Question

At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k = 2.2 x 10^5 M^-1sec^-1

H2(g) + Ar(g) → 2 H(g) + Ar(g)

a. Calculate the rate of reaction when [H2] = 1.0 x 10^-3 M and [Ar] = 7.2x 10^-4 M.

b. Derive an expression for t½ for a second order reaction (Rate = k[A]^2).

Answer #1

During the initial stages of the following reaction the rate law
is
Rate = k[H2][Br2]½.
H2(g) + Br2(g) → 2 HBr(g)
What is the order of the reaction with respect to each component
and the overall order?

H2O2 decomposes at 20˚C in a first order
reaction where k = 1.06 x 10-3min-1. If the
initial concentration of H2O2 is 0.020 M,
what is [H2O2] after 3.5 days?
a.
9.6x10-5 M
b.
5.1x10-5 M
c.
4.4x10-5 M
d.
1.7x10-5 M
For the following
reaction, calculate the average reaction rate over the
last 2 minutes using the table of data below.
H2(g) +
2ICl(g)
I2(g) + 2HCl(g)
Time
(min) [ICl] (M)
-------------- -----------
0
2.000
2 ...

Determine the rate law and the value of k for the following
reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [
N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4 0.084 4.37 x
10-4 0.224 1.16 x 10-3 Determine the rate law and the value of k
for the following reaction using the data provided. 2 N2O5(g) → 4
NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.093 4.84 x 10-4
0.084 4.37 x 10-4...

at 300 K the reaction below obeys the rate law
rate=k[NOCl]2 where k=
2.8x10-5 M-1* S-1
2NOCl
------> 2NO + Cl2
Suppose
1.0 mole of NOCl is introduced into a 2.0- liter container at 300
k. How much NOCl will remain after 30 minutes?
the
answer is 0.95 mol but how do you get this?

The experimentally determined rate law for the reaction
2NO(g)+2H2(g)→N2(g)+2H2O(g) is
rate=k[NO]2[H2].
Part A
What are the reaction orders in this rate law?
Enter your answers numerically separated by commas.
nNO, nH2 =
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Part B
Would the reaction rate increase more if we double the
concentration of NO or the concentration of H2?
A) The reaction rate will increase more if we double the
concentration of NO.
B) The reaction rate will increase more if we double the...

A packed bed reactor has the reaction A --> B occurring. The
rate law is –rA = kCA where k = 15 L/g-min. The superficial gas
velocity is 4.8 kg/m2-s with a density of 0.45 kg/m3 and a
viscosity of 3.9x10-5 kg/m-s. The porosity, catalyst density, and
particle diameter are, respectively, 0.45, 2.2 g/cm3 and 0.255 cm.
The cross sectional area of the reactor is 12 cm2. The inlet
pressure is 100 kPa. Calculate the conversion ‘X’ when the catalyst...

1) If the rate law for the clock reaction is:
Rate = k [ I-] [ BrO3-]
[H+]
A clock reaction is run with the following initial
concentrations:
[I-]
[BrO3-]
[H+]
[S2O32-]
0.002
0.008
0.02
0.0001
The reaction time is 29 seconds
Calculate k in the rate law:
2)If the rate law for the clock reaction is:
Rate = k [ I-] [ BrO3-]
[H+]
A clock reaction is run...

Determine the rate law (be sure to include the value for k) for
the following reaction using the data provided.
NO2(g)+O3(g)->NO3(g)+O2(g)
[NO2] (M) [O3]i (M) initial rate
0.10 0.33 0.0223
0.10 0.66 0.01788
0.25 0.66 1.112
Please help with reasoning on how to find the order of the
reactions when they are not first or 0 order and how to find k.
Thank you!

The rate law for the reaction: 2H2+2NO--->N2+2H2O is
rate=k[H2][NO]^2. Which of the follwing mechanisms can be ruled out
on the basis of the observed rate expression? PLEASE EXPLAIN
Mechanism 1: H2+NO--->H2O+N (slow) / N+NO----->N2+O (fast)
/ O+H2----> N2+O (fast)
Mechanism 2: H2+2NO---->N2O+H2O (slow) / N2O+H2---->N2+H2O
(fast)
Mechanism 3: 2NO<----->N2O2 (fast equilibrium) /
N2O2+H2------>N2O+H2O (slow) / N2O+H2------>N2+H2O (fast)
PLEASE EXPLAIN WHY.

The
equilibrium constant, Kc, for the following reaction is 55.6 at 698
K.
H2 (g) + I2 (g) forward and reverse arrows 2 HI (g)
Calculate the equilibrium concentrations of reactants and
product when 0.383 moles kf H2 and 0.383 moles of I2 are introduced
into a 1.00 L vessel at 698 K.
[H2] = M
[I2] = M
[HI] = M

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