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Exam Review

Total questions: 95

Worksheet time: 1hrs 2mins

Name
Class
Date
1.

How much heat is required to change 25.8 g of water from 35°C to 98°C? Specific heat of water is 4.18 J/g °C.

a)

6780 J

b)

4500 J

c)

9000 J

d)

12000 J

2.

What is the term for the transition of a material from a gas to a solid?

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Evaporation

3.

Which states exist at the triple point of a substance?

a)

Solid, liquid, and gas

b)

Solid and liquid only

c)

Liquid and gas only

d)

Solid and gas only

4.

Substance A has a specific heat of 0.25 J/g°C, and substance B has a specific heat of 0.68 J/g°C. If both are initially at 25°C, when heated evenly, which will reach 50°C first?

a)

Substance A

b)

Substance B

c)

Both will reach at the same time

d)

Neither will reach 50°C

5.

How many calories are in a Big Mac? (33g fat, 44g carb and 25g protein)

(a)  

6.

If someone ate a doughnut that contained 500 calories, how many hours would they have to exercise to use those calories if they were burning 125 calories per hour?

a)

4 hours

b)

2 hours

c)

6 hours

d)

8 hours

7.

A student mixed aluminum with hydrochloric acid and the temperature of the surrounding water increased by 25°C. Was the reaction endothermic or exothermic?

(a)  

8.

If a system has a pressure of 2.5 atm and a volume of 1.0 L, what is the new volume if the pressure increases to 7.5 atm?

a)

0.33 L

b)

0.13 L

c)

0.75 L

d)

2.0 L

9.

How many moles are in a 2.5 L container if the pressure is 1.3 atm and the temperature is 298 K?

(a)  

10.

What is the total pressure if a 5.0L container at a temperature of 425K contains 1.3 moles of oxygen and 2.6 moles of nitrogen?

a)

16.4 atm

b)

10.2 atm

c)

22.8 atm

d)

8.7 atm

11.

If the following reaction is at STP, how many liters of CO₂ gas will be produced from 10.0g of CaCO₃ (molar mass=100.g/mole)? CaCO₃(s) → CO₂(g) + CaO(s)

a)

2.24 L

b)

1.12 L

c)

4.48 L

d)

22.4 L

12.

If a balloon has a volume of 3.0 L and contains 0.10 moles of gas. What is the new volume if the amount of gas is increased to 1.0 moles?

a)

30 L

b)

3.3 L

c)

0.30 L

d)

10 L

13.

What is the pressure of an 8.4L system that contains 0.75 moles of gas at 200.0K?

a)

1.5 atm

b)

0.82 atm

c)

2.5 atm

d)

3.1 atm

14.

A container has a pressure of 2.5 atm at 298 K, what is the new pressure if the temperature changes to 58°C?

a)

3.0 atm

b)

2.0 atm

c)

2.7 atm

d)

3.5 atm

15.

Standard temperature is 0.0 K and standard pressure is 1.0 atm?

a)

True

b)

False

16.

Putting a balloon in the freezer causes it to shrink. Why?

4 lines
17.

On a heating curve, what is happening when the temperature remains constant?

a)

A phase change is occurring (melting or boiling).

b)

The substance is cooling down rapidly.

c)

The substance is decomposing into new elements.

d)

The temperature sensor is malfunctioning.

18.

A 10.0 g piece of metal has a specific heat of 0.65 J/g°C. If it is initially at 25°C and has 5000 J of energy added, what is the final temperature?

(a)  

19.

How many significant figures are in 0.0034 cm?

(a)  

20.

How many significant figures are in 34040 cm?

a)

4

b)

3

c)

5

d)

2

21.

72.43 x 23 =

a)

1700

b)

1450.23

c)

1720.50

d)

1600.00

22.

18.42 / 9.21 =

(a)  

23.

0.04378 + 0.52622 =

(a)  

24.

Broken glass should be disposed of by:

a)

Throwing it in the regular trash without protection

b)

Placing in the glass disposal bin.

c)

Flushing it down the toilet

d)

Leaving it on the ground

25.

You are allowed to eat or drink the following in lab:

a)

Water only

b)

Food only

c)

Both food and drinks

d)

Nothing

26.

2430 km = ___ m

a)

2,430,000

b)

243,000

c)

24,300

d)

24,300,000

27.

27842 mm = ____ km

a)

0.027842

b)

0.27842

c)

2.7842

d)

0.0027842

28.

823 lb = _____ kg (2.20 lb = 1.0 kg)

a)

374

b)

410.50

c)

250.00

d)

600.00

29.

What is the density of an object with a mass of 13.75 g and a volume of 8.25 cm³?

a)

1.67 g/cm³

b)

0.60 g/cm³

c)

2.10 g/cm³

d)

1.20 g/cm³

30.

If a measuring device has markings for 1 mL, which of the following would be a correct way to report a measurement?

a)

10 mL

b)

10.0 mL

c)

10.00 mL

31.

If a cube has a volume of 1.25 m³, how many mm³ is it (in scientific notation)?

a)

1.25 x 10^9 mm³

b)

1.25 x 10^6 mm³

c)

1.25 x 10310^3 mm³

d)

1.25 x 10^12 mm³

32.

If a metal has a density of 8.5 g/cm³ and a mass of 17.0 g, what is the volume?

a)

2.0 cm³

b)

0.5 cm³

c)

8.5 cm³

d)

17.0 cm³

33.

1500.0 + 10 =

a)

1510

b)

1501.0

c)

1490.0

d)

1600.0

34.

28.4 x 4.7 =

a)

130

b)

120.5

c)

141.2

d)

100.7

35.

328 cm = ___ inches

a)

129

b)

100.25

c)

150.00

d)

80.50

36.

2.3 moles of Fe contain _______________ atoms.

a)

1.4 x 10^24

b)

6.02x10236.02 x 10^23

c)

3.45 x 10^23

d)

2.76 x 10^24

37.

4.8 x 10^24 atoms of Ag are 4.8x10244.8 x 10^{24} moles.

a)

7.97

b)

0.80

c)

12.04

d)

1.20

38.

Molar mass of N₂O₅ = _______________ g/mole.

a)

108.01

b)

90.02

c)

120.05

d)

142.00

39.

Molar mass of PbCl₂ = _______________ g/mole.

a)

278.1

b)

208.2

c)

236.5

d)

250.0

40.

72 g of H₂O (molar mass = 18 g/mole) = _______________ moles H₂O

a)

4

b)

2

c)

18

d)

36

41.

14 moles of C₆H₁₂O₆ (180 g/mole) = _______________ g C₆H₁₂O₆

a)

2520

b)

1800

c)

1260

d)

3240

42.

The coefficients that balance the following equation are: __Ca(OH)₂ (aq) + ___HCl(aq) → __H₂O(l) + __CaCl₂(aq)

a)

1, 2, 2, 1

b)

2, 1, 1, 2

c)

1, 1, 2, 2

d)

2, 2, 1, 1

43.

2Mg(s) + O2(g) → 2MgO(s) is an example of a ______ reaction.

a)

combination (or synthesis)

b)

decomposition

c)

displacement

d)

redox

44.

In a balanced equation, the terms g, s, and aq stand for _______, _______, and _______.

a)

gas, solid, aqueous

b)

gas, solution, acid

c)

graphite, salt, alkali

d)

gold, sulfur, aqua

45.

Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) is an example of a ________ reaction.

a)

single displacement (or single replacement)

b)

double displacement

c)

decomposition

d)

combination

46.

__________ appear on the left side of a balanced equation.

a)

Reactants

b)

Products

c)

Catalysts

d)

Solvents

47.

__________ appear on the right side of a balanced equation.

a)

Products

b)

Reactants

c)

Catalysts

d)

Coefficients

48.

When the temperature increases, the rate of a reaction increases because __________.

a)

the particles have more energy and collide more frequently/effectively

b)

the particles lose energy and move slower

c)

the concentration of reactants decreases

d)

the reaction becomes independent of temperature

49.

Increasing concentration (increases/decreases) the rate of a reaction. Which is it?

(a)  

50.

Using the equation FeCl3(aq) + 3NaSCN(aq) → Fe(SCN)3 (s) + 3NaCl(aq), (a)   moles of Fe(SCN)3 would be produced from 270 moles of NaSCN?

51.

If you were given 10 moles of H2 and 6 moles of O2, which would be limiting? 2H2(g) + O2(g) → 2H2O(g)

a)

H2

b)

O2

c)

H2O

d)

None of the above

52.

The correct coefficients for balancing the following equation are: __CH4(g) + __O2(g) → __H2O(g) + __CO2(g)

a)

1, 2, 2, 1

b)

2, 1, 2, 1

c)

1, 1, 1, 2

d)

2, 2, 1, 1

53.

The fact that we must have equal mass on both sides of an equation is the law of __________.

a)

conservation of mass

b)

conservation of energy

c)

conservation of momentum

d)

conservation of charge

54.

If you add 450 mL of distilled water to 50 mL of a solution that is 2.0 M, what is the new concentration?

a)

0.2 M

b)

0.5 M

c)

1.0 M

d)

2.0 M

55.

If a solution has a pH of 7.8, the [H3O+] is

a)

1.6 x 10^{-8} M

b)

7.8 x 10^{-7} M

c)

1.0 x 10−710^{-7} M

d)

6.3 x 10^{-6} M

56.

If the pH of a solution is 3.8, the pOH is:

a)

10.2

b)

3.8

c)

7.0

d)

0.2

57.

The role of a buffer is to

a)

resist changes in pH

b)

increase the rate of reaction

c)

completely neutralize acids

d)

provide energy to cells

58.

If the [OH−]=2×10−4[OH^-] = 2 \times 10^{-4} , the pH= (a)  

59.

Nitric acid (HNO3) is a weak acid.

a)

True

b)

False

60.

When ammonia is added to water, the water acts as an acid.

a)

True

b)

False

61.

When HCl is added to water, water acts as a base.

a)

True

b)

False

62.

Adding 100.0g of sodium carbonate to 1.0 L of water will give concentration of:

a)

0.943 M

b)

0.500 M

c)

1.200 M

d)

0.250 M

63.

If a solution is made from 12.5 g of NaCl and 187.5 g of H2O, what is the m/m%?

a)

6.25%

b)

12.5%

c)

18.75%

d)

25%

64.

How many grams of sodium sulfate would be required to produce 500. mL of 0.25 M solution?

a)

17.75 g

b)

8.88 g

c)

35.50 g

d)

4.44 g

65.

What is the [OH-] if [H3O+]=2.5x10−4[H3O+] = 2.5 x 10^{-4} ?

a)

4.0x10−11M4.0 x 10^{-11} M

b)

2.5 x 10^{-4} M

c)

1.0 x 10−710^{-7} M

d)

4.0 x 10^{-8} M

66.

When a solution is acidic the pH is less than 7.

a)

True

b)

False

67.

When you add an acid to a buffered solution the pH goes up.

a)

True

b)

False

68.

Most solutes are more soluble at higher temperatures than lower temperatures.

a)

True

b)

False

69.

When an acid and base react, the result is

a)

salt and water

b)

oxygen and hydrogen

c)

carbon dioxide and water

d)

ammonia and methane

70.

Number of protons in a copper atom.

a)

29

b)

26

c)

24

d)

30

71.

If you have 100.0 grams of an isotope with a half life of 2.5 days, how much will remain after 7.5 days?

a)

12.5 grams

b)

25.0 grams

c)

50.0 grams

d)

6.25 grams

72.

How many electrons does Ag+ contain?

(a)  

73.

The formula for phosphorus tribromide is:

a)

PBr3

b)

PBr5

c)

PB3

d)

P3Br

74.

The formula for the bromide ion is:

a)

Br-

b)

Br2

c)

BrO3-

d)

Br+

75.

The name of SrS is:

4 lines
76.

The number of protons in uranium.

(a)  

77.

The charge on ruthenium in Ru(SO4)2 is:

(a)  

78.

The number of neutrons in 32P is:

a)

17

b)

15

c)

16

d)

18

79.

The name of PO3 is:

a)

Phosphorus trioxide

b)

Phosphate

c)

Phosphite

d)

Hypophosphite

80.

There are ____ neutrons in the most common isotope of nitrogen.

a)

7

b)

6

c)

8

d)

5

81.

Fusion is the breaking apart of a nucleus in radioactive decay.

a)

True

b)

False

82.

The formula for cobalt (II) oxide is:

a)

CoO

b)

Co2O3

c)

Co3O4

d)

Co(OH)2

83.

True or False, sulfur trioxide is ionic.

a)

True

b)

False

84.

MoO is ionic.

a)

True

b)

False

85.

An atom of europium contains ___ protons.

a)

63

b)

47

c)

78

d)

54

86.

if an atom does not contain an equal number of protons and electrons, it is an ion.

a)

True

b)

False

87.

If an atom loses an electron, it is negatively charged.

a)

True

b)

False

88.

The name for PO3^3- is:

a)

Phosphite ion

b)

Phosphate ion

c)

Perphosphate ion

d)

Hypophosphite ion

89.

The name of Md is:

(a)  

90.

A noble gas in period 4.

a)

Krypton

b)

Argon

c)

Xenon

d)

Neon

91.

Element described by group 4A and period 3.

a)

Silicon

b)

Carbon

c)

Germanium

d)

Tin

92.

Number of atoms in 4.3 moles of Au.

a)
5.67 x 10^24 atoms
b)
2.59 x 10^24 atoms
c)
1.74 x 10^23 atoms
d)
3.01 x 10^25 atoms
93.

How many grams are in 4.3 moles of Au?

a)

846.5 grams

b)

120.0 grams

c)

500.0 grams

d)

1000.0 grams

94.

What is the electron configuration of antimony?

a)

[Kr] 4d10 5s2 5p3

b)

[Xe] 4f14 5d10 6s2 6p3

c)

[Ar] 3d10 4s2 4p3

d)

[Ne] 3s2 3p3

95.

What shape is the compound PCl5?

a)

Trigonal bipyramidal

b)

Tetrahedral

c)

Octahedral

d)

Square planar

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