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CHE 1302 Study Guide - Quiz Guide: Molecularity, Elementary Reaction, Activated Complex

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greyduck910
20 Dec 2017
School
Baylor University
Department
Chemistry
Course
CHE 1302
Professor
Mc Grath

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Document Summary

Reaction rate change in concentration per unit time (can refer to products or reactants) Can be affected by concentration, temperature, surface area (particle size), catalysts/inhibitors. Reaction rates are always > 0 (but remember: change in concentration of a substance being consumed is < 0) For a reaction forming compound a , rate = Units of reaction rate are always concentration/time (usually mol l 1 s 1 or m s 1) also need to consider stoichiometry of the reaction (balanced equation): for the reaction aa bb, reaction rate = . The rate law for a reaction is a relationship between reaction rate and reactant concentrations. For the general reaction aa + bb + products, the rate law is. Normally a m, b n . Units of k depend on the overall reaction order (note: units of rate are still always mol l 1 s 1)

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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

An average reaction rate is calculated as the change in theconcentration of reactants or products over a period of time in thecourse of the reaction. An instantaneous reaction rate is the rateat a particular moment in the reaction and is usually determinedgraphically.

The reaction of compound A forming compound B was studied and thefollowing data were collected:

Time (s) [A](M)
0. 0.184
200. 0.129
500. 0.069
800. 0.031
1200. 0.019
1500. 0.016

a.) What is the average reaction rate between 0. and 1500. s?
b.) What is the average reaction rate between 200. s and 1200.s?
c.) What is the instantaneous rate of the reaction at t=800s?

Please show units of measure

A student studies the kinetics of reaction 1 below using a clock reaction technique, reaction 2, and the procedures given in this experiment. For reaction mixture 1, he measures a time to color change of 121 seconds and for reaction mixture 2, he measures a time of 58 seconds. The temperatures of the reaction mixtures were the same for both experiments.

6I– (aq)+ BrO3– (aq) + 6H+(aq) --> 3I2 (aq) + Br– (aq) + 3H2O(l) (Reaction1,slow)

I2 (aq) + 2 S2O32– (aq) --> 2 I– (aq) + S4O62– (aq) (Reaction 2, fast)

a. Determine the change in concentration of S2O32– that occurred during the time period measured. This should be the same for both the reaction mixtures. First, use M1V1=M2V2 to determine the initial concentration of the S2O32– after mixing the contents of the two flasks but before the reaction begins. Next, find the final concentration of S2O32– by remembering that all the S2O32– is consumed when the color change occurs. You can then find the change in the concentration of S2O32–.

[S2O32–]0 =

∆[S2O32–] =


b. Use the stoichiometry of Reactions 1 and 2 to determine the change in concentration of BrO3– during

the same time period. ∆[BrO3–] =

c. Calculate the initial rate for each reaction mixture. Recall that Rate = − ∆[BrO− ] / ∆t

Rate for mixture 1:

Rate for mixture 2:

d. Method of Initial Rates

Complete the table below using M1V1=M2V2 to find the initial concentration of each reactant after mixing the contents of flasks I and II for both reaction mixtures. Enter the initial rates computed above.

Rxn Mixture [I–]0(M) [BrO3–]0(M) [H+]0 (M) Rate (M/s)

1

2

Use the method of initial rates and the relevant data above to determine the order of reaction 1 with respect to the concentration of iodide ions.

Order with respect to [I–]:_________________________

e. It is critical for the success of this experiment that the concentrations of the reactants I–, BrO3–, and H+ do not change significantly over the time period measured.

Why is this important?

f. By what percent did the bromate ion concentration change during the time period considered for mixture 1 in this experiment?

PercentChange = (|∆[BrO3− ]| / [BrO3− ]0 ) x 100%