reactant. In the case of second-order
reactions, the rate is proportional to the square of the
concentration of the reactant.
Select the image to explore the simulation, which will help you
to understand how second-order reactions are identified by the
nature of their plots. You can also observe the rate law for
different reactions.
In the simulation, you can select one of the three different...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg of 238U to decay to 2.5 kg. What mass of 206Pb is produced? (5 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ ΔGIRT Ke=e AGⓇ = -nF8° Units/Constants: Volt: 1 V=1/C Faraday: 1 F -96,485 C/mol e Arrhenius Equation: k = Ae Ea/RT R= 8.314 J/mol K Integrated Rate...
help!!
(CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time (s) 0.600 0 0.424 10.0 0.300 20.0 0.212 30.0 0.150 40.0 Determine the rate law for this reaction and calculate the rate constant. (20 points) E (V) Thermodynamics: AGº - AH-TAS Nernst Equation: 8 = 8°-(RT/nF)InQ AGⓇ--RTINK At 25°C: 8-6° -0.0591/n)logQ AG RT K-e AG° = -nF8° Units/Constants: Volt: 1 V-1 JC Faraday: 1 F -96,485 C/mole Ea/RT Arrhenius Equation: k = Ae R-8.314...
7. Using the following reaction progress diagram, answer the questions below: wiring Energy A G Rxn. a. How many steps are in the reaction? How do you know? (4 points) b. Which letter corresponds to the rate-determining-step? Explain your choice. (6 points) c. Is the reaction exothermic or endothermic? How do you know? (4 points) d. If the energy at point B is lowered, what will happen to the rate of the reaction will it increase, decrease, or stay the...
5. How much faster would a reaction be if a catalyst is used that lowers the activation energy from 20.0 kJ/mol to 10.0 kJ/mol? Do the calculation at two temperatures: first at 25.0°C and then at 0.0°C. (20 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ AGRT Ke=e AGⓇ =-nF8° Units/Constants: Volt: 1 V = 1 J/C Faraday: 1 F = 96,485 C/mole Arrhenius Equation:...
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
75 To stop a car, first you require a certain reaction time to be 2The psition of a particle moving along the x sxis depends on gin braking: then the car slows at a constant rate. Suppose that the the time according to the equationxbP, where a is in me total distance moved by your car during these two phases is 56.7 m lers and rin secondh What are the units of (a) constant e and (b) con- when its...
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