CHEM 1001 Study Guide - Midterm Guide: Activation Energy, Activated Complex, Collision Frequency

48 views3 pages

oliveduck990

11 Jan 2018

School

Department

Course

Professor

For unlimited access to Study Guides, a Grade+ subscription is required.

Document Summary

14. 1 rate of a chemical reaction: = concentration / time. Initial rate of reaction can be calculating by using 1(slope of tangent line at t=0) or measuring reactant"s concentration as soon as possible after mixing/after short t. 14. 3 effect of concentration on reaction rates: the rate law. Rate law/equation: experimentally determined to predict relationship between rate of reaction. Larger k value = faster reaction: note: can use high school method to determine rate law using table. Just remember to use log if exponents are going to be a fraction, & when solving for k units can be left as m, & remember to check answer at the end using diff. experiment #. 14. 4 zero-order reactions: sum of exponents = 0, so rate of reaction = k = constant. * k = -m = [a]0/tfinal: integrated rate law: expresses concentration of reactant as function of time. y = mx + b. Which is equivalent to [a]t = -kt + [a]0.

Related Questions

What is the instantaneous rate of the reaction at t=800s?

The answer is rate= 6.8x10^-5 m/s but I need an explanation as to how to do the problem

Could you please answer these questions

=======

======

=====

======

====

10-

======

11-

===

12-

=====

13-

The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Show transcribed image text The decomposition of N2O5 can be described by the equation Given these data for the reaction at 45degreeC in carbon tetrachloride solution, calculate the average rate of reaction for each successive time interval. Approximate the instantaneous rate of this reaction at time f = 40 s. The blue curve is the plot of the data. The orange line is tangent to the blue curve at t = 40 s. Consider the reaction described by the following equation. The rate law is What are the missing entries in the following table? What will the initial rate be if [A] is tripled and [B] is halved? Using the given data, determine the rate constant of this reaction. Using the given data, calculate the rate constant of this reaction. The rate constant for this first-order reaction is 0.620 s-1 at 400 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.770 M to 0.280 M? The rate constant for this zero-order reaction is 0.0120 M - s-1 at 300 degree C. How long (in seconds) would it take for the concentration of A to decrease from 0.800 M to 0.200 M? The rate constant for the reaction is 0.830 M 1 s-1 at 200 degree C. If the initial concentration of A is 0.00870 M, what will be the concentration after 795 s? For A products, time and concentration data were collected and plotted as shown here. Determine the reaction order, the rate constant, and the units of the rate constant. After 79.0 min, 40.0% of a compound has decomposed. What is the half-life of this reaction assuming first-order kinetics? A particular reactant decomposes with a half-life of 137 s when its initial concentration is 0.303 M. The same reactant decomposes with a half-life of 219 s when its initial concentration is 0.190 M. Determine the reaction order. What is the value and unit of the rate constant for this reaction? For each of the following cases, identify the order with respect to the reactant, A. The half-life of A decreases as the initial concentration of A decreases A threefold increase in the initial concentration of A leads to a ninefold increase in the initial rate. A threefold increase in the initial concentration of A leads to a 1.73-fold increase in the initial rate The time required for [A] to decrease from [A]0 to [A]o/2 is equal to the time required for [A] to decrease from [A]q/2 to [AJq/4.

Can someone help me with these calculations? I am very confusedwith how to do them. The lab is based off of this: http://course1.winona.edu/jfranz/lab/chem%20213%20lab/Exp2_CV_Kinetic_Study.pdf.Also above and below is my data.