Chemistry Assignment 1: Kinetics, Equilibrium, and Reaction Rates

This document presents solutions to a Chemistry Assignment covering key concepts in chemical kinetics and equilibrium. The assignment includes multiple-choice questions and detailed proofs for each answer, addressing topics such as rate laws, reaction orders, the effect of temperature on reaction rates, and equilibrium constants. It also covers the application of Le Chatelier's principle, and the calculation of equilibrium concentrations. The solutions demonstrate the application of relevant formulas and data analysis to arrive at the correct answers. The assignment also includes a section on the equilibrium constant, and how it relates to the direction of a reaction. The document concludes with a list of cited sources from chemistry textbooks.

Chemistry Assignment 1
CHEMISTRY ASSIGNMENT
Name of student
Institution
Date

Chemistry Assignment 2
Q1
Choice C; 8
Proof
rate = K[A][B]^2
when conc. of A and B is doubled
new rate law
rate = K [2A][2B]^2
rate = 8K[A][B]^2
rate increases by 8 times
Q2
Choice D
Proof

Chemistry Assignment 3

Chemistry Assignment 4
Q3
Choice D
Proof
Formula :
ln[A]0/[A] = kt
k = 1/ t * ln[A]0/[A]
Data :
[A]0 = 0.45 M
[A] = 0.32M
t = 42 min
k = 1 /42 min ( ln ( 0.64 / 0.32 )
= 0.0476min-1
[A]0 = 0.45 M
90% completed means 10% will be left .
10% of 0.45 M = 0.045 M
t = 1 / 0.0476min-1 ln ( 0.32 / 0.16 )
= 42 min

Chemistry Assignment 5
Q4
Choice A
Proof
Q5
Choice B
Proof
we have to use the following equation
ln (k2/k1) = -(Ea/R)(1/T2 - 1/T1)
T1 = 37 ºC + 273 = 310 K T2 = 40 + 273 = 313K
Ea 50 kj / mol or 50000 J/mole , R = 8.314 J/°K*mole
put all these in above equation
ln (k2/k1) = -[(50000 / (8.314) x (1/313) - (1/310)]
ln (k2/k1) = 0.186
K2/K1 = e0.186 = 1.20
so reaction will increase 1.2 time
Q6
Choice D

Chemistry Assignment 6
Proof
Q7
Choice D
Proof
From the given equation:
NO2 + CO -> NO2 + CO2
rate = k[NO2]2[CO]0
rate = k[NO2]2
The equation is based off of the slowest step.
so From step 1:
rate = k[NO2]2
Both matches.
Q8
Choice D
Proof
I- is the catalyst....as it is produced back...and after adding all the steps...it gets canceled on both
sides....Thus it is non consummable...and only aids in reaction to take plac

Chemistry Assignment 7
Q9
Choice B
Proof
B) Kc = [Br2] [F2]5 / [BrF5]2
As,
2BrF5(g) <=====> Br2(g)+5F2(g)
So,
Kc= [Br2][F2]5/[BrF5]2
Q10
Choice E
Proof
second equation is not balanced..it should be 2SO3-->2SO2+O2
then
k1=[SO3]/[SO2][O2]^1/2
K2=[O2][SO2]^2/[SO3]^2
so k1^2=1/K2
none of these
Q11
Choice E
At equilibrium, the rate constant of the forward reaction is equal to the rate constant for
the reverse reaction.
Q12
Choice B ; 3<4<1<2
Proof
Use the Kp values to determine which of the reactions tends to goto completion.
For the Reaction cC + dD<-->aA + bB the equilibrium constantexpression is this:

Chemistry Assignment 8
A large value of Kp means Products > Reactants. A reallylarge value for Kp means Products >>>
Reactants. Likewise a small value of Kp means Products < Reactants. Areally small value for Kp
means Products <<<Reactants.
Q13
Choice B. … 3.2
Proof
2H2S(g) ---> 2H2(g) + S2(g)
Kc = [H2]2[S2]/[H2S]2
[H2] = 4.0 mol / 4.0 L = 1.0 M
[S2]= 0.80 mol / 4.0 L = 0.2 M
[H2S] = 1.0 mol / 4.0 L = 0.25 M
Kc = 1.02 x 0.2 / 0.252 = 3.2
Q14
Choice D
Proof
A + 2 B = C
K1 = [C] / [A][B]^2
C = D + E
K2 = [D][E]/ [C]
A + 2 B = D + E
K c= [D][E] / [A][B]^2
K1K2 = [C] / [A][B]^2 x [D][E] / [C] = Kc
D) Kc = (K1)(K2) is your answer

Chemistry Assignment 9
Q15
No, the reaction is towards the left
Proof
[HOCl] = 0.25 / 3 = 0.08333
[Cl20] = 0.001 / 3 = 3.333 x 10-4
[H20] = 0.56 / 3 = 0.18666
Q = [1]^2 / [0.1] [0.1]
Q = 111.599
as
Q > K , the reaction will towards the left
Q16
No change in equilibrium
Change the volume of the system: When the volume is changed, the concentrations and the
partial pressures of both reactants and products are changed and thus, the both side moles are
same.

Chemistry Assignment 10
Work cited
Atkins, P.W., De Paula, J. and Keeler, J., 2018. Atkins' physical chemistry. Oxford university
press.
Jensen, F., 2017. Introduction to computational chemistry. John wiley & sons.
Joh Brown, W.H. and Poon, T., 2016. Introduction to organic chemistry. John Wiley & Sons. n
Wiley & Sons.
Schwarzenbach, R.P., Gschwend, P.M. and Imboden, D.M., 2016. Environmental organic
chemistry.
Wirth, T. ed., 2016. Hypervalent iodine chemistry (Vol. 373). Cham: Springer International
Publishing.