Category 1
Category 2
Category 3
Units 1
Units 2
100
In the reaction: 2NO2 → 2NO + O2 at 3000 °C, the concentration of NO2 decreased from 0.0150 M to 0.0115 M in 100 s. What is the rate of disappearance of NO2 in M/s?
What is the rate of reaction?
rate = - (Delta [A] )/ (Delta t)
100
The rate constant for a reaction is 1.5 x 10-4 M-1s-1 at 100 oC, and 1.2 x 10-3 M-1s-1 at 150 oC. What is the energy of activation?
What is Arrhenius equation?
ln((k2)/(k1)) = -(Ea)/R (1/(T2)-1/(T1))
100
Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0592 M/s. 2NO2(g) → N2O4(g)
What is the relative rate equation?
Rate of reaction= 1/(coeff) * Rate
100
"t" represents:
What is time.
100
"t1/2" represents:
What is half-life.
200
For the reaction 2A + B → C, what is the rate constant, k?
What is generic rate law?
(rate1)/(rate2)
200
The reaction A → B is third order with respect to A. What happens to the rate of reaction when the concentration of A is doubled?
What is rate law?
New Rate = x*Old Rate
200
A first-order reaction has a rate constant of 4.4x10-3 s-1 at 350 K and a rate constant of 9.8x10-2 s-1 at 580K. What is the activation energy?
What is Arrhenius equation?
ln((k2)/(k1)) = -(Ea)/R (1/(T2)-1/(T1))
200
The units for the gas constant, R.
J/(mol*k)
200
The units of the activation energy, Ea.
J/(mol)
300
Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0592 M/s:
2NO2 (g) → N2O4 (g)
What is the relative rate equation AND rate of reaction?
Rate of reaction = 1/(coeff) * Rate
300
For the reaction 2A+3B → C + 2D, what is the order of reaction with respect to A?
What is generic rate law?
(rate1)/(rate2)
300
Consider the zero order reaction: 2NH3 (g) → N2 (g) + 3H2 (g)
What is the rate constant if it takes 60 seconds for a 0.50 M NH3 to decompose to 0.25M?
What is integrated rate law? (Zeroth order)
[A]t = - kt + [A]0
t1/2 = "[A]o"/(2k)
300
The units for rate of a reaction (rate of appearance/disappearance).
M/s
300
The units for rate constant (zeroth order reaction).
M s-1
400
Consider the first order reaction:
Br2 → 2Br
How long does it take for 15% of the reactant to be consumed (initial [Br2] = 0.50 M)?
What is integrated rate law?
ln([A]t) = - kt + ln([A]0)
400
A reaction is in first order of the reactant A. A solution initially has 0.120 M of A is found to have 0.015 M after 54 min. What is the half-life?
What is integrated rate law AND half-life? (First order)
ln([A]t) = - kt + ln([A]0)
t1/2 = ln2/k
400
A → product is a first order reaction. If the initial sample contained 100. g, what is the amount of A left over after 6 half-lives?
What is half-life?
100. g * (½)6 = 1.56 g
(Didn't need to use the first order half life equation because this question isn't asking for time or for the value of k.)
400
The units for rate constant (first order reaction).
s-1
400
The units for rate constant (second order reaction).
M-1s-1
500
A reaction with activation energy of 120 kJ/mol has a rate constant of 0.25 s-1 at 310 K. What will be the temperature for the rate constant to be doubled?
What is Arrhenius equation?
ln((k2)/(k1)) = -(Ea)/R (1/(T2)-1/(T1))
500
Consider the following reaction: 2NOBr (g) → 2NO (g) + Br (g)
The rate constant has the value 0.036 M-1s-1. How long does it take for the reactant to decompose to 25% (initial [NOBr] = 0.90 M)?
What is integrated rate law? (Second order)
1/([A]t) = kt + 1/([A]0)
500
A reaction is known to obey 2nd order kinetics, with k = 0.45 M-1s-1. Calculate the rate of this reaction if the concentration of starting material is 0.15 M.
What is rate law?
500
The units for rate constant (third order reaction).
M-2s-1
500
The units for rate constant (fourth order reaction).
M-3s-1