1) What Is the Empirical Formula of a Compound That Contains 27.0% S, 13.4% O, and 59.6%

AP Exam review-2013

Name:______

Complete 6 of 1-12

1) What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?

A) SOCl2

B) SOCl

C)

D)

E)

2) Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced of and of. What is the empirical formula of the compound?

A)

B)

C)

D)

E)

3) What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water?

A) 0.204

B) 0.0162

C) 0.0485

D) 0.219

E) 0.102

4) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:

In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of produced 3.5 g of. The % yield of the reaction is ______.

A) 47

B) 37

C) 74

D) 66

E) 26

5) Which of the following are weak electrolytes?

HCl

KCl

A) HCl , ,, KCl

B) , KCl

C) ,

D) HCl , , KCl

E) HCl , KCl

6) The net ionic equation for the reaction between aqueous solutions of HF and KOH is ______.

A)

B)

C)

D)

E)

7) Which hydroxides are strong bases?

KOH

NaOH

A)

B)

C) KOH, NaOH

D)

E) None of these is a strong base.

8) A neutralization reaction between an acid and a metal hydroxide produces ______.

A) hydrogen gas

B) water and a salt

C) oxygen gas

D) sodium hydroxide

E) ammonia

9) Based on the equations below, which metal is the most active?

A) N

B) Ag

C) Cu

D) Pb

E) Ni

10) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid in a solid given that a 0.7984 g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

A) 97.78

B) 48.89

C) 28.59

D) 1.086

E) 22.83

11) A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ______.

A) 1.02

B) 0.114

C) 0.454

D) 0.227

E) 0.113

12) When aqueous solutions of ______are mixed, a precipitate forms.

A) NaI and KBr

B)

C)

D)

E)

Complete 5 of 13-22

13) The ΔE of a system that releases 12.4 J of heat and does 4.2 J of work on the surroundings is ______J.

A) -16.6

B) 12.4

C) 4.2

D) 16.6

E) -8.2

14) The value of for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 25.0 g of with water is ______kJ.

A) 80.8

B) 40.4

C) 67.5

D) 20.2

E) -126

15) The molar heat capacity of a compound with the formula is 88.0 J/mol-K. The specific heat of this substance is ______J/g-K.

A) 88.0

B) 4.89

C) 1.13

D)

E) -88.0

16) A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2 °C to 30.5 °C. Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is ______g.

A) 1.5

B) 72

C) 65

D) 8.1

E) 6.6

17) The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of of lead from 22 °C to 37 °C?

A) 2.0

B) -0.13

C)

D) 0.13

E) 29

18) The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 13.9-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0 °C to ______°C. Assume that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.

A) 35.2 °C

B) 24.0 °C

C) 37.0 °C

D) 37.8 °C

E) 40.2 °C

19) The value of for the following reaction is -3351 kJ:

The value of for is ______kJ.

A) -3351

B) -16.43

C) -32.86

D) -1676

E) +3351

20) Given the data in the table below, for the reaction

is ______kJ.

A) -150

B) -1172

C) -1540

D) -1892

E) The of is needed for the calculation.

21) When a system ______, ΔE is always negative.

A) gives off heat and does work

B) absorbs heat and has work done on it

C) gives off heat and has work done on it

D) none of the above is always negative.

E) absorbs heat and does work

22) A ______ΔH corresponds to an ______process.

A) negative, exothermic

B) negative, endothermic

C) positive, exothermic

D) zero, exothermic

E) zero, endothermic

Complete 3 of 23-29

23) Electromagnetic radiation travels through vacuum at a speed of ______m/s.

A) 125

B)

C) 10,000

D) 186,000

E) It depends on wavelength.

24) What is the wavelength of light (nm) that has a frequency of?

A)

B)

C)

D) 932

E) 649

25) The wavelength of a photon that has an energy of is ______m.

A)

B)

C)

D)

E)

26) A mole of yellow photons of wavelength 527 nm has ______kJ of energy.

A) 227

B) 165

C)

D)

E)

27) Of the following, ______radiation has the longest wavelength and ______radiation has the greatest energy.

gamma ultraviolet visible

A) visible, gamma

B) visible, ultraviolet

C) gamma, gamma

D) ultraviolet, gamma

E) gamma, visible

28) The n = 2 to n = 6 transition in the Bohr hydrogen atom corresponds to the ______of a photon with a wavelength of ______nm.

A) emission, 410

B) absorption, 660

C) absorption, 410

D) emission, 94

E) emission, 390

29) What is the de Broglie wavelength (m) of a 25 g object moving at a speed of 5.0 m/s?

A)

B)

C)

D)

E)

Complete 4 of 30-38

30) The azimuthal quantum number is 3 in ______orbitals.

A) a

B) d

C) f

D) p

E) s

31) There are ______unpaired electrons in a ground state phosphorus atom.

A) 4

B) 3

C) 2

D) 1

E) 0

32) Which is the correct ground-state electron configuration for silver?

A)

B)

C)

D)

E)

33) The ______have the greatest electron affinities.

A) alkaline earth metals

B) alkali metals

C) chalcogens

D) transition metals

E) halogens

34) In general, as you go across a period in the periodic table from left to right:

(1) the atomic radius ______;

(2) the electron affinity becomes ______negative; and

(3) the first ionization energy ______.

A) decreases, decreasingly, increases

B) increases, increasingly, decreases

C) increases, increasingly, increases

D) decreases, increasingly, increases

E) decreases, increasingly, decreases

35) For a given arrangement of ions, the lattice energy increases as ionic radius ______and as ionic charge ______.

A) increases, decreases

B) decreases, increases

C) increases, increases

D) decreases, decreases

E) This cannot be predicted.

36) What is the electron configuration for the ion?

A)

B)

C)

D)

E)

37) The formal charge on nitrogen in is ______.

A) 0

B) -1

C) -2

D) +2

E) +1

38) Using the table of average bond energies below, the for the reaction is ______kJ.

Bond: C≡C C-C H-I C-I C-H

D (kJ/mol): 839 348 299 240 413

A) +160

B) +217

C) -217

D) -63

E) +63

Complete 2 of 39-42

39) The bond angle in the on is approximately ______.

A) 180 °

B) 109.5 °

C) 90 °

D) 120 °

E) 60 °

40) has "T-shaped" geometry. There are ______non-bonding domains in this molecule.

A) 1

B) 2

C) 3

D) 4

E) 0

41) Of the following molecules, only ______is polar.

A)

B)

C)

D)

E)

42) Of the following, the central atom is hybridized only in ______.

A)

B)

C)

D)

E)

Complete 5 of 43-53

43) A closed-end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 12.2 cm. Atmospheric pressure was 783 mm Hg. The pressure of the argon in the container was ______mm Hg.

A) 882

B) 661

C) 771

D) 795

E) 122

44) A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was ______atm.

A) 4.00

B) 2.00

C) 16.0

D) 8.00

E) 1.00

45) If 3.21 mol of a gas occupies 56.2 L at 44 °C and 793 torr, 5.29 mol of this gas occupies ______L under these conditions.

A) 92.6

B) 61.7

C) 30.9

D) 14.7

E) 478

46) If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy ______L at STP.

A) 3.92

B) 5.08

C) 25.5

D) 12.9

E) 50.8

47) A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mm Hg. The flask is opened and more gas is added to the flask. The new pressure is 795 mm Hg and the temperature is now 26 °C. There are now ______mol of gas in the flask.

A) 0.28

B) 1.6

C) 2.1

D) 2.9

E) 3.5

48) The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ______g/L.

A) 3.86

B) 0.194

C) 0.432

D) 0.719

E)

49) The volume of hydrogen gas at 38.0 °C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is ______L.

A) 0.592

B)

C)

D) 2.84

E) 1.68

50) A vessel contained, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ______torr.

A) 42.4

B) 239

C) 521

D) 19.4

E) 760

51) A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ______atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C.

A) 2.6

B) 3.7

C) 1.0

D) 9.2

E) 24

52) A sample of gas (2.0 mmol) effused through a pinhole in 5.5 s. It will take ______s for the same amount of to effuse under the same conditions.

A) 4.2

B) 5.5

C) 3.1

D) 7.3

E) 9.6

53) Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.00 mol of neon gas at 100 °C is ______atm. (,)

A) 0.730

B) 1.37

C) 1.21

D) 1.00

E) 0.367

Complete 2 of 54-58

54) The substance with the largest heat of vaporization is ______.

A)

B)

C)

D)

E)

55) The heat of fusion of water is 6.01 kJ/mol. The heat capacity of liquid water is . The conversion of of ice at 0.00 °C to liquid water at 22.0 °C requires ______kJ of heat.

A) 21.3

B)

C) 17.2

D) 0.469

E) Insufficient data are given.

56) The phase diagram of a substance is shown above. The area labeled ______indicates the gas phase for the substance.

A) w

B) x

C) y

D) z

E) y and z

57) According to the phase diagram shown above, the normal boiling point of this substance is ______°C.

A) -3

B) 10

C) 29

D) 38

E) 0

58) molecules are held together by ______.

A) ion-ion interactions

B) hydrogen bonding

C) ion-dipole interactions

D) dipole-dipole interactions

E) dispersion forces

Complete 4 of 59-65

59) The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is ______M.

A)

B)

C)

D)

E) 0.80

60) The solubility of monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution at 20 °C that is 4.22 M in monohydrate is best described as a(n) ______solution. The formula weight of monohydrate is 168.97 g/mol.

A) hydrated

B) solvated

C) supersaturated

D) unsaturated

E) saturated

61) The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is ______molal.

A) 0.0167

B) 0.0207

C)

D) 0.0186

E) 2.46

62) A solution is prepared by dissolving 15.0 g of in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The mole fraction of in the solution is ______.

A) 0.0640

B) 0.0597

C) 0.940

D) 0.922

E) 16.8

63) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a vapor pressure of ______atm.

A) 0.413

B) 0.498

C) 0.790

D) 0.367

E) 0.0918

64) What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of (formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for water is 1.86 °C/m.

A) -3.34

B) -1.11

C) 3.34

D) 1.11

E) 0.00

65) A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33 °C. Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is ______g/mol.

A) 69.0

B) 333

C) 619

D) 161

E) 62.1