Question

What is the difference between zero, first, and second order
chemical reactions in terms of the form of their rate equation and
how can I graph concentration-time data showing which order they
are?

Answer #1

**rate equations are**

**1) zero order :**

**r = k**

**integrate rate law is**

**[A]t = -kt + [A]o**

**comparing it with y = mx + c**

**now**

**draw graph of [A] againsit time**

**if you get a straight line with a negative
slope**

**then the reaction is zero order**

**2) first order :**

**r = k [A]**

**integrated rate law is**

**ln [A] = -kt + ln [A]o**

**now**

**draw a graph of ln [A] vs time (t)**

**if you get a straight line with a negative
slope**

**then**

**the reaction is 1st order**

**3) second order :**

**r = k [A]^2**

**integrated rate law is**

**1/[A] = kt + ( 1/[A]o)**

**now**

**draw a graph of 1 /[A] vs time (t)**

**if you get a straight line with a positive
slope**

**then**

**the reaction is 2nd order**

When looking at a graph how do you know if it is zero order,
first order, second order. Would I be right to assume that if the y
axis, would be In HOF for first order, HOF for zero order, and
1/HOF for second order. Would the equation y = mx+b change. For
example y = -0.17x-0.61 change? What would be an example of the
equation for zero, first and second order?

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
1.) The reactant concentration in a zero-order reaction was
6.00×10−2M after 165 s and
3.50×10−2Mafter 385 s . What is the rate
constant for this reaction?
2.)What was the initial reactant concentration for the reaction
described in Part A?
3.)The reactant concentration in a first-order reaction was
6.70×10−2
M after 40.0 s and 2.50×10−3Mafter
95.0 s ....

How can I convert a second orde ODE into a first-order coupled
equation in terms of the variables of X and P for a simple harmonic
oscillator using the Hamiltonian Equation?

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]=−kt+[A]0
[A] vs. t
−k
1
ln[A]=−kt+ln[A]0
ln[A] vs. t
−k
2
1[A]= kt+1[A]0
1[A] vs. t
k
------------
Part A
The reactant concentration in a zero-order reaction was
5.00×10−2M after 110 s and
4.00×10−2M after 375 s . What is the rate
constant for this reaction?
----------
Part B...

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]=−kt+[A]0
[A] vs. t
−k
1
ln[A]=−kt+ln[A]0
ln[A] vs. t
−k
2
1[A]= kt+1[A]0
1[A] vs. t
k
Part A
The reactant concentration in a zero-order reaction was
8.00×10−2M after 200 s and
2.50×10−2Mafter 390 s . What is the rate
constant for this reaction?
Express your answer with the...

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]=−kt+[A]0
[A] vs. t
−k
1
ln[A]=−kt+ln[A]0
ln[A] vs. t
−k
2
1[A]= kt+1[A]0
1[A] vs. t
k
Part A
The reactant concentration in a zero-order reaction was
7.00×10−2M after 135 s and
2.50×10−2M after 315 s . What is the rate
constant for this reaction?
Express your answer with...

The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]=−kt+[A]0
[A] vs. t
−k
1
ln[A]=−kt+ln[A]0
ln[A] vs. t
−k
2
1[A]= kt+1[A]0
1[A] vs. t
k
Part A
The reactant concentration in a zero-order reaction was
5.00×10−2M after 200 s and
2.50×10−2M after 310 s . What is the rate
constant for this reaction?
Express your answer with...

The first-order decomposition of a colored chemical species, X,
into colorless products is monitored with a spectrophotometer by
measuring changes in absorbance over time. Species X has a molar
absorptivity constant of 5.00x103 cm–1M–1 and the path length of
the cuvette containing the reaction mixture is 1.00 cm. The data
from the experiment are given in the table below.
[X]
(M)
Absorbance (A)
Time (min)
?
0.600
0.0
4.00 x 10-5
0.200
35.0
3.00 x 10-5
0.150
44.2
1.50 x...

The radioisotope studies today decays following either zero
order or first order, or second order kinetics. The graphs produced
by the integrated rate law plot different variables on the x and y
axis depending on the order of the reaction. Look up in your
textbook for the straight line plots of these three types of rate
laws. Draw the plots in your notebook and label it. Give an
equation that can be use to determine the half life of the...

Item 4
The integrated rate laws for zero-, first-, and second-order
reaction may be arranged such that they resemble the equation for a
straight line,y=mx+b.
Order
Integrated Rate Law
Graph
Slope
0
[A]t=−kt+[A]0
[A]t vs. t
−k
1
ln[A]t=−kt+ln[A]0
ln[A]t vs. t
−k
2
1[A]t= kt+1[A]0
1[A]t vs. t
k
Part A
The reactant concentration in a zero-order reaction was
6.00×10−2 mol L−1 after 140 s and 3.50×10−2
mol L−1 after 400 s . What is the rate constant for...

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