The reaction A(aq) ---> B(aq) + C(aq) is a first order
reaction. The half-life of A(aq)...
The reaction A(aq) ---> B(aq) + C(aq) is a first order
reaction. The half-life of A(aq) is 86.6 s at 25.0oC and
its half-life is 66.2 s at 45.0oC. What is its half-life
(in s) at 65.0oC?
(a) The reaction A(aq) → B(aq) is a first order reaction with
respect to A(aq). The concentration of A(aq) after 200.0 seconds of
reaction is 0.960 M and the concentration of A(aq) after 1000.0
seconds of reaction is 0.738 M. What was the concentration of A(aq)
after 661.0 seconds of reaction?
(b) The reaction A(aq) → B(aq) + C(aq) is a first order reaction
with respect to A(aq). The half-life of A(aq) is 74.5 s at
25.0oC. Its activation energy...
Suppose the half-life is 55.0 s for a first order reaction and
the reactant concentration is 0.0761 M 40.1 s after the reaction
starts. How many seconds after the start of the reaction does it
take for the reactant concentration to decrease to 0.0183 M?
QUESTION 1
The half-life for a reaction that is
first-order in A is 15 minutes. How long will it take for the
concentration of A to change from 0.16 M to 0.040
M?
A(g) → B(g) + C(g)
60 min
45 min
30 min
23 min
15 min
4 points
QUESTION 2
When a 0.100 mol of a pure compound is dissolved in 1.0 L of
water, the solution pH changes from 7.00 to 4.24. Which of the
following...
The reaction A(aq) → 2 B(aq) is a second order reaction with
respect to A(aq). Its activation energy is 41.3 kJ/mol. When the
concentration of A(aq) is 0.100 M and the temperature is
25.0oC, the rate of reaction is 0.333 M/s. What is the
rate of reaction when we increase the concentration of A(aq) to
0.272 M and we raise the temperature to 54.9 oC?
The reaction A → B + C is known to be first order in A. Below
are data showing the concentration of A as a function of reaction
time.
Time, h
[A], M
0.5
5.00 x 10-2
1
4.51 x 10-2
2
4.06 x 10-2
3
3.30 x 10-2
4
2.18 x 10-2
5
1.77 x 10-2
6
1.44 x 10-2
(a) What is the average rate
of reaction between 0.5 and 2 h? Report the units as well as...
Suppose a chemical reaction is first order and has a half-life
of 2.5 hr at 100 ºC. Which of the following statements
is false regarding this reaction if the temperature is
changed?
Question 5 options:
A)
The half-life at 125 ºC is 1.8 hr.
B)
The half-life at 275 ºC is 3.5 hr.
C)
The half-life at 75 ºC is 4.7 hr.
D)
Not enough information has been provided in order to make a
conclusion.
A first-order reaction has a half-life of 17.3 minutes. What is
the time required for the reactant concentration to decrease to
2.0% of it's origional value?
Thank you!
Exercise 14.80
The half-life for the first-order decomposition of nitramide,
NH2NO2(aq)→N2O(g)+H2O(l), is
123 min at 15∘C.
Part A
If 170 mL of a 0.105 M NH2NO2 solution is allowed to decompose,
how long must the reaction proceed to yield 46.0 mL of
N2O(g) collected over water at 15∘C and a barometric
pressure of 756 mmHg ? (The vapor pressure of water at 15∘C is 12.8
mmHg.)
Express your answer using two significant figures.
t =
min
Please show as much...
A certain first order reaction has a half-life of 0.35 hours.
How long will it take for 12.5 % of the reactant to react?
For a certain first order reaction, it was found that after 35
seconds; only 15 % of the reactants had reacted. What is the
numerical value of the rate constant?
A certain first-order reaction has a half-life of 25 seconds.
What percentage of the reactant will remain after 125 seconds?
A certain first-order reaction has a...
1) A first-order reaction has a half-life of 15.5 s . How long
does it take for the concentration of the reactant in the reaction
to fall to one-eighth of its initial value?
2) The rate constant for a certain reaction is k = 4.30×10−3 s−1
. If the initial reactant concentration was 0.350 M, what will the
concentration be after 8.00 minutes?