Chem 104 - Final Study

How many grams of NaOH are contained in 5.0 x 10^2 mL of a 0.83 M sodium hydroxide solution? a. 17 g b. 83 g c. 0.42 g d. 33 g e. 415 g

a. 17 g

What volume of 18 M sulfuric acid must be used to prepare 2.40 L of 0.175 M H2SO4? a. 23 mL b. 0.42 mL c. 1.3 x 10^3 mL d. 3.6 mL e. 7.6 mL

a. 23 mL

You mix 55 mL of 1.00 M silver nitrate with 25 mL of 1.17 M sodium chloride. What mass of silver chloride should you form? a. 4.2 g b. 8.4 g c. 4.6 g d. 9.2 g e. None of these

a. 4.2 g

Adipic acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a. C3H5O2 b. C3H3O4 c. C2HO3 d. C2H5O4 e. C3HO3

a. C3H5O2

Four identical 1.0 L flasks contain the gases He, CL2, CH4, and NH3 , each at 0 deg C and 1 atm pressure. In which gas do the molecules have the highest velocity? a. He b. Cl2 c. CH4 d. NH3 e. All gases have the same highest average velocity

a. He

Liquids with large intermolecular forces tend to have high surface tension True False

True

Using the information below, calculate [Delta H Fusion] for PbO(s) PbO(s) + CO(g) -> Pb(s) + CO2(g) [Delta H]= -131.4 kJ [Delta H Fusion] for CO2(g)= -393.5 kJ/mol [Delta H Fusion] for CO(g)= -110.5 kJ/mol a) -151.6 kJ/mol b) -283.0 kJ/mol c) +283.0 kJ/mol d) -372 kJ/mol e) +252.1 kJ/mol

a) -151.6 kJ/mol

How many p orbitals have the value n=1? a) 0 b) 3 c) 5 d) 7 e) 1

a) 0

Bromine exists naturally as a mixture of bromine- 79 and bromine- 81 isotopes. An atom of bromine- 79 contains ____________. a) 35 protons, 44 neutrons, 35 electrons b) 34 protons and 35 electrons, only c) 44 protons, 44 electrons, and 35 neutrons d) 35 protons, 79 neutrons, and 35 electrons e) 79 protons, 79 electrons, and 35 neutrons

a) 35 protons, 44 neutrons, 35 electrons

What is the wavelength of a photon of red light (in nm) whose frequency is 4.58 x 10^14 Hz? a) 655 nm b) 1.53 x 10^6 nm c) 153 nm d) 458 nm e) None of these

a) 655 nm

How many molecules of ammonia, NH3, are present in 0.121 moles of ammonia? a) 7.29 x 10^22 b) 2.01 x 10^-25 c) 2.91 x 10^23 d) 1.21 x 10^-1 e) 1.45

a) 7.29 x 10^22

Which of the following molecules contains a double bond? a) CO2 b) NH3 c) H2O d) all e) none

a) CO2

Which of the following has the smallest radius? a) K+ b) Cl- c) Rb+ d) S^2- e) Ar

a) K+

Which of the following atoms or ions has three unpaired electrons? a) N b) O c) Al d) S^2- e) Ti^2+

a) N

Order the elements S, Cl, and F in terms of increasing ionization energy. a) S, Cl, F b) Cl, F, S c) F, S, Cl d) F, Cl, S e) S, F, Cl

a) S, Cl, F

The Lewis structure for CHCl3 has nine lone electron pairs. a) True b) False

a) True

Which of the following combinations of quantum numbers is not allowed? a) n=1, l=1, ml=0, ms=1/2 b) n=3, l=0, ml=0, ms=-1/2 c) n=2, l=1, ml= -1, ms=1/2 d) n=4, l=3, ml=-2, ms=-1/2 e) n=4, l=2, ml=0, ms=1/2

a) n=1, l=1, ml=0, ms=1/2

How many resonance structures can be drawn for the molecule O3? a) 1 b) 2 c) 3 d) 4 e) 5

b) 2

If n=2, how many orbitals are possible? a) 3 b) 4 c) 2 d) 8 e) 6

b) 4

What is the wavelength of light that is emitted when an excited electron in the hydrogen atom falls from n=5 to n=4? a) 2.47 x 10^5 m b) 4.05 x 10^-6 m c) 4.90 x 10^-20 m d) 1.46 x 10^-6 m e) None of these

b) 4.05 x 10^-6 m

For the elements Ba, F, and N, the order of increasing electronegativity is: a) Ba < F < N b) Ba < N < F c) N < F < Ba d) F < Ba < N e) None of these

b) Ba < N < F

Phosphoric acid can be prepared by the reaction of sulfuric acid with "phosphate rock" according to the equation: Ca3(PO4)2 + 3H2SO4 -> 3CaSO4 + 2H3PO4 a. Ca3(PO4)2 b. H2SO4 c. CaSO4 d. H3PO4 e. none of these

b) H2SO4

The electron configuration for the barium atom is _______. a) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 b) [Xe]6s^2 c) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 d) 1s^2 2s^2 sp^6 3s^2 3p^6 4s^2 e) None of these

b) [Xe]6s^2

The oxidation state of chlorine in ClO2^- is ______. a. 0 b. +3 c. -3 d. +5 e. -5

b. +3

The empirical formula of styrene is CH; it's molar mass is 104.1 g/mol. What is the molecular formula of styrene? a. C2H4 b. C8H8 c. C10H12 d. C6H6 e. None of these

b. C8H8

Which of the following compounds have the lowest viscosity? a. CCl4 (l) b. N2 (g) c. H2O (l) d. CH3 - (CH2)25 - CH3 (l) e. HCl (g)

b. N2 (g)

In which of the following does nitrogen have an oxidation of +4? a. HNO3 b. NO2 c. N2O d. NH4Cl e. NaNO2

b. NO2

In the reaction N2(g) +3H2(g) -> 2NH3(g), N2 is: a. Oxidized b. Reduced c. The electron donor d. The reducing agent e. Two of these

b. Reduced

In the reaction 2Cs(s) + Cl2(g) -> 2CsCl(s), Cl2 is: a. The reducing agent b. The oxidizing agent c. Oxidized d. The electron donor

b. The oxidizing agent

In the cyanide ion (CN-), the nitrogen has a formal charge of ________. a) -2 b) -1 c) 0 d) 2 e) More information is needed.

c) 0

Using the following thermochemical data: 2Ga(s) + 6HF(g) -> 2GaF3(s) + 3H2(g) [Delta H]= -699.4 kJ/mol 2Ga(s) + 6HCl(g) -> 2GaCl3(s) + 3H2(g) [Delta H]= -495.6 kJ/mol Calculate [Delta H] for the following reaction: GaF3(s) + 3HCl(g) -> GaCl3(s) + 3HF(g) a) -1195.0 kJ/mol b) 203.8 kJ/mol c) 101.9 kJ/mol d) 407.6 kJ/mol e) -597.5 kJ/mol

c) 101.9 kJ/mol

How many of the following postulates of Dalton's atomic theory are still scientifically accepted? I. All atoms of the same element are identical. II. Compounds are combinations of different atoms. III. A chemical reaction changes the way atoms are grouped together. IV. Atoms are indestructible. a) 0 b) 1 c) 2 d) 3 e) 4

c) 2

Yellow light can have a wavelength of 576 nm. The energy of a photon of this light is: a) 1.14 x 10^-31 J b) 5.76 x 10^-7 J c) 3.45 x 10^-19 J d) 5.20 x 10^14 J e) 2.90 x 10^18 J

c) 3.45 x 10^-19 J

Consider the reaction: C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l) [Delta H] = -1.37 x 10^3 kJ When a 19.2-g sample of ethyl alcohol (molar mass = 46.07 g/mol) is burned, how much energy is released as heat? a) 0.417 kJ b) 0.571 kJ c) 5.71 x 10^2 kJ d) 2.63 x 10^4 kJ e) 2.40 kJ

c) 5.71 x 10^2 kJ

Which of the following combinations of quantum numbers ("n, l, ml, ms") do not represent permissible solutions of the Schrodinger equation for the electron in the hydrogen atom (i.e., which combination of quantum numbers is not allowed)? a) 9, 8, -4, 1/2 b) 8, 2, 2, 1/2 c) 6, -5, -1, 1/2 d) 6, 5, -5, 1/2 e) All are allowed

c) 6, -5, -1, 1/2

Choose the correct equation for the standard enthalpy of formation of CO(g), where [Delta H Fusion] for CO= -110.5 kJ/mol (gr indicates graphite). a) 2C(gr) + O2(g) -> 2CO(g), [Delta H]= -110.5 kJ b) C(gr) + O(g) -> CO(g), [Delta H]= -110.5 kJ c) C(gr) + 1/2O2(g) -> CO(g), [Delta H]= -110.5 kJ d) C(gr) + CO2(g) -> 2CO(g), [Delta H]= -110.5 kJ e) CO(g) -> C(gr) + O(g), [Delta H]= -110.5 kJ

c) C(gr) + 1/2O2(g) -> CO(g), [Delta H]= -110.5 kJ

Which of the following does not have a standard enthalpy of formation equal to zero at 25 degrees C and 1.0 atm? a) F2(g) b) Al(s) c) H2O(l) d) H2(g) e) They all have a standard enthalpy equal to zero.

c) H2O(l)

Which of the following species is best described by drawing resonance structures? a) PH3 b) NH4 c) O3 d) SO3 e) HCN

c) O3

An element has the electron configuration [Kr] 5s^2 4d^10 5p^2. The element is a(n) _________. a) nonmetal b) transition element c) metal d) lanthanide e) actinide

c) metal

What is the coefficient for water when the following equation is balanced? As (OH)3 (s) + H2SO4 (aq) -> As2 (SO4)3 (aq) +H20 (l) a. 1 b. 2 c. 4 d. 6 e. 12

d) 6

A 5.96-g sample of AgNO3 is reacted with BaCl2 according to the equation 2AgNO3(aq) + BaCl2(aq) -> 2 AgCl(s) + Ba(NO3)2 (aq) to give 4.43 g of AgCl. What is the percent yield of AgCl? a. 62.8 % b. 74.5 % c. 44.1 % d. 88.2 % e. 100%

d) 88.2%

Order the elements S, Cl, and F in terms of increasing atomic radii. a) S, Cl, F b) Cl, F, S c) F, S, Cl d) F, Cl, S e) S, F, Cl

d) F, Cl, S

Which of the following pairs of compounds can be used to illustrate the law of multiple proportions? a) NH4 and NH4Cl b) ZnO2 and ZnCl2 c) H2O and HCl d) NO and NO2 e) CH4 and CO2

d) NO and NO2

Which of the following statements about atomic structure is false? a) An atom is a mostly empty space. b) Almost all of the mass of the atom is concentrated in the nucleus. c) The protons and neutrons in the nucleus are very tightly packed. d) The number of protons and neutrons is always the same in the neutral atom. e) All of the above statements (A-D) are true.

d) The number of protons and neutrons is always the same in the neutral atom.

The oxidation state of iodine in IO3^3 is _____. a. 0 b. +3 c. -3 d. +5 e. -5

d. +5

With the volume of 5.00 M HF will 5.15 g of calcium hydroxide react completely, according to the following reaction? 2HF + Ca(OH)2 -> CaF2 + 2H20 a. 13.9 mL b. 139 mL c. 695 mL d. 27.8 mL e. 36.0 mL

d. 27.8 mL

When sodium chloride and lead (II) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular equation? a. PbCl (s) b. Pb2Cl (s) c. NaNO3 (aq) d. 2NaNO3 (aq) e. 2PbCl2 (s)

d. 2NaNO3 (aq)

How much energy is needed to convert 57.2 grams of ice at 0.00 deg. C to water at 75.0 deg. C? Specific heat (ice) =2.10 j/g deg. C Specific heat (water) = 4.18 j/g deg. C Heat of fusion = 333 J/g Heat of vaporization = 2258 J/g a. 17.9 kj b. 2.05 kj c. 28.1 kj d. 37.0 kj e. 147 kj

d. 37.0 kj

A gaseous mixture containing 1.5 mol Ar and 3.5 mol CO2 has a total pressure of 6.0 atm. What is the partial pressure of CO2? a. 1.8 atm b. 1.1 atm c. 14 atm d. 4.2 atm e. 6.0 atm

d. 4.2 atm

The partial pressures of CH4, N2 and O2 in a sample of gas were found to be 163 mmHg, 475 mmHg and 551 mmHg, respectively. Calculate the mole fraction of oxygen. a. 19.7 b. 0.399 c. 0.463 d. 0.725 e. 0.359

c. 0.463

How many grams of potassium are in 15.0 g of K2CrO7? a. 2.42 g b. 0.767 g c. 4.84 g d. 78.2 g e. 30.0 g

c. 4.84 g

A 17.1 g sample of HF is dissolved in water to give 2.0 x 10^2 mL of solution. The concentration of the solution is: a. 0.85 M b. 0.17 M c. 0.09 M d. 4.3 M e. 8.6 M

d. 4.3 M

Zinc metal is added to hydrochloric acid to generate hydrogen gas, which is collected over a liquid whose vapor pressure is the same as pure water at 20.0 deg. C (18 torr). The volume of the gas mixture is 1.7 L, and its total pressure is 0.810 atm. Determine the partial pressure of the hydrogen gas in the mixture. a. 562 torr b. 580 torr c. 598 torr d. 616 torr e. 634 torr

c. 598 torr

A 0.4774-g sample of a compound known to contain only carbon, hydrogen, and oxygen was burned in oxygen to yield 0.8871 g of CO2 and 0.1816 g H20. What is the empirical formula of the compound? a. CHO b. C2H2O c. C3H3O2 d. C6H3O2 e. C3H6O2

c. C3H3O2

In the reaction 2Ca (s) + O2 (g) -> 2CaO(s), which species of oxidized? a. O2 b. O2- c. Ca d. Ca^2+ e. None of these

c. Ca

Aqueous solutions of sodium sulfide and copper (II) chloride are mixed together. Which statement is correct? a. Both NaCl and CuS precipitate from solution b. No reaction will occur c. CuS will precipitate from solution d. NaCl will precipitate from solution e. A gas is released

c. CuS will precipitate from solution

On a relative basis, the weaker the intermolecular forces in a substance: a. The greater its heat of vaporization b. The more it deivates from ideal gas behavior c. The greater its vapor pressure at a particular temperature d. The higher its melting point e. None of these

c. The greater its vapor pressure at a particular temperature

In which case is the bond polarity incorrect? a) +H-F- b) +K-O- c) +Mg-H- d) +Cl-I- e) +Si-S-

d) +Cl-I-

What is the specific heat capacity of a metal if it requires 177.5 J to change the temperature of 15.0 g of the metal from 25.00 degrees C to 34.00 degrees C? a) 0.761 J/g degrees C b) 11.8 J/g degrees C c) 19.7 J/g degrees C d) 1.31 J/g degrees C e) 313 J/g degrees C

d) 1.31 J/g degrees C

In the Lewis structure for SF6, the central sulfur atom shares _______ electrons. a) 4 b) 8 c) 10 d) 12 e) None of the above, because SF6 is an ionic compound.

d) 12

Nitric oxide, NO, is made from the oxidation of NH3, and the reaction is represented by the equation: 4NH3 + 5O2 -> 4NO + 6H20 What mass of O2 would be required to react completely with 7.76 g of NH3? a. 5.16 g O2 b. 11.7 g O2 c. 9.11 g O2 d. 18.2 g O2 e. 14.6 g O2

d) 18.2 g O2

The complete electron configuration of iodine is __________. a) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5d^10 5p^5 b) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4d^10 4p^5 c) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 4p^6 5s^2 4d^10 5d^10 5p^5 d) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5 e) None of these

d) 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^5

In the Lewis structure for ICl2-, how many lone pairs of electrons are around the central iodine atom? a) 0 b) 1 c) 2 d) 3

d) 3

Consider the following reaction: CH4 (g) + 4CL2 (g) -> CCl4 (g) +4HCL (g) What mass of CCl4 is formed by the reaction of 4.80 g of methane with an excess of chlorine? a. 11.5 g b. 0.50 g c. 738 g d. 46.0 g e. None of these

d) 46.0 g

Hydrogen bonding is a type of London Dispersion force True False

False

Methane (CH4) exhibits stronger hydrogen bond interactions than ammonia (NH3). True False

False

Combustion of coal releases sulfur dioxide into the atmosphere. The following process converts this gas into sulfuric acid, a component of acid rain. 2SO2 (g) + O2(g) -> 2SO3(g) SO3(g) H2O (l) -> H2SO4 (aq) If each ton of coal produces 1.30 x 10^4 L of sulfur dioxide (measure at STP), what mass of sulfuric acid can result from combustion of each ton of coal? (1 ton = 1000kg) a. 2.85 x 10^1 kg H2SO4 b. 2.86 x 10^4 kg H2SO4 c. 5.69 x 10^7 kg H2SO4 d. 5.69 x 10^1 kg H2SO4 e. 1.14 x 10^2 kg H2SO4

d. 5.69 x 10^1 kg H2SO4

Which of the species below would you expect to show the least hydrogen bonding? a. NH3 b. H2O c. HF d. CH4 e. All show equal hydrogen bonding

d. CH4

Which of the following would you expect to have the highest boiling point? a. F2 b. Cl2 c. Br2 d. I2 e. All of the above have the same boiling point

d. I2

Which of the following atomic symbols is incorrect? a) 14/6 C b) 37/17 Cl c) 32/15 P d) 39/19 K e) 14/8 N

e) 14/8 N

Which of the following could not be a valid "ml" quantum number for a 4d orbital? a) 2 b) 0 c) -1 d) 1 e) 4

e) 4

Consider the reaction: H2(g) + 1/2 O2(g) -> H2O(l) [Delta H] = -286 kJ Which of the following is true? a) The reaction is exothermic. b) The reaction is endothermic. c) The enthalpy of the products is less than that of the reactants. d) Heat is absorbed by the system. e) Both A and C are true.

e) Both A and C are true.

In which pair do both compounds exhibit predominantly ionic bonding? a) PCl3 and HF b) Na2SO3 and CH4 c) Kl and O3 d) BaF2 and H2O e) CsCl and MgO

e) CsCl and MgO

When 20.0 g of C2H6 and 60.0 g O2 react to form CO2 and H2O, how many grams of water are formed? a. 14.5 g b. 18.0 g c. 58.0 g d. 20.0 g e. None of these

e) None of these

Rutherford's experiment was important because it showed that: a) radioactive elements give off alpha particles. b) gold foil can be made to be only a few atoms thick. c) a zinc sulfide screen scintillates when struck by a charged particle. d) the mass of the atom is uniformly distributed throughout the atom. e) an atom is mostly empty space.

e) an atom is mostly empty space.

The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species? a. 2Br^- (aq) b. PO4^3- (aq) c. 2Ca3(PO4)2 (s) d. 6NaBr(aq) e. 3Ca^2+(aq)

e. 3Ca^2+(aq)

A sample of gas is in a 50.0 mL container at a pressure of 645 torr and a temperature of 25 deg. C. The entire sample is heated to a temperature of 35 deg. C and transferred to a new container whose volume is 77.9 mL. The pressure of the gas in the second container is about: a. 580 torr b. 401 torr c. 1.04 x 10^3 torr d. 155 torr e. 428 torr

e. 428 torr

An oxide of iron has the formula Fe3O4. What mass percent of iron does it contain? a. 0.72% b. 28% c. 30% d. 70% e. 72%

e. 72%

Four identical 1.0 L flasks contain the gases He, CL2, CH4, and NH3 , each at 0 deg C and 1 atm pressure. Which gas sample has the greatest number of molecules? a. He b. Cl2 c. CH4 d. NH3 e. All gases have the same greatest number of molecules

e. All gases have the same greatest number of molecules

Which of the following salts is insoluble in water? a. Na2S b. K2CO3 c. Pb(NO3)2 d. CaCl2 e. All of these are soluble in water

e. All of these are soluble in water

In the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are ______. a. NaSO4 + H2O b. NaSO3 + 2H2O c. 2NaSO4 + H2O d. Na2S + 2H2O e. Na2SO4 + 2H2O

e. Na2SO4 + 2H2O