Download Haley CHM2045 Final Review

CHM2045 Study Union Final Review
Fall 2015
Chapter One
1. Classify each substance as a pure substance or a mixture. If it is a pure substance, classify
it as an element or a compound. If it is a mixture, classify it was homogeneous or
heterogeneous.
1. Gold
2. Vegetable soup
3. Carbon Dioxide
4. Kool-Aid
2. Convert 331 K to degrees F.
3. Calculate each to the correct number of significant figures.
1. (221.5 x 32.4) + 12 =
2. (54.0003 x 2.7004)/ 12.7 =
3. 55.9 + 2.03 =
4. Classify each property as physical or chemical.
1. the tendency of ethyl alcohol to burn
2. the shine of silver
3. the smell of paint
4. the density of water
5. Based on the diagram, classify each as a
physical or chemical change.
Important Things from Chapter One
D=M/V
1 mL=1cm3
Rules for Significant Figures:
1. In multiplication and division, the result has the same amount of sig figs as the factor
with the fewest sig figs.
2. In addition and subtraction, the result has the same number of places after the
decimal as the quantity with the fewest spaces after the decimal.
3. ROUND ONLY THE FINAL ANSWER
Chapter Two
1. A hydrogen filled balloon was ignited and 3.70 g of hydrogen reacted with 17.3 g of oxygen.
How many moles of water vapor was formed assuming it was the only product? How many
grams?
2. Determine the number of protons, neutrons, and electrons in each of the following isotopes.
1. K-40
2. Ra-226
3. N-14
4. Br-85
3. Calculate the mass in g of each sample.
1. 1.22 x 1027 Manganese atoms
2. 4.3 moles of Carbon Dioxide
4. Copper has two naturally occurring isotopes: Cu-63 with a mass of 62.9396 amu and a
natural abundance of 69.17%, and Cu-65 with a mass of 64.9278 amu and a natural
abundance of 30.83%. Calculate the atomic mass of Copper. (p.67)
5. Determine the number of atoms in 1.85 mL of mercury assuming it has a density of 13.5
g/mL.
Important Things from Chapter Two
Chapter Three
1. Calculate the mass percent of of carbon in each of the following compounds.
1. C2H5Cl
2. C2H6
2. Name each of the following.
1. CF4
2. Li3(PO4)
3. H2CO3
4. Pb(SO4)
3. Propose a formula for each of the following.
1. Copper (II) Fluoride
2. Boron Trichloride
3. Sulfurous Acid
4. Aluminum Oxide
4. Balance the following reactions.
1. ___ AlBr3 + ____ K2SO4 —> ____ KBr + ____ Al2(SO4)3
2. ____ CF4 + ____ Br2 —> ____ CBr4 + ____ F2____
3. Na3PO4 + ____ KOH —> ____ NaOH + ____ K3PO4
5. The elemental mass percent composition of Vitamin C is 40.92% C, 4.58% H, and 54.50%
O. Determine the empirical formula.
Important Things from Chapter Three
KNOW THE POLYATOMIC IONS
Chapter Four
1. Starting with 86.3 g NO and 25.6 g H2, find the theoretical yield of ammonia in grams.
2NO + 5H2 —> 2NH3 + 2H2O
2. If you dissolve 35.5 g of LiBr in enough water to make 2.25 L of solution, what is the molarity
of the solution?
3. Write a complete ionic and net ionic equations for the following reaction.
2KOH (aq) + H2SO4 (aq) —> 2H2O + K2SO4
4. Identify the oxidizing agent and reducing agent in the following reaction
CO2 + H2 —> CO + H2O
5. Write a balanced equation for the combustion of liquid butanol (C4H9OH)
Important Things from Chapter Four
KNOW YOUR REACTIONS
-Combustion: Oxygen in reactants, water and carbon dioxide as products
-Redox: Change in oxidation states
-Precipitation: yields a solid from two aqueous reactants
-Acid/Base (Neutralization): Acid + Base yields water and a salt
-Gas Evolution
KNOW YOUR SOLUBILITY RULES
Chapter Five
1. Calculate the density of hydrogen gas at 150 degrees Celsius and a pressure of 725
mmHg.
2. A 1.0 L mixture of He, Ar, and Ne has a total pressure of 654 mmHg at 298 K. If the partial
pressure of He is 378 mmHg and the partial pressure of Ne is 112 mmHg, what is the
partial pressure of Ar?
3. Lithium reacts with nitrogen gas in the following reaction, 6Li + N2 —> 2Li3N What mass
of lithium reacts completely with 58.5 mL of N2 gas at STP?
4. What is the pressure in a 15.0 L cylinder filled with 27.2 g of oxygen gas at a temperature of
302 K?
5. A sample of a gas has an initial volume of 14.1 L at a pressure of 2.31 atm. If the sample is
compressed to a volume of 10.3 L, what is the resulting pressure?
Important Things from Chapter Five
Boyles Law- P1V1=P2V2
Charles Law- V1/T1=V2/T2
Avogadro’s Law- V1/n1=V2/n2
Ideal gas law- PV=nRT
Mole fraction= X= mol part/total mol
Partial pressure= X*total pressure
D= (P*mm)/RT
KNOW THE CONCEPTS BEHIND THESE EQUATIONS
Chapter Six
1. When 2.37 g of glucose (C6H11O6) undergoes combustion in a bomb calorimeter, the
temperature rises from 37.5 degrees C to 89.2 degrees C. Find the change in energy for the
combustion of glucose in kJ/mol. The heat capacity of the calorimeter, determined in a
separate experiment, is 4.90 kJ/degreeC.
2. Label each of the following as endothermic or exothermic
1. Sweat evaporating from the skin
2. Water vapor condensing on a window
3. Ice sublimating A gas tank contains 15.7 g of butane, C4H10
4. Wood burning in a fire
3. . Calculate the heat in kJ associated with the complete combustion of all the butane in the
tank.
2C4H10 + 13O2 —> 8CO2 + 10H2O
deltaH= -2044 kJ
4. There is a sample 22 g of water in a coffee cup calorimeter initially at 32 degrees Celsius.
After absorbing 5.3 kJ of heat, what is the final temperature?
5. 2 C (s) + 2H2O (g) —> CH4 (g) + CO2 (g)
Determine the standard enthalpy change for
this reaction from the following standard enthalpies of reaction:
1. C (s) + H2O (g) —> CO (g) + H2 (g)
deltaH= 131.3 kJ
2. CO (g) + H2O (g) —> CO2 (g) +H2 (g)
deltaH= -41.2 kJ
3. CH4 (g) + H2O (g) —> 3H2 (g) + CO (g) deltaH= 206.1 kJ
Important Things from Chapter Six
Bomb calorimetry- q=c*deltaT
Coffee cup calorimetry- q=m*c*deltaT
w=-P*deltaV
deltaH= deltaE + P*deltaV
deltaE= q + w
Chapter Seven
1. According to the quantum-mechanical model for the hydrogen atom, which electron
transition would produce light with the longer wavelength, 2p —> 1s or 3p —> 1s?
2. Calculate the wavelength of the light emitted when an electron in a hydrogen atom makes
the transition n=3 —> n=2.
3. Which of the following sets of quantum numbers is impossible?
1. n=3 l=2 ml=0
2. n=4 l=1 ml=-2
3. n=3 l=1 ml=-1
4. n=2 l=0 ml=0
4. Calculate the energy of an electro magnetic radiation with a frequency of 7.0 x 1013 s-1.
5. Calculate the frequency of an electromagnetic radiation with a wavelength of 752.7 nm.
Important Things from Chapter Seven
Energy and wavelength are inversely proportional
Chapter Eight
1. Find the electron configuration of the following elements
1. Cu
2. Ar
3. Br
2. Place the following in order of decreasing electron affinity. Na, F, Cl, Ge, N
3. Place the the same elements in order of increasing metallic character.
4. Use the periodic table to identify the element of each electron configuration
1. [Ar] 4s2 3d10 4p6
2. [Kr] 5s2
5. Choose the larger atom of each pair
1. Sn or Si
2. Br or Ga
3. C or F
Important Things from Chapter Eight
KNOW THE PERIODIC TRENDS
Pauli Exclusion Principle: no two electrons in an atom can have the same four quantum
numbers
Aufbau Principle: The lowest energy orbitals must be filled first
Hund’s Rule: When filling orbitals, electrons must be filled singly at first with parallel spins
Chapter Nine
1. Place the following compounds in order of decreasing lattice energy: NaCl, CaO, HCl
2. Draw the lewis structures of the following compounds
1. NO212. CO323. SeCl5
3. Place the following compounds in order of increasing electronegativity: HI, BeF, LiI, CO2
4. Which of the following compounds are polar?
1. H2O
2. CF4
3. HCCl3
4. O2
5. Order the compounds in order of increasing carbon-carbon strength, HCCH, H2CCH2,
H3CCH3
Important Things From Chapter Nine
Know the periodic trends for lattice energy and electronegativity
Know Born Haber Cycle Steps
Chapter Ten
1. What is the bond order of He2? What does this bond order mean?
2. Determine the electron and molecular geometries of the following compounds
1. H2O
2. BF3
3. SeCl6
3. Name the hybridization scheme in each electron geometry
1. tetrahedral
2. linear
3. trigonal planar
4. Determine the hybridization of each carbon atom in the following caffeine molecule
Important Things From Chapter Ten