Question

The decomposition of N2O to N2 and O2 is a first-order reaction. At 730°C, the rate constant of the reaction is 1.94 × 10-4 min-1. If the initial pressure of N2O is 4.70 atm at 730°C, calculate the total gas pressure after one half-life. Assume that the volume remains constant.

Answer #1

The decomposition of N2O to N2 and O2 is a first-order reaction.
At 730°C, the rate constant of the reaction is 1.94 × 10-4 min-1.
If the initial pressure of N2O is 4.70 atm at 730°C, calculate the
total gas pressure after one half-life. Assume that the volume
remains constant.

The decomposition of N2O to N2 and O2 is a first-order reaction.
At 730°C the half-life of the reaction is 3.58 × 103 min. If the
initial pressure of N2O is 4.50 atm at 730°C, calculate the total
gas pressure after one half-life. Assume that the volume remains
constant.

The rate constant for the first-order decomposition of
N2O5 by the reaction
2 N2O5 (g) 4 NO2(g) + O2(g) is k, = 3.38 x 10-5 s
-1 at 25 C. What is the half-life of N2O5?
What will be the partial pressure, initially 500 Torr, at ( a) 50
s; (b) 20 min, (c) 2 hr
after initiation of the reaction?

The rate constant for the first-order decomposition of
a compound A in the
reaction 2 A P is k, =3.56 x 10-7 s-1 at 25°C. What is the
half-life of A? What will be the
pressure, initially 33.0 kPa at (a) 50 s, (b) 20 min, (c) 20 h
after initiation of the reaction?

The first order rate constant of the gas-phase decomposition of
dimethyl ether, (CH3 )2O(g) --> CH4 (g)+
H2(g)+ CO(g) is 3.2 *10-4 s-1 at
450 C . The reaction is carried out in a constant volume container.
Initially, only dimethyl ether is present, and the pressure is
0.350 atm. What is the pressure after 8.0 min? Assume ideal gas
behavior.

The specific rate constant for the first-order decomposition of
N2O5(g) to NO2(g) and O2(g) is
7.48×10−3s−1 at a given temperature.
A. Find the length of time required for the total pressure in a
system containing N2O5 at an initial pressure of 0.100 atm to rise
to 0.200 atm .
B. Find the total pressure after 110 s of reaction.

The first-order decomposition of N2O at a fixed temperature has
a rate constant of 0.385 s-1. If the initial concentration of N2O
is 21.4 M, what is the concentration of N2O after 50 s?

Consider the decomposition of nitrous oxide, laughing gas, 2 N2O
(g) = 2 N2(g) + O2(g)
At 25⁰C, Kc is 7.3 x 1034
(a) Based on the information given, what can you say about the
rate of decomposition of the reaction?
(b) Based on the information given, does nitrous oxide have a
tendency to decompose into nitrogen gas and oxygen?
(c) What is the Kp for the reaction at 25⁰C?

For a particular first-order reaction, it takes 48 minutes for
the concentration of the reactant to decrease to 25% of its initial
value. What is the value for rate constant (in s-1) for
the reaction?
Select one:
A. 4.8 × 10-4 s-1
B. 6.0 × 10-3 s-1
C. 1.0 × 10-4 s-1
D. 2.9 × 10-2 s-1
For the first-order reaction, 2 N2O(g) → 2
N2(g) + O2(g), what is the
concentration of N2O after 3 half-lives if 0.15 mol...

1) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g) 2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of
N2O5 is
0.105 M, the concentration of
N2O5 will
be Mafter 391 s have
passed.
2) The gas phase decomposition of dinitrogen pentoxide at 335
K
N2O5(g)2
NO2(g) + ½ O2(g)
is first order in
N2O5 with a rate constant of
4.70×10-3
s-1.
If the initial concentration of...

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