The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea-69.0 kJ/mol. If the rate constant of thisreaction is 7.3 × 10³ M-1 -1'Sat 314.0 °C, what will the rate constant be at 286.0 °C?Round your answer to 2 significant digits.1 -1k= -MS?0x2X3 The rate constant k for a certain reaction is measured at two different temperatures:temperaturek196.0 °C6.7 x 10874.0 °C4.5 x 107Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction.aRound your answer to 2 significant digits.

Dear student , since you have posted multiple questions we will allow to solve only first question…

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea-69.0 kJ/mol. If the rate constant of this -1 -1 reaction is 7.3 × 10³ M 'S at 314.0 °C, what will the rate constant be at 286.0 °C? Round your answer to 2 significant digits. 1 -1 k= -M S X 3 ?

The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea-69.0 kJ/mol. If the rate constant of this -1 -1 reaction is 7.3 × 10³ M 'S at 314.0 °C, what will the rate constant be at 286.0 °C? Round your answer to 2 significant digits. 1 -1 k= -M S X 3 ?

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 of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 54.0 kJ/mol. If the rate constant of this reaction is 2.0 × 10³ M¹s -1.-1 at 222.0 °C, what will the rate constant be at 272.0 °C? Round your answer to 2 significant digits. k = M .S Ś 囧

A certain reaction has an activation energy of 58.70 kJ/mol. At what Kelvin temperature will the reaction proceed 7.00 times faster than it did at 287 K? T=
The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E,=11.0 kJ/mol. If the rate constant of this a 1 - 1 reaction is 3.2 × 10° M S. at 112.0 °C, what will the rate constant be at 149.0 °C? Round your answer to 2 significant digits. 1 - 1 k = ] M x10 •S ?
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 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?
A certain reaction has k = 8.82 x 10-4 s-1 at 373 K and k = 2.36 × 10-3 s-1 at 401 K. What is the numerical value of the activation energy (in kJ/mol) for this reaction? Give your answer to three sig figs.
The activation energy of a reaction is 33.4 kJ/mol. The rate constant for this reaction is 3.5 x 10-4 at 297.4 K. What is its rate constant at 347.7 K?
Consider this reaction. 2A B It obeys the rate law: rate = k [A] 2 and k = 0.188 M -1 s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? Consider this reaction. 2A B It obeys the rate law: rate = k [A] 2 and k = 0.188 M -1s -1 If the initial concentration of A is 0.600 M, at what time will the concentration be 50.0% of that value? 793 s 8.87 s 182 s 9.48 x 103 s 79.1 s 3.07 x 10-3 s 1.50 x 109 s 5.22 x 10-2 s
Consider a reaction A → B with activation energy 50.7 kJ/mol. At 19.5 °C, the rate constant, k, for this reaction is 0.095 s−1. Calculate the temperature, T (in °C), at which k = 0.329 s−1. Assume the pre-exponential factor (A) is constant with temperature. �=0.08206 L⋅atmmol⋅K=8.314 Jmol⋅K �K=�∘C+273.15 1 kJ = 1000 J Report your answer to three significant figures without the unit. Example: 20.0. Be sure that your answer is in °C and not Kelvin!
The rate constant for the formation of hydrogen iodide from the elements H₂(g) + 1₂(g) → 2Hİ(g) is 2.7 x 10-4 L/(mol-s) at 600 K and 3.5 x 10-3 L/(mol·s) at 650 K. a. Find the activation energy Ea. J/mol b. Then calculate the rate constant at 719 K. L/(mol.s)
The reaction C₂H₂(g) → 2C₂H₂(g) - has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-1. What is the value of the rate constant at 820.0 K? k = 9.42 X10-26 Incorrect S-1
Consider this reaction: →NH4OHaq+NH3aqH2Oaq At a certain temperature it obeys this rate law.rate =·26.0M−1s−1NH4OH2 Suppose a vessel contains NH4OH at a concentration of 1.28M. Calculate the concentration of NH4OH in the vessel 0.270 seconds later. You may assume no other reaction is important.Round your answer to 2 significant digits. =___M