Question

1)At 25°C, some second-order reaction 3 **X
_{(g)}**

**Example of answer:** **(a)**
**k** = *[*** type
your answer]** M

2)

For some second-order reaction: **3** **X
_{(g)}**

The following data were obtained at 400°C:

[A]_{o} = 9.38 x 10^{-1} M

[A]_{t} = 2.35 x 10^{-3} M

t = 543 s

Calculate the rate constant for this reaction.

**Example of answer:** k =
*[*** type your answer with
correct units]**.

3)

The activation energy for the following reaction: **2
N _{2}O _{(g)}**

By what factor (how many times) will the rate constant increase when the temperature is raised from 728°C to 852°C?

*Hint: Consider which temperature: lower or higher
corresponds bigger rate constant.*

**Example of answer:** =
*[*** type your
answer]**. (k

Answer #1

For the reaction, A(g) + B(g) => 2 C(g), the following data
were obtained at constant temperature.
Experiment
Initial [A], mol/L
Initial [B], mol/L
Initial Rate, M/min
1
0.10
0.10
2 x 10-4
2
0.30
0.30
5.4 x 10-3
3
0.10
0.30
1.8 x 10-3
4
0.20
0.40
6.4 x 10-3
Which of the following is the correct rate law for the
reaction?
1.
Rate = k[A][B]
2.
Rate = k[A]2[B]
3.
Rate = k[A]2[B]2
4.
Rate = k[A]
5....

For the reaction
2 NOBr(g)----> 2 NO(g) + Br2(g)
the rate law is second order in NOBr with a rate constant of
8.50 x 10-2 M-1·s-1 at
35°C. If the initial concentration of NOBr is 1.00
M, how many seconds does it take for [NOBr] to
decrease to 0.10 M?
A) 47 seconds
B) 72 seconds
C) 106 seconds
D) 163 seconds
E) 224 seconds
The answer is C (106 seconds) how do you get
this? Please be detailed and...

For the decomposition reaction CH_33COH (g) → CH_44(g) +
CO(g), the second order rate constant changes from 0.105
M^{-1}−1s^{-1}−1 at 759 K to 0.343 M^{-1}−1s^{-1}−1 at
791 K. What rate constant is expected at 836 K?

1)A second order reaction has a rate constant of 3.7
M-1min-1. if the initial concentration of the reactant is 0.0100M,
what is the concentration remaining after 15 min?
a) .0099M
b) .0056M
c) .0025M
d) .0064M
2) the rate constant for the first order decomposition
of A at 500 degrees Celsius is 9.2 x 10 to the negative 3rd powers
s-1. How long will it take for 90.8 % of a 0.500M sample of A to
decompose
a) 2.5 x...

For the reaction
A + 2 B + C → 3 D + 2 F
the following experimental data were obtained.
Experiment
[A] (M)
[B] (M)
[C] (M)
Rate (M/min)
1
0.10
0.10
0.10
2.0 x 10-5
2
0.10
0.10
0.30
6.0 x 10-5
3
0.20
0.10
0.10
8.0 x 10-5
4
0.10
0.40
0.10
2.0 x 10-5
Part #1:
Which represents the correct rate law?
A) Rate = k
[A]0[B]2[C]
B) Rate = k
[A]2[B]0[C]
C) Rate = k...

15.28
Consider the following reaction:
2 N2O(g) ? 2 N2(g)+O2(g)
A
In the first 13.0 s of the reaction,
1.6×10?2 mol of O2 is produced in a reaction
vessel with a volume of 0.400 L . What is the average
rate of the reaction over this time interval?
Express your answer using two significant figures.
B.
Predict the rate of change in the concentration of N2O over this
time interval. In other words, what is ?[N2O]?t?
Express your answer using two significant figures.

The reaction 2NO(g) + O2(g) 2NO2(g) is second order in NO and
first order in O2. When [NO] = 0.2 M and [O2] = 3.4 M, the observed
rate of disappearance of NO is 0.00001265 M/s.
A) What is the value of the rate constant?
B) What are the units of the rate constant?
- M0 s-1
- M-3 s-1
- s-1
- M3 s
- M-1
- M1 s1
- M-1 s-1
- M-1 s-2
- M-2 s-1
-...

1.
2CH4(g)⇌C2H2(g)+3H2(g)
K = 0.160 at 1658 ∘C . What is Kp for the
reaction at this temperature?
Express your answer numerically.
2.
N2(g)+3H2(g)⇌2NH3(g)
Kp = 4.75×10−3 at 306 ∘C . What is
K for the reaction at this temperature?
Enter your answer numerically.
3.
Given the two reactions
H2S⇌HS− + H+, K1 =
9.12×10−8, and
HS−⇌S2− + H+, K2 =
1.52×10−19,
what is the equilibrium constant Kfinal for the
following reaction?
S2− + 2H+⇌H2S
Enter your answer numerically.
4.
Given the...

The temperature at a point (x, y, z) is given by T(x, y, z) =
100e^(−x^2 − 3y^2 − 9z^2) where T is measured in °C and x, y, z in
meters. (a) Find the rate of change of temperature at the point
P(2, −1, 2) in the direction towards the point (5, −2, 3). (b) In
which direction does the temperature increase fastest at P? (c)
Find the maximum rate of increase at P.

The reaction is 2H202(1) = 2H20(l) + 02(g)
The reaction is second order equation and show all work
How long does it take the solution to decrease by 10% of the
original concentration if k = 4.18 x 10^9 at constant
temperature

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