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Chemistry 2nd Semester Review

Total questions: 77

Worksheet time: 3hrs 34mins

Name
Class
Date
1.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
2.

An exothermic reaction means the transfer to heat energy goes from​ the (a)   to the​ (b)  

Choose from the below words
system
surroundings
beaker
water
3.

You have 150g of water that is heated from 10.0°C until its temperature is 27°C.  If the specific heat of water is 4.18 J/g°C, calculate the amount of heat energy needed to cause this rise in temperature. (type answers in without units and no decimals)

(a)  

4.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
5.

A negative Q value means...

a)

it was exothermic

b)

it was endothermic

c)

energy left and entered the system

d)

it was reactive

6.

If a sample of 5.2 g of water (c=4.18) loses 7,923 J of energy, what was the change in temperature?

a)

364.5 CoC^o  

b)

-364.5 CoC^o  

c)

11,000 CoC^o  

d)

32 CoC^o  

7.

Calculate ΔT\Delta T  when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

8.

Calculate A 50g sample is heated with 500 joules of energy and has a 10*C temperature change. Calculate it’s specific heat.

a)

1 j/g*C

b)

250000 j/g*C

c)

500 j/g*C

d)

10 j/g*C

9.

A sample of a compound has a mass of 77 g and a specific heat of 0.885 J/g*K. In order to increase the temperature by 25 degrees Celsius, how much heat must be added? ( q=mcΔTq=mc\Delta T  )

a)

-3.48 J

b)

3.48 J

c)

1704 J

d)

-1704 J

10.

A sample of a compound has a mass of 30 g and a specific heat of 0.258 J/g*K. If its temperature drops 40 K, how much heat was released? ( q=mcΔTq=mc\Delta T  )

a)

309.6 J

b)

-309.6 J

c)

465 J

d)

-465 J

11.

The quantity of heat required to change the temperature of 1 g of water 1 C

a)

Specific Heat

b)

Heat

c)

Joule

d)

Calorie

12.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

13.

What device is used to measure the amount of heat involved in a chemical reaction or physical process?

a)

barometer

b)

calorimeter

c)

thermometer

14.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
15.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

16.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
17.

How does a solution become supersaturated?

a)

Vigorous stirring to dissolve more solute than usual.

b)

Heat the solution to increase the solute then let it cool.

c)

Add more solvent to lower the concentration.

d)

Keep pouring solute in the solvent until it goes in.

18.
When 50 grams of KCl is dissolved in 100 grams of water at 50 ºC, the solution can be correctly described as:
a)
supersaturated
b)
unsaturated
c)
saturated
19.
When 20 grams of KNO3 is dissolved in 100 grams of water at 80 ºC, the solution can be correctly described as:
a)
supersaturated
b)
saturated
c)
unsaturated
20.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
21.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
22.
What is a solute?
a)
The substance that does the dissolving in a solution.
b)
The substance that is dissolved into the solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
23.

Which of the following actions would dilute a solution?

a)

Adding more solute

b)

Removing some solvent

c)

Adding more solvent

d)

Heating the solution

24.

Which of the following solutions is the most dilute?

a)

25 ml citric acid

50 ml water

b)

10 ml citric acid

50 ml water

c)

25 ml citric acid

150 ml water

d)

75 ml citric acid

150 ml water

25.

Jackson is making dinner and is trying to dissolve salt into a pot of water. The salt is dissolving slowly. What should Jackson do to speed up the rate of dissolving?

a)

He should put larger salt particles in the water.

b)

He should heat the water to a higher temperature.

c)

He should completely stop stirring the pot of water.

d)

He should slow down the speed he is stirring the pot.

26.

What combination would dissolve a solid solute the fastest?

a)

high temperature, no stirring

b)

no heat, no stirring

c)

sugar cube, no heat

d)

high temperature, stirring

27.

What is the molarity of 1.2 moles of CaCO3 in 1.22 L of solution?

a)

0.98 M

b)

9.8 M

c)

5.11 M

d)

0.16 M

28.

What is the percent by mass of a solution made by dissolving 20.0 g of NaCl into 180.0 g of water?

a)

10.0 %

b)

11.1 %

c)

80.0 %

d)

20.0 %

29.

What is the percent concentration of sugar in pink lemonade if 28 g of sugar is added to 209 g of water?

a)

14.7 %

b)

5.14 %

c)

13.4 %

d)

8.47 %

e)

11.8 %

30.
If you have 0.045 L of 0.465 M potassium bromide. How many moles of potassium bromide are present?
a)
20.9 mol
b)
0.021 mol
c)
0.02 mol
d)
0.0209 mol
31.
How many L are required to make 3.5 M hydrochloric acid using 1.1 moles? 
a)
3.18 L
b)
0.31 L
c)
3.85 L
d)
4.6 L
32.
Calculate the volume that a 0.323-mol sample of a gas will occupy at -8oC and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
33.
The volume of a gas is increased from 150.0 mL to 350.0 mL by heating it. If the original temperature of the gas was 25oC, what will its final temperature be (in oC)
a)
146 oC
b)
10.7 oC
c)
58.3 oC
d)
422 oC
34.
At a constant temperature, the volume decreases.  What happens to the pressure?
a)
increases
b)
decreases
c)
stays the same
35.
At a constant pressure, the volume decreases.  What happens to the temperature?
a)
increases
b)
decreases
c)
stays the same
36.
A 2.00 L sample of pure oxygen gas (O2) is measured at STP.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
37.
A 7.00 L sample of argon gas at 420. K exerts a pressure of 625 kPa.  If the gas is compressed to 1.25 L and the temperature is lowered to 350 K, what will be its new pressure in atm?
a)
10.4 atm
b)
2920 atm
c)
2916.7 atm
d)
28.8 atm
38.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
39.

For the problem below, what is the value for the final pressure?

A gas with a volume of 4.0 L at 90.0 kPa expands until the pressure drops to 20.0 kPa. What is its new volume if the temperature doesn’t change?

a)

14.0 L

b)

20.0 L

c)

90.0 L

d)

18.0 L

40.
The pressure on a sample of gas is increased from 1.0 atm to 3.0 atm. If the new volume is 0.52 L, find the original volume.
a)

1.25 L

b)

1.56 L

c)

0.173 L

d)

None of these is very close.

41.
What is the new volume of the gas if the pressure on 350 L of oxygen at 720 mm Hg is decreased to 600 mm Hg?
a)
420 L
b)
29.16 L
c)
4200.0 L
d)
291.6 L
42.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
43.

The coldest temperature, 0 Kelvin, that can be reached. It is the temperature at which all molecular motion stops.

a)

Zero Celsius

b)

Freezing Point

c)

STP

d)

Absolute Zero

44.

a hypothetical gas that perfectly fits all the assumptions of the kinetic-molecular theory

a)

Real Gas

b)

Ideal Gas

c)

Standard Gas

d)

Universal Gas

45.

Movement of molecules from an area of higher concentration to an area of lower concentration.

a)

Effusion

b)

Diffusion

c)

Ideal Gas

d)

Kinetic Molecular Theory

46.

An instrument that measures atmospheric pressure

a)

Barometer

b)

Thermometer

c)

Spirometer

d)

Altimeter

47.
Which of the following is NOT a factor affecting reaction rate?
a)
temperature
b)
catalysts
c)
particle size
d)
polarity
48.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
49.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
50.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
51.
Limestone chunks are reaction with hydrochloric acid solution at constant temperature with average speed. If we crash the chunks of limestone into powder how would speed of reaction change?
a)
Reaction speeds up
b)
Reaction does not change
c)
Reaction slows down
d)
Reaction stops
52.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
53.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing surface area

d)

all of the above

54.

Which alteration will shift the equilibrium reaction below to form more reactants? NH4Cl + heat <-> NH3 + HCl

a)

Increase concentration of NH3 and HCl

b)

decrease concentration of NH3 and HCl

c)

increase the temperature

d)

add a catayst

55.
Given the reaction at equilibrium:
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the forward reaction rate due to
a)
a decrease in the number of effective collisions
b)
an increase in the number of effective collisions
c)
a decrease in the activation energy
d)
an increase in the activation energy
56.
Given the equation representing a reaction at equilibrium: 
N2(g) + 3H2(g) --> 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
a)
decreasing the concentration of H2(g)
b)
decreasing the pressure
c)
increasing the concentration of N2(g)
d)
increasing the temperature
57.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if N2 was removed?
a)
Shift right 
b)
Shift left
c)
No shift
d)
Shift both directions
58.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if H2 was removed?
a)
Shift right 
b)
Shift left
c)
No shift
d)
Shift both directions
59.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
60.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
61.

Consider the following reaction. What would be the equilibrium constant expression?

4Br2(g) + CH4(g) ↔ 4HBr(g) + CBr4(g)

a)

Kc = [Br2]4 [CH4]/ [HBr]4 [CBr4]

b)

Kc = [HBr]4 [CBr4]/ [Br2]4 [CH4]

c)

Kc = [HBr ]/ [Br2]4 [CH4]

d)

Kc = [HBr]4 [CBr4]/ [Br2]4 [CH]4

62.

What is the reaction/equation for this Kc expression

a)

2N2 + O2 ⇌ 2NO

b)

N2 + O2 ⇌ NO

c)

NO ⇌ 2NO

d)

N2 + O2 ⇌ 2NO

63.

When acid and base react with each other.what compound are formed?

a)

Water only

b)

Metal oxide only

c)

Salt and water

d)

All the above

64.

What is the nature of water

a)

Acidic

b)

Basic

c)

Netural

d)

None of the above

65.

This image represents

a)

neutralization reaction

b)

synthesis

c)

decompostion

d)

single displacement

66.
What are properties of a base?
a)
Slippery, bitter, does not react with metals, pH above 7.
b)
Slippery, bitter, reacts with metals, pH below 7.
c)
Sour, reacts with metals, pH below 7
d)
Sour, reacts with metals, pH above 7.
67.

Which is the correct set of acid properties?

a)

sour taste, reacts with metals, change litmus paper blue

b)

sour taste, reacts with metals, change litmus paper red

c)

bitter taste, slippery, change litmus paper red

d)

sour taste, slippery, change litmus paper red

68.

According to Bronsted-Lowry, what does an acid do?

a)

It donates a proton (H+).

b)

It accepts a proton (H+)

c)

It produces H+ in water.

d)

It produces OH- in water.

69.

What is the Lewis definition of acid and bases (Remember what do we know Lewis from?)

a)

Acids have H

Bases have OH

b)

Acids are proton donors

Bases are proton acceptors

c)

Acids can gain protons, Bases can lose protons

d)

Acids are electron acceptors

Bases are electron donors

70.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

71.

The strongest bases have pH values close to

a)

0

b)

14

c)

7

d)

5

72.

NaOH is a strong base.

What is the pH of a 0.01 M NaOH soltuion?

a)

2

b)

9

c)

12

d)

14

73.

The pH of a solution is 8.43. What is the hydrogen ion H+ concentration?

a)

3.7 x 10-9 M

b)

2.7 x 10-6 M

c)

1.0 x 10-8.43 M

d)

1.0 x 10-14

74.

If the [H+] of a solution is 6.8 x 10-9 M, the pH is

a)

8.17

b)

5.73

c)

9.99

d)

8.62

75.

if the [H+] of a solution is 8.4 x 10-3 M, the pOH of the solution will be

a)

2.08

b)

11.92

c)

1.02

d)

12.98

76.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

77.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

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