lity and 18.3 Gibbs Free Etab1esccaps lockOKINETICS AND EQUILIBRIUMUsing the Arrhenius equation to calculate k at one temperature...The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-27.0 kJ/mol. If the rate constant of thisreaction is 1.4 x 105 Ms at 221.0 °C, what will the rate constant be at 142.0 °C?-1Round your answer to 2 significant digits.k=M¹₁controlExplanation11188.377A2ZaltoptionCheckWS#3XD.²E26TcommandXD$45RC♫OVNItv%5FITVMacBook Pro6(97GWeYB&7HUⒸ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | AccessibilityYou*8N▬▬▬▬▬3/5J(<9MKO3/5OLIP-command:{altLara V282)[11?option?9fildbAI

Answered: Image /qna-images/answer/abd74d12-7eab-44b1-8d4d-33d6e87522d8.jpg

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-27.0 kJ/mol. If the rate constant of this -1 reaction is 1.4×10 M¹s at 221.0 °C, what will the rate constant be at 142.0 °C? Round your answer to 2 significant digits. k= X G

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E-27.0 kJ/mol. If the rate constant of this -1 reaction is 1.4×10 M¹s at 221.0 °C, what will the rate constant be at 142.0 °C? Round your answer to 2 significant digits. k= X G

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...

See similar textbooks

Similar questions

The rate constant k for a certain reaction is measured at two different temperatures: temperature k 215.0 °C 3.7 x 107 134.0 °C 1.4 x 106 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. kJ E = 0 mol ? 0 x10 X
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 314.0 °C 2.1 x 10¹1 384.0 °C 4.3 × 10¹1 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. kJ E = x10 a mol X Ś ?
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=64.0 kJ/mol. If the rate constant of this -1 reaction is 0.0021 M - 1 S. at 40.0 °C, what will the rate constant be at -32.0 °C? Round your answer to 2 significant digits. 1 |M - 1 k = •S Ox10
A certain catalyzed reaction is known to have an activation energy E= 11.0 kJ/mol. Furthermore, the rate of this reaction is measured at 296. K and found to be 1.1 × 10 M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 296. K to 326. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 11.0 kJ/mol to 11.6 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one choose one choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5% V
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 248.0 °C 9.9 x 108 169.0 °C 9.8 x 107 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 mol X S ?
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 59.0 °C 6.5 x 101 14 163.0 °C |4.2 × 10 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E, for this reaction. a Round your answer to 2 significant digits. kJ E x10 mol
A certain catalyzed reaction is Known to have an activation energy Ea=29.0 kJ/mol. Furthermore, the rate of this reaction is measured at 331 K and found to be 2.7× 10* M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is raised by 10% from 331 K to 364 K. How will the rate or the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed which has the eftect of raising the activation energy by 10%, from 29.0 kJ/mol to 31.9 kJ mol How will the rate or the reaction change?
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 278.0 °C 207.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. Ea 2.1×10⁹ 4.5×108 kJ mol x10 X
A reaction having an activation energy of 55.1 kJ/mol has a rate constant of 4.2 x 10-8 s-1 when the temperature is 427. K. What is the rate constant (in s=1) when the temperature is 613. K?
What is the activation energy of a reaction if it has the following rate constants?
The rate constant k for a certain reaction is measured at two different temperatures: temperature 311.0 °C E = a 246.0 °C Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. 0 kJ k 1.4 × 10¹⁰ 2.0 × 10⁹ mol x10 × S
The rate constant k for a certain reaction is measured at two different temperatures: temperature k 407.0 °C 4.8 x 10¹0 268.0 °C 2.3 × 10 ¹0 a Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. kJ E = x10 a mol X 3 ?