Module 1 & 2
Module 3 & 4
Module 5 & 6
Module 7 & 8
Module 9 & 10
Module 11 & 12
Module 13 & 14
Trivia:)
100
One resonance structure for thiocyanate ion is drawn below. What is the formal charge on each atom?
a. S = 0, C = +2, N = -3
b. S = 0, C = -1, N = 0
c. S = 0, C = 0, N = -1
d. S = -2, C = +4, N = -3
e. S = -1, C = 0, N = 0
c. S = 0, C = 0, N = -1
100
What do the point and arrows demonstrate respectively?
100
% by mass equation
(mass solute (g)/ total mass of solution (g)) *100
100
Label the energy diagram below as exothermic or endothermic
Exothermic
100
According to the Brønsted-Lowry definition, a base
a. increases the H3O+ concentration in an aqueous solution.
b. increases the OH- concentration in an aqueous solution.
c. is a proton acceptor.
d. is a proton donor.
e. is an electron-pair donor.
c. is a proton acceptor.
100
A saturated solution means the reaction is at equilibrium
A) True
B)False
A) True
100
Which of these species has the highest entropy (S°) at 25°C?
A) CH3OH(l) B) CO(g) C) MgCO3(s) D) H2O(l) E) Ni(s)
B) CO(g)
100
Who would win: 100 men Vs. 1 gorilla
Chat says 100 men
200
Which of the following hydrocarbons has two π bonds?
a.C4H6
b.C7H14
c.C3H6
d.C6H12
e.C8H18
a. C4H6
200
What intermolecular force or bond is primarily responsible for the solubility of chlorine (Cl2) in water?
a. dipole/dipole force
b. hydrogen bonding
c. dipole/induced dipole force
d. ion-dipole force
e. ion-induced dipole force
c. dipole/induced dipole force
200
Molality Equation
moles solute/ kg of solvent
200
A 0th order reactant cannot influence a reaction based on its concentration
A) True
B) False
A) True
200
What are the strong acids?
HI, HCl, HBr, HNO3, HClO3, HClO4, H2SO4
200
Sodium Nitrate is insoluble in water
A) True
B)False
B) False
200
Determine the oxidation number of Sulfur in H2SO4
S=+6
200
Which U.S. document begins with “We the People”?
The Constitution
300
What is the hybridization of the sulfur atom in SO2?
a) sp3d2
b)sp
c) sp2
d) sp3d
c) sp2
300
Which of the following hydrocarbons can have cis and trans isomers?
a. propene
b. 1-butene
c. 2-ethylbutane
d. 2-pentyne
e. 3-hexene
e. 3-hexene
300
Which of the following changes are likely to increase the rate of a chemical reaction?
1. Adding a catalyst
2. Increasing the temperature of the reactants
3. Increasing the concentrations of the reactants
a. 1 only
b. 2 only
c. 3 only
d. 1 and 3
e. 1, 2, and 3
e. 1, 2, and 3
300
A gaseous mixture of NO2 and N2O4 is in equilibrium. If the concentration of N2O4 is 7.1 × 10-4 M, what is the concentration of NO2?
2 NO2(g) ⇋ N2O4(g) Kc = 170
a. 1.7 × 10-11 M b. 4.2 × 10-6 M
c. 2.0 × 10-3 M d. 4.9 × 102 M
e. 2.4 × 105 M
c. 2.0 × 10-3 M
300
Identify the acid and conjugate base of the following reaction
HCO3-+ HPO42- -> H2CO3 + PO43-
Acid: HPO42-
Conj. Base: PO43-
300
A titration of an acid and base to the equivalence point results in a noticeably acidic solution. It is likely this titration involves
A) a strong acid and a weak base.
B) a weak acid and a strong base.
C) a weak acid and a weak base (where Ka equals Kb).
D) a strong acid and a strong base.
A) a strong acid and a weak base.
300
A certain electrochemical cell has for its cell reaction:
Zn + HgO → ZnO + Hg
Which is the half-reaction occurring at the anode?
A) HgO + 2e- → Hg + O2– C) Zn → Zn2+ + 2e-
B) Zn2+ + 2e- → Zn D) ZnO + 2e- → Zn
C) Zn → Zn2+ + 2e-
300
In Breaking Bad, what is Walter White’s street name?
Heisenberg
400
Which of the following is a correct Lewis structure for N2O?
(2)
400
An unsaturated hydrocarbon is
a. a compound in which all carbon atoms have four single bonds.
b. a cycloalkane with five or more carbons.
c. a hydrocarbon that is a gas at room temperature.
d. a compound in which one or more carbon atoms have double or triple bonds.
e. a hydrocarbon that contains oxygen.
d. a compound in which one or more carbon atoms have double or triple bonds.
400
How are the exponents in a rate law determined?
1. They are equal to the concentrations of the reactants.
2. They are equal to the coefficients in the balanced chemical equation.
3. They are determined by experimentation.
a. 1 only
b. 2 only
c. 3 only
d. 1 and 2
e. 2 and 3
c. 3 only
400
What is the overall order of the reaction below
2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
if it proceeds via the following rate law?
rate= k[NO]2[H2]
a. zero-order
b. first-order
c. second-order
d. third-order
e. fourth-order
d. third-order
400
Which one of these salts will form a basic solution on dissolving in water?
A) KCl B) KI C) NaNO2 D) NH4NO3 E) KBr
C) NaNO2
400
Find the normality of 15M of H2SO3
30 N
N= nM
400
Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion.
4Al(s) + 3O2(g) → 2Al2O3(s)
Using the thermodynamic data provided below, calculate ΔS° for this reaction.
A) 182.3 J/K·mol D) –626.2 J/K·mol
B) 131.5 J/K·mol E) –802.9 J/K·mol
C) –182.3 J/K·mol
D) –626.2 J/K·mol
400
How many colors are there in a rainbow?
7
500
How many sigma (σ) bonds and pi (π) bonds are in acetic acid?
7 sigma and 1 pi bond
500
What is the balanced chemical equation for the combustion of 2-methyl-1-butene?
a. 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l)
b. 2 C5H10(g) + 15O2(g) → 10CO2(g) + 10H2O(l)
c. C4H8(g) + 6O2(g) → 4CO2(g) + 4H2O(l)
d. C4H10(g) + 13O2(g) → 5CO2(g) + 6H2O(l)
e. C5H12(g) + 9O2(g) → 6CO2(g) + 6H2O(l)
a. 2C4H10(g)+ 13O2(g) → 8CO2(g) + 10H2O(l)
500
The Henry's law constant for N2 in water at 37 °C is
8.2 × 10-7 M/mm Hg. What is the equilibrium concentration of N2 in water when the partial pressure of N2 is 634 mm Hg?
a. 1.3 × 10-9 M
b. 5.2 × 10-4 M
c. 1.9 × 10-2 M
d. 1.9 × 103 M
e. 7.7 × 108 M
b. 5.2 *10-4
Henry's Law (C=kP)
500
The half-life of a first-order decomposition reaction is 2.36 hours. If the initial concentration of reactant is 0.52 M, what is the concentration of reactant after 752 seconds?
a. 0.046 M
b. 0.16 M
c. 0.26 M
d. 0.47 M
e. 0.49 M
e) 0.49 M
*use first order concentration & half-life equations*
500
What is the H+ ion concentration in a 4.8*10-2 M KOH solution?
A) 4.8* 10-2 M B) 4.8*10-12 M C) 1.0* 10-7 M
D) 2.1* 10-13 M E) 4.8*10-11 M
D) 2.1*10-13
500
At 1500°C the equilibrium constant for the reaction CO(g) + 2H2(g) ⇋ CH3OH(g) has the value
Kp = 1.4 × 10-7. Calculate ΔG° for this reaction at 1500°C. (R=8.314 J/mol*K)
A) 105 kJ/mol D) –105 kJ/mol
B) 1.07 kJ/mol E) 233 kJ/mol
C) –233 kJ/mol
E) 233 kJ/mol
ΔG°=−RTlnK
500
Determine the overall cell potential of the following redox reaction
PbCl2(s) + 2 Li(s) → Pb(s) + 2 Li+(aq) + 2 Cl-(aq)
E°cell= 2.92 V
500
What does URL stand for
Uniform Resource Locator
600
Calculate the number of chlorine atoms in 441g calcium chloride.
4.79*1024 chlorine atoms in 441g of CaCl2
600
At its boiling point of -42.1 °C, 14.6 kJ of heat (q) is required to vaporize 33.9 g of propane (C3H8). What is the molar enthalpy of vaporization of propane? (Hint: Heating Curves graph)
a. 2.32 kJ/mol
b. 11.2 kJ/mol
c. 19.0 kJ/mol
d. 97.8 kJ/mol
e. 473 kJ/mol
c. 19.0 kJ/mol
q=nΔHvap
600
A 9.50 % by mass solution of acetone (C3H6O) in water has a density of 0.9849 g/mL at 20°C. What is the molarity of this solution?
A) 0.621 M
B) 1.61 M
C) 1.66 M
D) 1.71 M
E) 16.9 M
B) 1.61M
600
Phosgene, COCl2, a poisonous gas, decomposes according to the equation COCl2(g)->CO(g) + Cl2(g). Calculate Kp for this reaction if Kc = 0.083 at 900 degrees C. (R=0.0821 L*atm/mol *K)
A) 0.125
B) 8.0
C) 6.1
D) 0.16
B) 8.0
Kp=Kc(RT)Δ n
600
What is the H3O+ concentration of an aqueous solution with a pH of 12.17?
a. 6.8 × 10-13 M b. 1.9 × 10-9 M
c. 5.2 × 10-6 M d. 1.5 × 10-2 M e. 1.1 M
a. 6.8 × 10-13 M
10-12.17 =[H]
600
Calculate the pH of a buffer solution that contains 0.25 M benzoic acid (C6H5COOH) and 0.15M sodium benzoate (C6H5COONa). [Ka = 6.5*10-5 for benzoic acid]
A) 3.97 B) 4.83 C) 4.19 D) 3.40 E) 4.41
A) 3.97
(pH=-log(Ka)+log(conj. base/ acid)
600
Complete and balance the following redox equation that occurs in acidic solution using the set of smallest whole-number coefficients. What is the sum of all the coefficients in the equation?
PbO2(s) + Cl- → Pb2+ + Cl2(g) (acidic solution)
A) 2 B) 4 C) 5 D) 9 E) 11
E) 11
600
In George Orwell’s 1984, what is the name of the totalitarian regime’s leader?
Big Brother
700
Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of iodine trichloride, ICl3.
A) The e- pair geometry is tetrahedral, the molecular geometry is trigonal-planar.
B) The e- pair geometry is trigonal-bipyramidal, the molecular geometry is T-shaped.
C) The e- pair geometry is tetrahedral, the molecular geometry is trigonal-pyramidal.
D) The e- pair geometry is trigonal-planar, the molecular geometry is trigonal-planar.
E) The e- pair geometry is trigonal-bipyramidal, the molecular geometry is trigonal-planar.
B) The e- pair geometry is trigonal-bipyramidal, the molecular geometry is T-shaped.
700
Hydrogen bonding is present in which of the following molecular solids?
1) Formic Acid
2) Dimethyl Ether
3) Ammonia
4) Pentanol
A) 1, 2, and 4
B) 1, 3, and 4
C) 1, 2, 3, and 4
D) none of them
B) 1, 3, and 4
700
What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH) dissolved in enough water to make 500 mL of solution at 27°C? (R=0.0821 atm/M*K)
A) 0.014 atm
B) 0.037 atm
C) 0.456 atm
D) 0.01 atm
E) 11.2 atm
E) 11.2 atm
π = iMRT
700
For the first-order decomposition of N2O5 at 340 K, where k = 5.8 × 10-3 s-1, calculate the original concentration if the concentration of N2O5 is 0.41 M after 209 seconds.
a. 0.12 M
b. 0.23 M
c. 0.72 M
d. 1.4 M
e. 1.7 M
Around 1.4M
*ln[A]t=-kt+ ln[A]o*
700
What is the pH of an aqueous solution of 0.30 M HF and 0.15 M F- ? (Ka of HF = 7.2 × 10-4) (Hint: Buffer Solution)
a. 1.83 b. 2.84 c. 3.14 d. 3.44 e. 10.86
b. 2.84
pH=pKa+ [conj base]/[acid]
700
The solubility product for chromium(III) fluoride is Ksp = 6.6 × 10-11. What is the molar solubility of chromium(III) fluoride? (Hint: Ksp=[as]a[bs]b)
A) 1.6 × 10-3M D) 2.2 × 10-3 M
B) 1.2 × 10-3 M E) 1.6 × 10-6 M
C) 6.6 × 10-11 M
B) 1.2 × 10-3 M
700
Al3+ is reduced to Al(s) at an electrode. If a current of 2.00 ampere is passed for 48 hours, what mass of aluminum is deposited at the electrode? Assume 100% current efficiency. (mol x = A*t/nF)
a. 3.58 g b. 32.2 g c. 48.3 g d. 96.6 g
e. 2.90 × 102 g
b. 32.2 g
Current: 2 Amp.
Time: 48 hours ->172800 seconds
F=96500 C/mol
n(electrons per mol of Al)=3
700
What is the largest organ in the human body?
The skin