general chemistry-bomb calorimeter

1. A 5.00 g sample of a brownie with nuts is burned in a bomb calorimeter containing 2025 g of water. The temperature of the water increases from 23.50C to 33.47C. How much heat, in joules, did the brownie release when it burned? (Cwater = 4.184 J/gC)

1.99  105 J
8.45  104 J

2.80  105 J
7.00  102 J

4.92  102 J

2. Which of the following compounds is a ketone?




3. Iron metal reacts with hydrochloric acid as follows:

2Fe(s) + 6HCl(aq)  2FeCl3(aq) + 3H2(g)

If 22.4 g of iron react with excess HCl, and 59.4 g of FeCl3 are collected, what is the percent yield of the reaction?

A) 65.0% B) 109% C) 91.4% D) 73.0% E) not enough information given

4. In the process of obtaining lead from PbS, or galena, the galena is “roasted” (heated in the presence of oxygen), so that the following reaction occurs:

2PbS(s) + 3O2(g)  2PbO(s) + 2SO2(g)

If 50.0 g of PbS reacts with 25.0 g of oxygen, how many grams of PbO will be formed?

A) 116 g B) 46.6 g C) 163 g D) 69.9 g E) 93.2 g

5. Phosphorus trichloride can be made by the reaction:

P4(s) + 6Cl2(g)  4PCl3(l)

What is the maximum amount of phosphorus trichloride that can be formed if 10 molecules of P4 react with 36 molecules of chlorine?

4 molecules
24 molecules

6 molecules
46 molecules

12 molecules

6. Consider the reaction:

Zn(s) + NO3(aq)  NH3(aq) + Zn(OH)42(aq)

When this equation is balanced in basic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

A) 3, 3 B) 2, 1 C) 6, 8 D) 5, 6 E) 2, 3

7. If the pH of a blood sample is 7.60, what is the H3O+ concentration in the blood?

A) 7.6 M B) 2.5  108 M C) 2.5  107 M D) 2.5  109 M E) 6.4 M

8. If CH3NH2 is added to water, what other compound could also be added in order to make a buffered solution?


none of these is correct


9. What is the pH of a 0.015 M NaOH solution?

A) 0.015 B) 1.82 C) 7.00 D) 12.18 E) –1.82

10. Ethane, C2H6, can be formed by reacting acetylene, C2H2, with hydrogen gas as follows:

C2H2(g) + H2(g)  C2H6(g) Exothermic

What change will be observed if the temperature of the reaction mixture at equilibrium were increased?

The concentration of C2H6 will increase.

The concentration of both C2H2 and H2 will increase.

The concentration of both C2H2 and H2 will decrease.

The concentration of H2 only will decrease.

There will be no change in the equilibrium concentrations.

11. Consider the following reaction:

N2O4(g)  2NO2(g) q = +58.2 kJ

What will cause an increase in the concentration of NO2 at equilibrium?

The NO2 concentration can never change because the reaction is at equilibrium.

an increase in temperature

an increase in pressure

a decrease in volume

adding a catalyst

12. Which of the following compounds is an aldehyde?




13. Which one of the following reactions is an example of an oxidation-reduction reaction?

BaO(s) + CO2(g)  BaCO3(s)

H2(g) + F2(g)  2HF(g)

CaCO3(s)  CaO(s) + CO2(g)

HCl(aq) + NaOH(aq)  NaCl(aq) + H2O(l)

Ba2+(aq) + SO42–(aq)  BaSO4(s)

14. Consider the following reaction:

Mn(s) + CuSO4(aq)  MnSO4(aq) + Cu(s)

Which of the following statements regarding this reaction is correct?

Manganese is neither oxidized nor reduced.

The sulfate ion is oxidized.

Copper is the reducing agent.

Manganese is the oxidizing agent.

Each copper gains two electrons.

15. In which of the following choices is the oxidation number incorrect?

Cr3+(aq); oxidation number = 3+
K+(aq); oxidation number = 1+

Cl(aq); oxidation number = 1–
Ag(s); oxidation number = 1+

F2(g); oxidation number = 0

16. What is the oxidation number of boron in sodium tetraborate, Na2B4O7?

A) +12 B) –3 C) +14 D) +3 E) +4

17. Consider the reaction:

H3AsO3(aq) + BiO3(aq)  H3AsO4(aq) + Bi(s)

When this equation is balanced in acidic solution, the coefficient for water will be__________, and the number of electrons transferred will be __________.

A) 2, 6 B) 2, 1 C) 1, 10 D) 1, 2 E) 2, 3

18. Given that 4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g), if 82.0 g of NH3 react with sufficient oxygen, how many grams of NO will be formed?

A) 145 g B) 5.80  102 g C) 46.5 g D) 186 g E) 11.6 g

19. Balance the following skeletal equation:

Ba(NO3)2(aq) + K2SO4(aq)  BaSO4(s) + KNO3(aq)

Ba(NO3)2(aq) + K2SO4(aq)  BaSO4(s) + KNO3(aq)

2Ba(NO3)2(aq) + K2SO4(aq)  2BaSO4(s) + KNO3(aq)

2Ba(NO3)2(aq) + 2K2SO4(aq)  2BaSO4(s) + 2KNO3(aq)

2Ba(NO3)2(aq) + 2K2SO4(aq)  2BaSO4(s) + 3KNO3(aq)

Ba(NO3)2(aq) + K2SO4(aq)  BaSO4(s) + 2KNO3(aq)

20. The condensed structural formula for the molecule shown in the figure is__________.




21. Which of the following is the molecular formula for the molecule represented in the figure?

A) C6H6 B) C6H8 C) C6H10 D) C6H12 E) C6H16

22. To which class of compounds does the molecule shown in the figure belong?

A) ketone B) aldehyde C) alcohol D) ester E) carboxylic acid

23. The position of equilibrium would not be appreciably affected by changes in the volume of the container for

NiO(s) + CO(g)  Ni(s) + CO2(g)
2CO(g) + O2(g)  2CO2(g)

BaCO3(s)  BaO(s) + CO2(g)
PCl5(s)  PCl3(g) + Cl2(g)

2H2O(g)  2H2(g) + O2(g)

24. Write the equilibrium constant expression for the reaction:

Pb2+(aq) + 2Cl(aq)  PbCl2(s)

















Keq = [Pb2+][ Cl]2















25. What is the balanced chemical equation that corresponds to the equilibrium constant expression (assuming a homogeneous equilibrium in the gas state)?







A + B2  C + D
C + D  A + B2

A + 2B  C + D
C + D  A + 2B

C + D  A + B

26. The graph shows the change in concentration of reactant and product as a reaction proceeds. At what point is equilibrium first reached?

A) I B) II C) III D) IV E) V

27. According to collision theory, the increase in the rate constant with increasing temperature is due mostly to the fact that

the activation energy decreases with increasing temperature.

the fraction of the collisions having sufficient energy to react increases with increasing temperature.

the pressure of the reactants increases with increasing temperature.

the heat change for most reactions is negative.

the fraction of the collisions that have the proper orientation for reaction increases with increasing temperature.

28. Silver nitrate, AgNO3, can be used to test for the presence of chloride ions in solution, because it readily forms a precipitate of AgCl. What volume of 2.0 M AgNO3 will be required to react with 50.0 mL of a 0.10 M HCl solution?

AgNO3(aq) + HCl(aq)  AgCl(s) + HNO3(aq)

A) 0.25 mL B) 25 mL C) 5.0  101 mL D) 2.5  102 mL E) 2.5 mL

29. What is the percent-by-mass concentration of antifreeze (ethylene glycol, C2H6O2) in an aqueous solution that contains 420.0 g of ethylene glycol in 1.00 L of solution. The density of the solution is 1.05 g/mL.

A) 2.50% B) 42.1% C) 40.0% D) 44.1% E) 60.0%

30. What mass of sodium nitrate is dissolved in 455 g of a solution that is 15.0% by mass NaNO3?

A) 68.3 g B) 30.3 g C) 4.40  102 g D) 3.03  103 g E) 15.0 g

31. Rank the following substances in order of increasing boiling point: F2, Ne, He, Cl2

F2 < Ne < He < Cl2 D) He < Ne < F2 < Cl2

F2 < He < Ne < Cl2 E) Cl2 < F2 < Ne < He

F2 < Cl2 < He < Ne

32. Which of the following substances can participate in hydrogen bonding?

A) CH4 B) HF C) CH3COCH3 D) SiH4 E) all of these choices are correct

33. Which choice correctly lists the intermolecular forces present in CH3NH2?

London forces only

dipole-dipole forces only

London forces, dipole-dipole forces, and hydrogen bonding

dipole-dipole forces and hydrogen bonding

hydrogen bonding only

34. The forces that hold CO2 together in the solid state are:

ionic bonds.

dipole-dipole forces.

London dispersion forces only.

covalent bonds.

attractions between nuclei and delocalized valence electrons.

35. Calculate the molar mass of a gas that has a density of 1.428 g/L at STP.

not enough information
32.01 g/mol

14.28 g/mol
0.7002 g/mol

0.4460 g/mol

36. A sample of H2 is collected over water at 22C. If the total pressure of the sample is 744 torr, what is the partial pressure of the H2? The vapor pressure of water at 22C is 19.8 torr.

A) 37.6 torr B) 0.979 atm C) 764 torr D) 724 torr E) 744 torr

37. If a 7.00 L container is filled with O2 to a pressure of 995 torr at 33.0C, calculate the mass of the oxygen in the container.

A) 11.7 g B) 0.365 g C) 277 g D) 2.57  103 g E) 0.0854 g

38. Which of the following gases will have a density of 2.104 g/L at 303 K and 1.31 atm?

A) He B) Ne C) Ar D) Kr E) Xe

39. Given a fixed amount of gas held at constant pressure, calculate the volume it would occupy if a 3.50 L sample were cooled from 90.0oC to 30.0oC.

A) 1.17 L B) 10.5 L C) 4.19 L D) 2.92 L E) 1.75 L

40. What volume of H2 would be collected at 21.5oC and a pressure of 695 torr if 5.25 g of zinc react according to the equation:

Zn(s) + 2HCl(aq)  ZnCl2(aq) + H2(g)

A) 1.06 L B) 4.25 L C) 1.80 L D) 2.12 L E) 5.49 L

41. Arrange the following bonds in order of increasing polarity: Cl-S, Cl-P, Cl-Si, Cl-Cl

Cl-S < Cl-P < Cl-Si < Cl-Cl D) Cl-Cl < Cl-S < Cl-P < Cl-Si

Cl-S < Cl-Si < Cl-P < Cl-Cl E) Cl-Cl < Cl-P < Cl-Si < Cl-S

Cl-Si < Cl-S < Cl-Cl < Cl-P

42. Predict the molecular shape and give the approximate bond angles of the SiH4 molecule.

linear, 180
trigonal pyramidal, 109.5

trigonal planar, 120
bent, 120

tetrahedral, 109.5

43. Which of the following molecules is polar?

A) BF3 B) CH4 C) CS2 D) PCl3 E) BeCl2

44. The electron configuration 1s22s22p6 applies to all of the following species except:

A) Ne B) F C) O2 D) Na+ E) Ca2+

45. Rank the following elements in order of increasing atomic size: Al, Ba, O, C

Al < Ba < O < C D) O < C < Al < Ba

Ba < Al < O < C E) C < O < Al < Ba

Ba < Al < C < O

46. Some elements have electron configurations that deviate from normal electron filling rules. Which element has the ground-state electron configuration [Ar]4s13d10?

A) Ni B) Ag C) Cd D) Sn E) Cu

47. The element that has four completely filled s sublevels, and three d electrons is:

A) V B) Cr C) Nb D) Ti E) Sc






1. What pressure will be exerted by 8.00 grams of helium in a 5000. L flask at 250C?

a. 39.1 atm

b. 0.00978 atm

c. 48.9 atm

d. 9.79 atn

e. None of the above

2. For which substance is hydrogen bonding important?

a. sodium hydride

b. hydrogen peroxide

c. methane

d. nickel (II) hydride

e. butane (C4H10)

3. Which of the following cannot function as a Bronsted-Lowry base?

a. OH¯

b. NH3

c. CH3NH2

d. CH4

e. I¯

4. Sodium sulfate is allowed to react with an aqueous solution of barium chloride. How many grams of sodium sulfate are required to produce 0.45 g of sodium chloride?

a. 0.55 g
b. 0.45 g
c. 1.1 g

d. 0.46 g
e. none of the above

5. How many p orbitals can exist in a single subshell?

a. 1

b. 2

c. 3

d. 6

e. not enough information

6. How many electrons, protons and neutrons, respectively, are in 60 Ni 2+ ?

a. 26, 28, 32

b. 28, 28, 32

c. 32, 28, 26

d. 26, 28, 28

e. 32, 28, 26

7. A balloon is inflated to 344 mL at a temperature of 55°C. The volume of the balloon decreases to 214 mL when placed in a refrigerator. What is the temperature of the refrigerator?

a. 88°C

b. 88 K

c. 204 K

d. 34°C

e. 55°C

8. What is the percent composition of oxygen in barium chlorate?

a. 31.6%

b. 15.8%

c. 5.26%

d. 21.7%

e. 19.2%

9. Which of the following has the lowest boiling point, based on structure, polarity, molar mass and bonding?

a. methane

b. carbon tetrafluoride

c. carbon tetrachloride

d. carbon tetrabromide

e. carbon tetraiodide

10. A detergent labeled “mild” has a pH of 7.80. What is the hydroxide ion concentration in this detergent?

a. 6.31 x 10-7 M

b. 1.6 x 10-8 M

c. 1.58 x 10-8 M

d. 4.9 x 10-7 M

e. 6.3 x 10-7 M

11. A 25.00 mL sample of calcium hydroxide was titrated with 12.76 mL of 0.0199 M hydrochloric acid. What is the concentration of the base?

a. 5.08 x 10-2 M

b. 1.02 x 10-2 M

c. 1.02 x 10-3 M

d. 6.88 x 10-3 M

e. 5.08 x 10-3 M

12. Which of the following orbital diagrams represent the valence electrons for oxygen?

a. (( (( ((

b. (( (( (( (_ (_

c. (( (( (_ (_

d. (( (( (_ (_ __

e. none of the above

13. For the complete combustion of 1-pentene (C5H10), how many liters of carbon dioxide gas will be formed by the reaction of 400 liters of oxygen when reacted with excess 1-pentene? (Assume that the reaction is at constant temperature and pressure.)

a. 400 L

b. 367 L

c. 600 L

d. 267 L

e. 825 L

14. Which has the highest melting point?

a. Fluorine

b. BH3

c. Chlorine

d. Potassium iodide

e. Potassium chloride

15. Zinc metal was reacted with hydrochloric acid to produce 48.1 g of gas, which was collected by displacement of water at the temperature of 22.0°C and a barometric pressure of 748 torr. The vapor pressure of water at 22.0°C is 20 mm Hg. What would the volume of this gas sample be at STP?

a. 43.8 mL

b. 42.6 mL

c. 41.9 mL

d. 50.1 mL

e. 45.0 mL

16. How much heat (in Joules) is required to raise the temperature of 50.0 g of brass from 20.0°C to 65.0°C? The specific heat of brass is 0.385 J/g°C.

a. 385 J

b. 1250 J

c. 5840 J

d. 436 J

e. 866 J

17. What volume of a 0.1000 M hydroiodic acid solution is needed to neutralize 25.0 mL of a

0.350 M barium hydroxide solution?

a. 175 mL

b. 140 mL

c. 140. mL

d. 75 mL

e. None of the above

18. What volume would 9.50 g of nitrogen gas occupy at 22.0°C and a pressure of 1.34 atm?

a. 0.306 L

b. 6.13 L

c. 53.2 L

d. 26.6 L

e. 12.2 L

19. A cylindrical tank of compressed air has a pressure of 145 atm at 25oC. The maximum pressure the tank can hold is 500. atm. If a fire breaks out in the lab and the cylinder reaches 1000oC, what is its new pressure and status?

a. 5800 atm: BOOM!

b. 33.9 atm: OK.

c. 619 atm: Run Away!

d. 500 atm: On the brink!

e. 172 atm: Whew

20. Which of the following are a buffer pair in water?

a. hydrochloric acid and sodium chloride

b. potassium hydroxide and sodium hydroxide

c. potassium hydroxide and potassium chloride

d. ammonia and ammonium chloride

e. ammonia and water

21. What is the percent by weight of sodium in sodium sulfate?

a. 16.2 %

b. 46.0 %

c. 31.4 %

d. 32.4 %

e. none of the above

22. How much methane is required to produce 55.0 g of carbon dioxide, when burned in excess oxygen?

a. 55.0 g
b. 1.25 g
c. 151 g

d. 12.5 g

e. 20.0 g

23. What is the molarity of a hydrochloric acid solution, if 15.78 mL of acid is needed to completely neutralize 10.00 mL of a 0.2000 M sodium hydroxide solution?

a. 7.890 M

b. 0.1267 M

c. 0.3156 M

d. 0.03156 M

e. 31.56M

24. How many mL of 1.80 M hydrochloric acid are required to completely react with 30.0 grams of calcium hydroxide?

a. 450. mL

b. 165 mL

c. 575 mL

d. 225 mL

e. none of the above

25. A gas has a volume of 230. mL and a pressure of 560 torr. What must the pressure be in order for the gas to have a volume of 345 mL at the same temperature?

a. 1.50 torr

b. 103 torr

c. 142 torr

d. 840 torr

e. none of the above

26. Predict the products from the following reaction: Ba(OH)2(aq) + H2SO4(aq) →

a. Ba2(SO4)3(aq) + 2H2O(l)

b. BaSO4(s) + 2H2O(l)

c. BaSO4(aq) + 2H2O(l)

d. BaSO4(aq) + H2(g) + O2(g)

e. No reaction

27.  Which is the correct name for CuSO4?

a. copper sulfate

b. copper (II) sulfite

c. copper (II) sulfate

d. copper (I) sulfate

e. curium (II) sulfite

28.  During a certain titration, it took 35.90 mL of 0.125 M potassium hydroxide to exactly neutralize 25.00 mL of sulfuric acid. Determine the molarity of the acid given the balanced neutralization reaction:
H2SO4(aq) + 2KOH(aq) → 2H2O(l) + K2SO4(aq)

A)    0.0898 M

B)     0.359 M

C)    0.00224 M

D)    0.00448 M

E)     0.179 M

29.  What is the diameter of the coin below?


A)    2.50 cm            B) 2.8 cm         C) 2.5 cm         D) 3 cm            E) 2.1 cm

30.Sodium sulfate is allowed to react with an aqueous solution of barium chloride to produce (you know). How many grams of sodium sulfate are required to produce 0.45 g of salt?

0.55 g

0.45 g

1.1 g

0.46 g

none of the above

31.  What is the answer to the following problem to the correct number of significant figures?

0.025 x 3.60 x 52.13

A)    4.7

B)     4.692

C)    4.70

D)    4.6

E)     4.69

32.  Which of the following correctly describes the Lewis structure of the carbonate ion?

A)    2 single bonds, 1 double bond, 8 lone pairs

B)     3 single bonds, 9 lone pairs

C)    1 single bond, 2 double bonds, 9 lone pairs

D)    3 double bonds, 6 lone pairs

33. What is the hydroxide concentration of a 3.33 x 10-3 M hydrochloric acid solution?

a. 3.00 x 10-12 M

b. 1.52 x 10-12 M

c. 7.00 x 10-7 M

d. 1.00 x 10-7 M

e. None of the above

34. When the pH of a solution is equal to 3.0,

a. [H3O+] < [OH-]

b. [H3O+] > [OH-]

c. [H3O+] + [OH-]

d. [H3O+] = [OH-]

e. [H3O+] / [OH-]

35. Name the following compound: P2Se

A)    diphosphorus selenide

B)     diphosphorus monoselenium

C)    diphosphorus monoselenide

D)    phosphorus selenide

E)     dipotassium monoselenide

36. Zinc reacts with HCl to produce ZnCl2 and hydrogen gas H2: Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g). How many grams of zinc can react with 225 mL of 0.200 M HCl?

A)    1.47 g

B)     3.78 g

C)    1.23 g

D)    0.89 g

E)     4.56 g

37. How many grams of ozone are generated from 3.25 g of fluorine in the reaction:
3F2(g) + 6H2O(l)


2O3(g) + 6HF(aq)?

A)    6.16 g   B)  4.10 g   C)  1.82 g   D)  2.74 g   E)  2.54 g

38. A sample of  phosgene (COCl2) gas exerts a pressure of 325 mm Hg at 50.0 oC. What pressure would it exert in atmospheres at 40.0 oC?

A)    315 atm

B)     0.332 atm

C)    252 atm

D)    0.414 atm

E)     367 atm

39. What volume in mL would 3.25 g of dinitrogen pentoxide occupy at a temperature of 273 K and 760 mm Hg?

A)    0.674 mL

B)     34.5 mL

C)    674 mL

D)    453 mL

E)     0.986 mL

40. How many grams of magnesium cyanide would you need to weigh out in order to prepare 275 mL of a 0.325 M solution?

A)    7.24 g

B)     4.50 g

C)    6.82 g

D)    9.56 g

E)     3.49 g

41. Diamond has a density of 3.52 g/mL. What is the volume in cubic centimeters of a diamond with a mass of 15.10 g?

A)    0.233 cm3

B)     53.2 cm3

C)    4.3 cm3

D)    4.29 cm3

E)     0.897 cm3

42. A solution is considered

a. A undefined entity

b. An element

c. A compound

d. A homogeneous mixture

e. A heterogeneous mixture

43. What is the pH of a solution with [H3O+] = 3.25 x 10-6 M?

A)    5.488

B)     3.78

C)    5.49

D)    4.951

E)     2.74

44. How many grams of tetrarsenic hexoxide are formed when 6.25g of arsenic react with 3.25 g of oxygen in the reaction 4As(s) + 3O2(g)



A)    132 g

B)     8.25 g

C)    33.0 g

D)    13.5 g

E)     34.6 g

45. How many protons, neutrons and electrons are present in the 7+ ion of the isotope of manganese-55?

A)    25 protons, 25 electrons, 30 neutrons

B)     25 protons, 18 electrons, 30 neutrons

C)    18 protons, 25 electrons, 55 neutrons

D)    55 protons, 18 electrons, 30 neutrons

E)     30 protons, 25 electrons, 55 neutrons

46. How many chlorine atoms are there in 3.25 g of carbon tetrachloride?

A)    1.271 x 1022

B)     5.083 x 1022

C)    1.27 x 1022

D)    5.08 x 1022

E)     3.72 x 1022

47. What are the expected products from the following reaction: HNO3(aq) + LiHCO3(aq) →

A)    CO2(g) + LiNO3(aq) + H2O(l)

B)     LiNO3(aq) + H2CO3(aq)

C)    CO2(g) + LiNO3(aq)

D)    CO2(g) + Li2NO3(aq) + H2O(l)

E)     No reaction

48. What kind of reaction is this: Mg(s) + 2HI(aq)


MgI2(s) + H2(g)

A)    single replacement  B)  neutralization   C)  decomposition   D)  double replacement

E) combustion

49. What is the electron configuration for cobalt?

A)    1s22s22p63s23p64s23d7

B)     1s22s22p63s23p64s23d6

C)    1s22s22p63s23p63d7

D)    1s22s22p63s23p64s23d4

E)     1s22s22p63s23p64s13d6

50. Mg metal reacts with HCl to produce hydrogen gas: Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). How many grams of magnesium are needed to prepare 5.00 L of H2 at 735 mm Hg and 18 ºC?

A)    4.91 g

B)     3.67 g

C)    2.90 g

D)    4.32 g

E)     6.49 g


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