Chemical Kinetics
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
|
|
||||
---|---|---|---|---|---|
Identify the methods used to monitor a reaction as it occurs in the reaction flask | Polarimeter Scetrometer Pressure measurement
🗑
|
||||
Give the charateristics of the first order reaction having only one reactant | The fate of the reaction is directly proportional to the concentration of the reactant
🗑
|
||||
Give the charateristics of a zero orcer reaction haing only one reactant | The rate of the reaction is not proportional to the concentration of the reactant
🗑
|
||||
Give the charateristics of a second order reaction having only one reactant | The rate of the reaction is proportional to the square of the concentration of the reactant
🗑
|
||||
What are the units for K in Rate= k[X][Y]^2? | 1/M^2s
🗑
|
||||
What are the units for K in Rate= k[X]^2[Y]^2? | 1/M^3s
🗑
|
||||
What are the units for K in Rate= k[X][Y]? | 1/Ms
🗑
|
||||
What are the units for K in Rate= k[X] and k[X]^0[Y]^0? | 1/s
🗑
|
||||
What are the units for K in Rate= k[X][Y]^1/2? | M-1/2s-1
🗑
|
||||
What are the units for K in Rate= k[X]^2? | M-1s-1
🗑
|
||||
Which of the following represents the integrated rate law for a first-order reaction? | ln[A]t/[A]o= -kt
🗑
|
||||
Which of the following represents the integrated rate law for a second-order reaction? | 1/[A]t 1/[A]o= kt
🗑
|
||||
Which of the following represents the integrated rate law for the zeroth-order reaction? | [A]t-[A]o= -kt
🗑
|
||||
What data should be ploteed to show that experimental concentraction data fits a second-order reaction? | ln[reactant] vs. time
🗑
|
||||
What data should be plotted to show that experimental concentration data fits a zeroth-order reaction? | [reactant]vs. time
🗑
|
||||
Which of the following statements is FALSE? | The half life of a first order reaction is dependent on initial concentraion of reactant The half life of a sencond order reaction is not dependent on concentraion
🗑
|
||||
Derive an expression for a '1/3-life' for a first-order reaction? | 1.099/k
🗑
|
||||
Derive an expression for a '1/4-life' for a first-order reaction? | 1.386/k
🗑
|
||||
For a reaction, what generally happens if the temp is increased? | an increase in k occurs, which results in a faster rate
🗑
|
||||
Identify the rate-determining step. | the slowest step
🗑
|
||||
Rate constants | are temp dependent
🗑
|
||||
Identify an homogenous catalyst. | H2SO4 w/ concentrated HCl
🗑
|
||||
Identify an heterogenous catalyst | Pd in H2 gas
🗑
|
||||
In the hydrogenation of double bonds, a catalyst is needed. In the last step, the reactant must escape from the surface into the gas phase. This step is known as | Desorption
🗑
|
||||
Biological catalysts that increase the rates of biochemical reactions are known as | enzymes
🗑
|
||||
What are the units of k in a zero order reaction? | M/s
🗑
|
||||
what are the units of k in a first order reaction? | 1/s
🗑
|
||||
What are the units of k in a second order reaction? | M-1s-1
🗑
|
||||
Given the law Rate= k[X][Y]^2, how does the rate of reaction change if the concentration of Y is doubled? | The rate of reaction will increase by a factor of 4
🗑
|
||||
Give the law Rate= k[X][Y]^2, how does that rate of reaction change if the contration of X is doubled? | The rate of reaction will increase by a factor of 2
🗑
|
||||
Given the law Rate= [X][Y], how does the rate of reaction change if the concentration of Y is doubled? | The rate of reaction will increase by a factor two
🗑
|
||||
Given the law Rate= k[X]^2[Y]^3, how does the rate of reaction change if the concentration of Y is doubled? | The rate of reaction will increase by a factor of 8
🗑
|
||||
Rate= k[A][B]^2, what will happen to the rate of reaction if the concentration of A is increased by a factor of 5.0? the rate will | increase by a factor of 5.00
🗑
|
||||
Rate= k[A][B]^2, what will happen to the rate of reaction if the concentration of B is increased by a factor of 3.00? the rate will | increase by a factor of 9.00
🗑
|
||||
What is the overall reaction order for the reaction that has the rate law: Rate= k[O2][NO]^2? | third order
🗑
|
||||
Given the law Rate= k[X]^2[Y]^3, how does the rate of reaction change if the concentration of X is doubled? | The rate of reaction will increase by a factor of four
🗑
|
||||
Which of the following represents the equation for a first-order half-life? | t 1/2= 0.693/k
🗑
|
||||
Which of the following represents the equation for a second-order half-life? | t 1/2= [A]o/2k
🗑
|
||||
Which of the following represents the equaton for a zero-order half-life? | t 1/2= [A]o/2k
🗑
|
||||
Which of the following reactions would you predict to have the smallest orientation factor? | NOCl2 + NO --> 2 NOCl
🗑
|
||||
Which of the following reactions would you predict to have a largest orientation factor? | H(g) + F(g) --> HF(g)
🗑
|
||||
Which rate law is termolecular? | rate=k[A][B]^2
🗑
|
||||
Which rate law is bimolecular? | rate=k[A][B]
🗑
|
||||
k | A
🗑
|
||||
n, in Rate= k[A]^n | reaction order
🗑
|
||||
t1/2 | half-life
🗑
|
||||
Ea | activation energy
🗑
|
||||
A | frequency factor
🗑
|
||||
Define half-life | a reaction is the time required for the concentration of a reaction to fall to one-half of its initial value
🗑
|
||||
Define activation energy | shows the energy of the molecule as the reaction proceeds
🗑
|
||||
Define frequency factor | represents the number of approaches to the activation barrier per unit
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Created by:
karmabites
Popular Chemistry sets