Question

the decomposition of hydrogen peroxide
H_{2}O_{2,} is first-order reaction. the half-life
of of reaction is 17.0minutes.

a.) What is the rate constant of the reaction?

b.) If you had a bottle of H_{2}O_{2}, how long
would it take for 80% to decompose?

Answer #1

The rate expression for first oder reaction =

=-dCA/dt= KCA

Where K= rate constant

which on integration and separation of variabled give -ln (1-XA)=Kt

XA =conversion= 1-CA/CAO, CAO= initial concentration and CAO= Concentration at time t and K= rate constant

for XA=0.5 that is the conversion t= t1/2 half life =17 minutes

-ln(1-XA)= -ln (0.5)= Kt1/2

given =0.693 = K t1/2

K= 0.693/ t1/2 = 0.693/17=0.0408 min-1

b) for 80% decomposition XA=0.8 time taken = t

-ln (1-0.8)= 0.0408*t

t= 39.44 minutes

The decomposition of hydrogen peroxide (H2O2) is a first order
reaction with a rate constant 1.8×10-5 s -1 at 20°C.
(a) What is the half life (in hours) for the reaction at
20°C?
(b) What is the molarity of H2O2 after four half lives if the
initial concentration is 0.30 M?
(c) How many hours will it take for the concentration to drop to
25% of its initial value?
*Help please!!!*

1.) The decomposition of phosphine (PH3) is a 1st
order reaction.
A.) If the half life of the reaction is 35.0s, what is the rate
constant?
B.) How long will it take for 75% of the phosphine to
decompose?

QUESTION 6
The first-order
decomposition of hydrogen peroxide occurs according to the
equation
2
H2O2(aq) --> 2 H2O(l) +
O2(g)
Using data from a
concentration-time study of this reaction, which plot will produce
a straight line?
[H2O2] versus time
[H2O2]2 versus time
1 /
[H2O2] versus time
ln[H2O2] versus time

in a first order decomposition reaction, 50.0% of a
compound decomposes in 15.0 min
(a) what is the rate constant of the reaction?
(b) how long does it take for 75.0% of the compound to
decompose

The decomposition of A to B is a first-order reaction with a
half-life of 85.9 min when the initial concentration of A is 0.483
M: A → 2B How long will it take for this initial concentration of A
to decrease by 23.0%? PLEASE HURRY I DONT HAVE MUCH TIME TO ANSWER
THIS

In a study of the gas phase decomposition of hydrogen
peroxide at 400 °C
H2O2(g)H2O(g)
+ ½ O2(g)
the following data were obtained:
[H2O2], M
0.133
6.65×10-2
3.33×10-2
1.67×10-2
seconds
0
16.1
48.2
112
Hint: It is not necessary to graph these
data.
(1)
The observed half life for this reaction when the starting
concentration is 0.133 M is s and
when the starting concentration is
6.65×10-2 M is
s.
(2)
The average (1/[H2O2]) / t
from t = 0...

Hydrogen peroxide decomposes to yield water and oxygen. The
decomposition is first order with a rate constant at 46°C of 1.6 ×
10-4 s-1. Calculate the partial pressure of
the oxygen produced from 1.25 L of a 0.750 M
H2O2 solution at 46°C over a period of 24.0
hours if the gas is collected in a 13.0 L container.
Please show all work! Thanks in advance!

1) The decomposition of hydrogen peroxide in dilute sodium
hydroxide at 20 °C
H2O2(aq)H2O(l)
+ ½ O2(g)
is first order in
H2O2 with a rate constant of
1.10×10-3
min-1.
If the initial concentration of
H2O2 is
9.20×10-2 M, the concentration of
H2O2 will be
1.83×10-2 M after____________
min have passed.
2) The gas phase decomposition of dimethyl ether at 500 °C
CH3OCH3(g)
CH4(g) + H2(g) + CO(g)
is first order in
CH3OCH3 with a rate constant
of 4.00×10-4
s-1.
If...

Data for the decomposition of hydrogen peroxide at some set
temperature T is include below. The rate law depends only on the
concentration of H2O2. Answer questions 6, 7 and 8.
2 H2O2 ---> 2 H2O + O2
t (seconds)
0 ,
60 , 120 ,
180 , 240 , 360 , 420 ,
600
[H2O2] (M) 0.882, 0.697, 0.566 ,0.458, 0.372, 0.236, 0.188,
0.094
What is the value of the rate constant K?
What is the half life of the reaction when the initial
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the partial order with respect to the peroxide (x) be found using
this catalase solution? If so, how would you do it? Describe in
detail the steps you would take or show a calculation.

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