general chemistry

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?

a. 0.55 g

b. 0.45 g

c. 1.1 g

d. 0.46 g

e. 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) 

®

 As4O6(s)?

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