Part AA certain reaction has an activation energy of 62.0 kJ/mol and a frequency factor of Aj = 5.10x1012 Ms1. What isthe rate constant, k, of this reaction at 23.0 C?Express your answer with the appropriate units. Indicate the multiplication of units explicitly either with amultiplication dot (asterisk) or a dash.> View Available Hint(s)ValueUnitsk=SubmitThe linear form of the Arrhenius equationThe Arrhenius equation can be rearranged to a form that resembles the equation for a straight line:( (+) + In AE,In k

The rate constant is found from the Arrhenius equation. k=Ae−Ea/RT where A is the frequency factor…

Part A A certain reaction has an activation energy of 62.0 kJ/mol and a frequency factor of A, - 5.10x1012 M-1s-1. What is the rate constant, k, of this reaction at 23.0 °C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly elther with a multiplication dot (asterisk) or a dash. > View Available Hint(s) HA k- Value Units Submit

Part A A certain reaction has an activation energy of 62.0 kJ/mol and a frequency factor of A, - 5.10x1012 M-1s-1. What is the rate constant, k, of this reaction at 23.0 °C ? Express your answer with the appropriate units. Indicate the multiplication of units explicitly elther with a multiplication dot (asterisk) or a dash. > View Available Hint(s) HA k- Value Units Submit

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

A certai.. cuction is second order in N, and second order in H,. Use this information to complete the table below. Round each of your answers to 3 significant digits. [N] [#.] H initial rate of reaction х10 2.01 M 2.18 M 99.0 M/s 3.07 M 2.18 M M/s ||M/s O Mls 0.483 M 9.07 M
View Policies Current Attempt in Progress For the reaction 2NOCI+ 2NO + Cl, the rate constant k equals 0.020 L mol-1s1 at a certain temperature. Determine how many minutes it would take for the NOCI concentration to drop from 0.081 M to 0.035 M. It would take minutes.
3) For reaction A ->B All of the following statements for the value of A[A]/ At are true except: a) change as long as the reaction continues. b) The sign is always negative. c) The sign is always positive. d) It depends on the reaction rate law
Calculate the rate constant considering the following rate data obtained at 25oC for the following reaction.
Give detailed.Solution Give correct answer please
Using the potential energy diagram determine the activation energy (each division is 10kg).
The initial concentration of a reactant is 0.580 M and the rate constant (k) is 0.0035 M-'s-1. Calculate the final concentration of the reactant after 11 minutes.
The rate constant (k) for a reaction was measured as a function of temperature. A plot of In k versus 1/T (in K) is linear and has a slope of - 6704 K. Calculate the activation energy for the reaction. Express your answer to four significant figures and include the appropriate units. ? J E, 5.570 10 mol Submit Previous Answers Bequest Answer X Incorrect; Try Again; 3 attempts remaining
A particular reaction has an activation energyof E a 189 k//mol . the rate constant for the reaction is 0.00205 457 degrees * C at what temperature (° would the rate constant be 0.200s ^ - 1
Can someone please help with question 11 a and b
please answer all as they are part of 1 question but different questions,,.
General Chemistry II- Ara Sinavi 13 According to the data given below calculate k and t1/2. For the hypothetical aqueous reaction: A B, the concentration change of A was monitored and several derived data were tabulated and two different plots were obtained. Based on these given plots and data: time(min) [A] (M) In[A] V [A] -0.2 0.65 -0.43 1.5 --0.4 10 0.51 -0.67 2.0 -0.6 S -0.8 20 0.42 -0.87 2.4 -1.0 30 0.36 -1.02 2.8 Карat