Chem Final

The moles of oxygen in a sample of 1.55 grams Ca3(PO4)2 are: (MW = 310.174 g/mol) a. 4.00 x 10-2 moles oxygen b. 2.00 x 10-2 moles oxygen. c. 6.25 x 10-4 moles oxygen. d. 1.00 x 10-2 moles oxygen. e. 2.41 x 1023 moles oxygen.

a. 4.00 x 10-2 moles oxygen

The average atomic mass of calcium is 40.078 amu. Which is the most abundant isotope of calcium? a. 40Ca. b. 41Ca. c. 42Ca. d. 43Ca. e. 44Ca.

a. 40Ca.

The mass of 0.500 moles of acetaminophen (C8H9NO2) is a. 75.6 grams. b. 68.6 grams. c. 48.0 grams. d. 21.5 grams. e. 151 grams.

a. 75.6 grams.

The covalent compound listed that exhibits the strongest intermolecular force interactions is: a. C10H22. b. C6H14. c. C3H8. d. C2H6. e. CH4.

a. C10H22.

The gas with the greatest density at STP (273 K & 1 atm) is: a. Chlorine (Cl2). b. Hydrogen (H2). c. Nitrogen (N2). d. Neon (Ne). e. Oxygen (O2).

a. Chlorine (Cl2).

The chemical formula for the neutral ionic compound that forms from Cu2+ and SO42- is: a. CuSO4. b. Cu2SO4. c. Cu(SO4)2. d. Cu2S2O8 e. none of these

a. CuSO4.

Arrange the following atoms in order of increasing atomic (covalent) radii. a. F < Cl < Br < I b. I < Br < Cl < F c. Cl < Br < I < F d. Br < Cl < I < F e. none of these are in the correct order

a. F < Cl < Br < I

Based on the enthalpies of atom combination given, the strongest bond listed is: a. H-F (∆Ho ac = - 567.7 kJ/molrxn). b. H-I (∆Ho ac = - 298.0 kJ/molrxn). c. H-Br (∆H ac = - 365.9 kJ/molrxn). d. H-Cl (∆H ac = - 431.6 kJ/molrxn). e. H-H (∆H ac = - 435.3 kJ/molrxn)

a. H-F (∆Ho ac = - 567.7 kJ/molrxn).

The compound that contains hydrogen in a negative oxidation state is: a. LiH. b. H2CO3. c. H2. d. LiOH. e. HF.

a. LiH.

For small molecules with similar molar masses, the intermolecular forces listed in order of increasing strength is: a. London dispersion forces < dipole-dipole forces < hydrogen bond forces. b. London dispersion forces < hydrogen bond forces < dipole-dipole forces. c. dipole-dipole forces < hydrogen bond forces < London dispersion forces. d. dipole-dipole forces < London dispersion forces < hydrogen bond forces. e. hydrogen bond forces < dipole-dipole forces < London dispersion forces.

a. London dispersion forces < dipole-dipole forces < hydrogen bond forces.

The bond with the greatest covalent character, based on the bond-type triangle is: a. N - O. b. C - O. c. H - O. d. S - O. e. Cl - O.

a. N - O.

When applying the ideal gas law, the specification listed below that is not important is: a. The chemical identity of the gas sample b. The temperature of the gas sample c. The pressure of the gas sample d. The volume of the container holding the gas sample e. These are all important.

a. The chemical identity of the gas sample

Which of the following ions is isoelectronic (has same electron configuration) with Kr? a. Y 3+ b. K + c. I - d. Ba2+ e. Cl

a. Y6^3+

The following postulates from Dalton's atomic theory now considered incorrect are: I. All the atoms of a given element are identical. II. Matter consists of very small particles known as atoms. III. Atoms are indestructible and also indivisible. IV. In a given compound, the atoms are always present in the same fixed numerical ratio. a. I and II b. I and III. c. I and IV. d. II and III. e. III and IV.

b. I and III.

The process that is accompanied by a decrease in entropy is: a. Rolling a pair of dice. b. Assembling a Lego® spaceship. c. Letting your toys pile up on the floor. d. Shooting Nerf® darts at the ceiling. e. Shuffling a deck of cards.

b. Assembling a Lego® spaceship.

A nonmetal in the same group as indium is: a. C - Carbon. b. B - Boron. c. Al - Aluminum. d. Tl - Thallium. e. I - Iodine.

b. B - Boron.

A covalent compound for which dipole-dipole forces are the strongest interaction is: a. CO2. b. CH3F. c. H2O. d. NaNO3. e. CH3OH.

b. CH3F.

The process that results in the largest net energy released from the system: a. CO2 (g) CO2 (l). b. CO2 (g) CO2 (s). c. CO2 (l) CO2 (g). d. CO2 (l) CO2 (s). e. CO2 (s) CO2 (l).

b. CO2 (g) CO2 (s).

Molality is: a. Moles solute per liter of solvent. b. Moles solute per kilogram of solvent. c. Moles solute per kilogram of solution. d. Grams solute per kilogram of solvent. e. Grams solute per liter of solution.

b. Moles solute per kilogram of solvent.

A common air pollutant was determined to contain 30.4% nitrogen and 69.6% oxygen by weight. The empirical formula for this compound is: a. NO. b. NO2. c. NO3. d. N2O. e. N3O

b. NO2.

An example of a chemical compound is: a. Brass (Cu and Zn solution). b. Rust (Fe2O3). c. Silicon chip (Si). d. Iron metal (Fe). e. Oxygen gas (O2).

b. Rust (Fe2O3).

8. During the decomposition of a metal chlorate at 21oC, the oxygen gas is collected by displacement of water in a gas collection bottle. The vapor pressure of water at 21oC is 19.0 mmHg and the gas collected has total pressure of 0.25 atm. The partial pressure of the oxygen gas is: a. 24.1 atm. b. 23.5 atm. c. 0.28 atm. d. 0.23 atm. e. 0.03 atm.

d. 0.23 atm.

. A young girl is given a 1.00L red balloon at the top of Pike's Peak, where it's a sunny 2°C. She boards a cog returning from the summit to the base of the mountain. As the train descends, the atmospheric pressure increases from 450 mmHg at the 14,110 ft summit to 755 mmHg at the base, where it's a much warmer 27°C. The volume of the balloon when the train reaches the base is: (assume unlimited shrinkability & expandability of the balloon) a. 13.5L. b. 8.05L c. 1.10L. d. 0.65L. e. 0.60L.

d. 0.65L.

The pressure inside a 2.5 liter propane tank filled with 0.56 moles propane at 25.2°C is: a. 0.0072 atm. b. 0.46 atm. c. 0.72 atm. d. 5.4 atm. e. 4100 atm.

d. 5.4 atm.

The volume of O2 gas required to completely react with 17.6 liters NO gas to form NO2 gas, if both gases are at standard temperature and pressure, is: 2 NO(g) + O2 (g) 2 NO2 (g) a. 22.4 L. b. 17.6 L. c. 11.2 L. d. 8.82 L. e. 4.41 L.

d. 8.82 L.

The non-polar molecule shown below is: a. CO. b. CHF3. c. OCS. d. CS2. e. H2O.

d. CS2

The most likely product of the reaction between calcium and sulfur would be: a. Ca2S3. b. CaS2. c. Ca2S. d. CaS e. Ca3S

d. CaS

The empirical formula for an unknown compound is determined to be HO. If the molecular weight of the compound is 33.994 g/mol, what is its molecular formula? a. HO b. H2O c. HO2 d. H2O2 e. (H2O)2

d. H2O2

An example of a homogeneous mixture is: a. Blueberry bagel. b. Orange juice, with pulp. c. Raisin Bran. d. Hot coffee w/ cream. e. Pop Tarts.

d. Hot coffee w/ cream.

Molarity is a unit defined as: a. Grams of solute dissolved in 1 liter of solution. b. Grams of solute dissolved in 1 kilogram of solvent. c. Moles of solute dissolved in 1 kilogram of solvent. d. Moles of solute dissolved in 1 liter of solution. e. Moles of solute dissolved in 1 mole of solution.

d. Moles of solute dissolved in 1 liter of solution.

An example of a chemical change is: a. Dry ice seems to vanish as it sublimes. b. Steam from boiling water condenses on the ceiling. c. The nitrogen gas is cooled until it finally becomes a liquid. d. The solid copper metal turns green as it forms a patina. e. The table salt is broken into smaller pieces in the salt grinder.

d. The solid copper metal turns green as it forms a patina.

The object that will heat (and cool) the fastest, assuming equal molar quantities of each is: a. Water CP = 75.3 J/K⋅mol. b. Iron skillet CP = 25.1 J/K⋅mol. c. Copper pot CP = 24.4 J/K⋅mol. d. Aluminum pan CP = 24.3 J/K⋅mol. e. Charcoal brick CP = 8.52 J/K⋅mol.

e. Charcoal brick CP = 8.52 J/K⋅mol.

The most polar bond in the list below is: a. O - N. b. O - Br. c. O - C. d. O - S. e. O - H.

e. O - H.

The Lewis symbol that has eight valence electrons is the: a. Sc2+ ion. b. Ar+ion. c. C atom. d. Li-ion. e. O2- ion.

e. O2- ion

Which atom has the following electron configuration: [Ne]3s2,3p3 ? a. B b. N c. Si d. Al e. P

e. P

Lithium reacts with a second element (represented here by the symbol E) to form an ionic compound with formula LiE. Element E is most probably from group: a. IIIA (13) b. IVA (14) c. VA (15) d. VIA (16) e. VIIA (17)

e. VIIA (17)

The reaction that results in an increase in entropy of the reaction system is: a. BaO (s) + CO2 (g) BaCO3 (s) b. CO (g) + 3 H2 (g) CH4 (g) + H2O (l) c. Na2CO3 (s) + CO2 (g) + H2O (g) 2 NaHCO3 (s) d. N2 (g) + 3 H2 (g) 2 NH3 (g) e. ZnO (s) + SO2 (g) ZnS (s) + 3/2 O2 (g)

e. ZnO (s) + SO2 (g) ZnS (s) + 3/2 O2 (g)

According to the kinetic theory of gases, the temperature of the gas particles in a gas sample is directly proportional to the: a. molar mass of the gas. b. number of moles of gas. c. shape of the gas particles. d. size of the gas particles. e. kinetic energy of the gas.

e. kinetic energy of the gas.

The solubility of a compound is determined by the strength of the: a. solute-solute interactions. b. solute-solvent interactions. c. solvent-solvent interactions. d. intramolecular bonds in the solute and solvent. e. solute-solute, solute-solvent, and solvent-solvent interactions.

e. solute-solute, solute-solvent, and solvent-solvent interactions.

What mass of PI3 may be produced when 7.0 g of P and 68.1 g of I2 are reacted according to the following reaction: 2P (s) + 3I2 (g) → 2PI3 (s) (MW: P = 30.97g/mol, I2 = 253.80g/mol, PI3 = 411.67 g/mol) a. 0.268 mol b. 73.6 g c. 92.9g d. 110 g e. 0.179 mol

b. 73.6 g

In a closed container, the following reaction is allowed to come to equilibrium. 2 NO (g) + O2 (g) 2 NO2 (g) ∆Hrxn = - 118.9 kJ/molrxn A change that causes a decrease in the O2 gas concentration as it returns to equilibrium is: a. adding more NO gas through an injection nozzle. b. increasing the volume of the reaction container. c. increasing the temperature of the reaction system. d. decreasing the pressure of the reaction system. e. adding NO2 gas from the reaction system.

a. adding more NO gas through an injection nozzle.

If you had 1.0 g of each of the following substances, which would occupy the greatest volume? a. olive oil (d = 0.89 g/mL) b. cocoa butter (d = 0.91 g/mL) c. ice (d = 0.917 g/mL) d. beeswax (d = 0.96 g/mL) e. water (d = 0.997 g/mL)

a. olive oil (d = 0.89 g/mL)

Electrons can have certain fixed energies and not others, because the energy of the electron is a. quantized. b. negative. c. a wave. d. orbital. e. small.

a. quantized.

In an ionic bond valance electrons are: a. transferred to the most electronegative atom. b. transferred to the least electronegative atom. c. shared between two atoms with high electronegativity. d. shared between two atoms with low electronegativity. e. shared between two atoms with different electronegativities.

a. transferred to the most electronegative atom.

The thermochemical equation for the standard enthalpy of formation (∆Hf) for HCl is: a. ½ H2 (g) + ½ Cl2 (g) HCl (g) b. H2 (g) + Cl2 (g) 2 HCl (g) c. H (g) + Cl (g) HCl (g) d. H (g) + Cl (g) HCl (l) e. HCl (g) ½ H2 (g) + ½ Cl2 (g)

a. ½ H2 (g) + ½ Cl2 (g) HCl (g)

The oxidation number of chlorine in sodium hypochlorite (NaClO) is: a. +2. b. +1. c. -1. d. -2. e. -3.

b. +1.

The solubility of barium sulfate (Ksp = 1.1 x 10-10 at 25oC) in aqueous solution is: a. 2.1 x 10-5M BaSO4 b. 1.0 x 10-5 M BaSO4 c. 1.1 x 10-10 M BaSO4 d. 5.5 x 10-11 M BaSO4 e. 1.2 x 10-20 M BaSO4

b. 1.0 x 10-5 M BaSO4

For the reaction: N2 (g) + 3 H2 (g) 2 NH3 (g) ∆H = - 92.4 kJ/molrxn The amount of enthalpy released from the reaction system when 1.00 mol H2 gas reacts is: a. 15.4 kJ. b. 30.8 kJ. c. 46.2 kJ. d. 185. kJ. e. 277. kJ.

b. 30.8 kJ.

During discharge of a lead-acid storage battery, the following chemical reaction takes place: 2PbSO4 + 2H2O Pb + PbO2 + 2H2SO4 Based on the ∆H values below, the ∆H°rxn for the battery discharge reaction is: Pb + PbO2 + 2SO3 2PbSO4 ∆H° = -775 kJ SO3 + H2O H2SO4 ∆H° = -113 kJ a. - 662 kJ/molrxn. b. 549 kJ/molrxn. c. 662 kJ/molrxn. d. 888 kJ/molrxn. e. 1001 kJ/molrxn.

b. 549 kJ/molrxn.

Coca Cola® is an aqueous solution containing 65 grams sugar in one 20 oz bottle, whereas an 8.0 oz can of RockStar® energy drink contains 31 grams sugar. The correct statement about these drinks is: a. The sugar is exactly the same concentration in Coca Cola and Rock Star. b. The sugar is less concentrated in the Coca Cola than the Rock Star. c. The sugar is more concentrated in the Coca Cola than the Rock Star. d. The Rock Star has more solute than the Coca Cola. e. The Coca Cola has less solvent than the Rock Star.

b. The sugar is less concentrated in the Coca Cola than the Rock Star.

Electronegativity decreases from top to bottom, down a group (column), due to: a. a decrease in the core charge. b. an increase in the distance of the valence electrons from the nucleus. c. an increase in the shielding of the core electrons by the valence electrons. d. a decrease in the shielding of the valence electrons by the core electrons. e. a decrease in the total number of protons in the nucleus.

b. an increase in the distance of the valence electrons from the nucleus.

When sodium metal reacts with sulfur to form an ionic compound, in the process, each sulfur atom: a. gains one electron. b. gains two electrons. c. loses two protons. d. loses one proton. e. loses one electron.

b. gains two electrons.

The Lewis symbol that has five valence electrons is: a. chlorine. b. phosphorus. c. aluminum. d. rubidium. e. strontium.

b. phosphorus.

When a reaction reaches equilibrium a. the forward and reverse reaction rates stop. b. the forward rate is the same as the reverse rate of reaction. c. the concentrations of the products and reactants become equal. d. the concentrations of the products and reactants continue to change. e. both b and c are true.

b. the forward rate is the same as the reverse rate of reaction.

During an exothermic chemical reaction, a surroundings become: a. warmer, as the reaction system undergoes an increase in potential energy. b. warmer, as the reaction system undergoes a decrease in potential energy. c. cooler, as the reaction system undergoes an increase in potential energy. d. cooler, as the reaction system undergoes a decrease in potential energy. e. Nothing happens to the surroundings!

b. warmer, as the reaction system undergoes a decrease in potential energy.

For a particular chemical reaction, ∆H > 0 and ∆S < 0, therefore this reaction: a. will always be spontaneous, regardless of temperature. b. will never be spontaneous, regardless of temperature. c. might be spontaneous, but spontaneity is favored at low temperatures. d. might be spontaneous, but spontaneity is favored at high temperatures. e. spontaneity cannot be predicted with the information given.

b. will never be spontaneous, regardless of temperature.

What is the core charge for the carbon atom, C? a. +1 b. +2 c. +4 d. +6 e. +8

c. +4

. A sealed glass container containing 0.80 moles O2 and 0.40 moles N2 gas has a total pressure inside the container of 0.90 atm. The partial pressure of the O2 gas is: a. 0.30 atm. b. 0.40 atm. c. 0.60 atm. d. 0.67 atm. e. 0.90 atm.

c. 0.60 atm.

The concentration of a sample of saltwater is 0.250 M NaCl. After evaporating 150.0 mL of the saltwater solution to dryness, the mass of sodium chloride (NaCl) left is: a. 0.0375 g. b. 1.67 g. c. 2.18 g. d. 21.8 g. e. 96.6 g.

c. 2.18 g.

When 7.00 g of NH4Cl is added to 18.8 g of water the molal concentration of the solution is: a. 0.372 m. b. 0.131 m. c. 6.96 m d. 53.5 m. e. 372 m.

c. 6.96 m

. Based on its Lewis structure, the atoms in the oxygen molecule (O2) are held together by: a. a single covalent bond. b. an ionic bond. c. a double covalent bond. d. a triple covalent bond. e. a magnetic dipole bond.

c. a double covalent bond.

As sodium sulfate (Na2SO4) is added to a saturated (equilibrium) solution of BaSO4 (Ksp = 1.1 x 10-10), the concentration of Ba2+ in solution will: a. decrease due to the ion suppression effect. b. increase due to the common ion effect. c. decrease due to the common ion effect. d. be unaffected because sodium sulfate is not soluble in water. e. be unaffected because sodium sulfate ions do not interfere with the dissolution of barium sulfate.

c. decrease due to the common ion effect.

The more polarizable a molecule, the stronger the induced dipole interactions; polarizability refers to the: a. magnitude of the dipole moment of a molecule. b. ease with which a dipole moment can ionize an atom or a molecule. c. ease with which the electron cloud of an atom or molecule can be perturbed. d. perturbation in a molecule's electron cloud due to hydrogen bonding. e. strength of the polar covalent bonds present in the molecule.

c. ease with which the electron cloud of an atom or molecule can be perturbed.

Of the following, the property describing an ionic compound is: a. malleable solid. b. low melting point. c. liquid form is a good conductor of electricity. d. solid form is a good conductor of heat. e. low electronegativity.

c. liquid form is a good conductor of electricity.

When diluting a 1.00 M NaOH solution to 0.100 M NaOH, a. the volume of the solution remains unchanged. b. the concentration of NaOH in the solution remains unchanged. c. the final volume of the solution must be 10X the initial volume. d. the initial volume of the solution must be 10X the final volume. e. the final moles of NaOH in solution will be 1 /10 the initial number of moles

c. the final volume of the solution must be 10X the initial volume.

At low temperatures and high pressures, the characteristic(s) of real gases that become significant (resulting in behavior that deviates from an ideal gas) is/are: a. the molecular volume of the gas. b. the attractive and repulsive forces between gas molecules. c. the molecular volume and the attractive/repulsive forces between gas molecules. d. the elastic collisions between gas molecules. e. the odor of the gas.

c. the molecular volume and the attractive/repulsive forces between gas molecules.

Yellow light has a frequency of 5.2 x 1014 s -1; red light has a frequency of 4.3 x 1014 s-1 . Which of the following correctly describes the relationship between the wavelength and energy of yellow versus red light? a. Red light has a shorter wavelength and less energy than yellow light. b. Red light has a shorter wavelength and more energy than yellow light. c. Yellow light has a shorter wavelength and less energy than red light. d. Yellow light has a shorter wavelength and more energy than red light. e. None of these.

d. Yellow light has a shorter wavelength and more energy than red light.

For a specific reaction, the equilibrium constant, Kc: a. increases if concentration of one of the products is decreased. b. increases if concentration of one of the products is increased. c. may be changed by addition of a catalyst. d. can change with temperature. e. always remains the same.

d. can change with temperature.

Lattice energy of a solid compound decreases with: a. decreasing ion radius. b. increasing ionic charge. c. increasing intermolecular forces. d. decreasing intermolecular forces and bond strength. e. increasing intermolecular forces and bond strength.

d. decreasing intermolecular forces and bond strength.

. The pair of compounds in this list that are most likely to be miscible (mix well) are: a. bromine (Br2) and water (H2O). b. ethanol (CH3CH2OH) and hexane (C6H14). c. carbon tetrachloride (CCl4) and methanol (CH3OH). d. methanol (CH3OH) and water (H2O). e. bromine (Br2) and ethanol (CH3CH2OH).

d. methanol (CH3OH) and water (H2O).

A resonance structure indicates that there is: a. more than one allotropic form of a compound. b. more than one ionic form of a compound. c. more than one isotopic form of an element. d. more than one Lewis structures representing the electron movement within the structure. e. more than one structural arrangements of the single bonds in a Lewis structure.

d. more than one Lewis structures representing the electron movement within the structure.

The correct set of quantum numbers designating a 4d orbital is: a. n = 3, l = 2, ml = -1 b. n = 4, l = 1, ml = -1 c. n = 4, l = 2, ml = -3 d. n = 4, l = 2, ml = 2 e. n = 4, l = 0, ml = 0

d. n = 4, l = 2, ml = 2

The subatomic particles that do not contribute to charge, but contribute significantly to the mass of the atom are the: a. electrons. b. neucleons. c. protons. d. neutrons. e. photons.

d. neutrons

. The loss of electrons describes the process known as: a. negation. b. positivity. c. reduction. d. oxidation. e. inflation.

d. oxidation.

The metal listed below that would react most rapidly and vigorously with water is: a. chromium. b. cobalt. c. gold. d. potassium. e. tungsten.

d. potassium.

A 1.00-L reaction system is injected with 0.100 moles H2, 0.100 moles X2 and 0.600 moles HX. Kc = 24.4 for the reaction, H2 (g) + X2 (g) 2 HX (g); therefore, the reaction will: a. proceed toward the right because Qc < Kc. b. proceed toward the right because Qc > Kc. c. proceed toward the left because Qc < Kc. d. proceed toward the left because Qc > Kc. e. be at equilibrium because Qc = Kc.

d. proceed toward the left because Qc > Kc.

. In the development of photographic film, the negative is produced in a redox reaction that involves hydrazine and silver bromide. N2H4 + 4 AgBr N2 + 4 HBr + 4 Ag The element being reduced in this reaction is: a. bromine. b. hydrogen. c. nitrogen. d. silver. e. silver and nitrogen.

d. silver.

2. Based on all the individual gas laws and hypotheses, the pressure of a gas is inversely proportional to the: a. amount of the gas (n). b. molarity of the gas (M). c. temperature of the gas (T). d. volume of the gas (V). e. density of the gas (d).

d. volume of the gas (V).

A chemical reaction is always spontaneous when: a. ∆H < 0. b. ∆G = 0. c. ∆S > 0. d. ∆G < 0. e. ∆G > 0.

d. ∆G < 0.

In the reaction 3 H2 (g) + N2 (g) 2 NH3 (g), the number of moles of hydrogen gas required to react with 1.50 moles nitrogen gas is: a. 0.500 mole H2. b. 1.50 mole H2. c. 2.00 moles H2. d. 3.00 moles H2. e. 4.50 moles H2.

e. 4.50 moles H2.