Question

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?

Answer #1

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 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 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 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!!!*

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.

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 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 decomposition reaction of NOBr is second order in NOBr, with
a rate constant at 20°C of 25 M-1 min-1. If the initial
concentration of NOBr is 0.025 M, find
(a) the time at which the concentration will be 0.010 M.
(b) the concentration after 145 min of reaction.

The decomposition of sulfuryl chloride (SO2Cl2) is a first-order
process. The rate constant for the decomposition at 660 K is
4.5×10−2s−1.
If we begin with an initial SO2Cl2 pressure of 450 torr , what
is the partial pressure of this substance after 68 s?
At what time will the partial pressure of SO2Cl2 decline to
one-third its initial value?

For a first-order reaction, the half-life is constant. It
depends only on the rate constant k and not on the reactant
concentration. It is expressed as t1/2=0.693k For a second-order
reaction, the half-life depends on the rate constant and the
concentration of the reactant and so is expressed as
t1/2=1k[A]0
Part A
A certain first-order reaction (A→products) has a rate constant
of 4.20×10−3 s−1 at 45 ∘C. How many minutes does it take
for the concentration of the reactant, [A],...

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 10 minutes ago

asked 12 minutes ago

asked 24 minutes ago

asked 35 minutes ago

asked 56 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago