Question

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

Answer #1

the decomposition of hydrogen peroxide
H2O2, is first-order reaction. the half-life
of of reaction is 17.0minutes.
a.) What is the rate constant of the reaction?
b.) If you had a bottle of H2O2, how long
would it take for 80% to decompose?

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?

1.) The decomposition of phosphine (PH3) is a 1st
order reaction.
A.) If the half life of the reaction is 35.0s, what is the rate
constant?
B.) How long will it take for 75% of the phosphine to
decompose?

The decomposition of A to B is a first-order reaction with a
half-life of 85.9 min when the initial concentration of A is 0.483
M: A → 2B How long will it take for this initial concentration of A
to decrease by 23.0%? PLEASE HURRY I DONT HAVE MUCH TIME TO ANSWER
THIS

13.What is the half-life in minutes of a compound if 75.0
percent of a given sample decomposes in 30.0 minutes? Assume
first-order kinetics.
The thermal decomposition of phosphine (PH3) into phosphorus and
molecular hydrogen is a first-order reaction: 4PH3(g) → P(g) +
6H2(g) The half-life of the reaction is 35.0 s at 680°C. Calculate
the first-order rate constant for the reaction: s−1 Calculate the
time required for 88.0 percent of the phosphine to decompose: s

The decomposition of a compound in a first-order solution, with
an activation energy of 52.3 kJ mol-1. A solution with 10% A
decomposes 10% in 10 min at 10 ° C. What percentage of
decomposition can be found with a 20% solution after 20 min at 20 °
C? Answer: 36.21%

Benzene diazonium chloride, C6H5NNCl, decomposes fallowing a
first order rate law.
C6H5NNCl→ C6H5 Cl+N2
If the rate constant at 20°C is 4.3 x 〖10〗^(-5)/s. How long
would it take for 83% of the compound to decompose? If the rate
constant is 9.0 x 〖10〗^(-4) at 55°C what will the activation energy
be?

The rate constant for the first order decomposition of 'A' at
500 degrees celcius is 9.2x10^-3 S^-1. How long will it take for
90.8% of a 0.500 M sample of 'A' to decompose?

A
compound decomposes by a first order reaction. We are told that the
initial concentration is 0.0350M. After 65 seconds, the
concentration of the compound is 0.0250M. What is the concentration
of the compound after 1.47 minutes?

The decomposition of N2O5 is first order reaction. N2O5(g)
decomposes to yield NO2 (g) and O2(g). At 48 deg C the rate
constant for the reaction is 1.2x10^-5 s^-1. Calculate the partial
pressure of NO2(g) produced from 1.0L of 0.700M N2O5 solution at 48
degC over a period of 22 hours if the gas is collected in a 10.0L
container

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