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Second Semester Accelerated Chemistry Review

Total questions: 70

Worksheet time: 3hrs 5mins

Name
Class
Date
1.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
2.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
3.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
4.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
5.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
6.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
125.2 g O2
7.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
8.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
9.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
10.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
11.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
12.

How many particles are in 13.5 grams of Beryllium?

a)

1.50 particles

b)

9.03 particles

c)

4.00x1023 particles

d)

9.03x1023 particles

13.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
14.
What is the molar mass of Fe3(PO4)2
a)
823.8g/mol
b)
357.5 g/mol
c)
455.6g/mol
d)
86.3g/mol
15.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
16.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
17.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
18.

Identify the Empirical Formula for:

C4H6

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

19.

Identify the Empirical Formula for:

Br2O6

a)

BrO3

b)

Br6O2

c)

BrO

d)

Br2O6

20.

Identify the Empirical Formula for:

C2H4

a)

CH

b)

CH2

c)

C4H2

d)

C2H4

21.

What describes the motion of a Gas Molecule?

a)

Molecules are far apart

b)

Move in constant, random motion

c)

It will travel in a straight path

d)

All of the above

22.

If pressure goes down in a container, what happens to volume when the temperature is held constant.

a)

Increase

b)

Decrease

23.

If temperature goes down in a container, what happens to volume when the pressure is held constant.

a)

Increase

b)

Decrease

24.

If you add gas particles to the container, what happens to the volume when the pressure and temperature is held constant.

a)

Increase

b)

Decrease

25.

How would you convert 34oC to Kelvin?

a)

K = oC + 273

b)

oC = K + 273

c)

K = oC - 273

d)

oC = K + 273

26.

What formula would you use to solve the following: A 0.562 L container of Helium has a pressure of 9.5 atm. What volume would be necessary to decrease the pressure to 2.4 atm?

a)
b)
c)
d)
27.

What formula would you use to solve the following: A sample of nitrogen gas was collected over water at a temperature of 23.0°C. What is the partial pressure of nitrogen if the atmospheric pressure (total) was 785 mmHg and the vapor pressure of water was 21.1 mmHg?

a)
b)
c)
d)
28.

What formula would you use to solve the following: A container of carbon monoxide gas is at a temperature of 65.0 °C and occupies a volume of 6.5L. At what temperature would it occupy a volume of 10.2L?

a)
b)
c)
d)
29.

What formula would you use to solve the following problem: A gas at 880mmHg and 298K occupies a container with an initial volume of 1.00 L. The pressure increases to 1980mmHg as the temperature rises to 398K. What will be the new volume?

a)
b)
c)
d)
30.

What formula would you use to solve the following: At high altitudes, pilots have to supplement their supply of oxygen. In this mixture, there are oxygen and nitrogen gases. If nitrogen’s partial pressure is 250mmHg, calculate the partial pressure of oxygen if the total pressure is 710mmHg.

a)
b)
c)
d)
31.

What formula would you use to solve the following: 6.25L of nitrogen gas is known to contain 5.21 moles. If the amount of nitrogen is increased to 12.64 moles, what new volume will result (at unchanged temperature and pressure)?

a)
b)
c)
d)
32.

What formula would you use to solve the following problem: A container has an initial volume of 4.5 L, a pressure of 450 kPa and is at a temperature of 15oC. If the container is expanded to 6.5 L while the pressure is decreased to 125 kPa, find the resulting temperature.

a)
b)
c)
d)
33.

What formula would you use to solve the following question: How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of

12.4 atm and a temperature of 850 C?

2H2(g) + O2(g) --> 2H2O(l)

a)
b)

STOICH and PV = nRT

c)
d)
34.

What formula would you use to solve the following: If a cylinder has a volume of 5.4 x 106 L of air at a pressure of 140 kPa and it is determined that there are 3.0 x 105 moles of CO2 present, calculate the temperature inside the cylinder.

a)
b)
c)
d)
35.

What formula would you use to solve the following problem: 76 L of compressed oxygen is at a temperature of 330 K. If there are 7.3 moles of oxygen in the container, calculate the pressure (in atm) inside the container.

a)
b)
c)
d)
36.

Which of the following is NOT a unit of Pressure?

a)

mmHg

b)

atm

c)

kelvin

d)

psi

37.

Which Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagodro's Law

d)

Combined Gas Las

38.

What Gas Law does this graph represent?

a)

Boyle's Law

b)

Charles' Law

c)

Avagadro's Law

d)

Combined Gas Law

39.

In the Question: A cylinder has a volume of 5.4 L of air at a pressure of 140 atm. If the volume is increased to 12.4L, what would the new pressure be? Which answer choice has the data correctly labeled?

a)

P1=5.4L, V1=140atm; P2= 12.4L, V2= ?

b)

P1=140atm, V1=5.4L ; P2= ?, V2=12.4L

c)

T1=140atm, V1=5.4L ; T2= ?, V2=12.4L

d)

There was no important data to label

40.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

41.

What unit do you use to measure Thermal Energy?

a)

J/g ºC

b)

g

c)

ºC

d)

J

42.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
43.

Water has a specific heat of 4184 J/gºC. Wood has a specific heat of 1760 J/gºC. What material needs more energy to raise the temperature 1ºC

a)

Wood

b)

Water

c)

Both are the same

44.
Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?
a)
Copper
b)
Carbon Steel
c)
Zinc
d)
Stainless Steel
45.
How does heat flow?
a)
Always from cold to warm
b)
Always from warm to cold
c)
Both warm to cold & cold to warm
d)
It depends on the temperature
46.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
47.

How many Joules of energy are required to change 10 gram of liquid water from 20 C to 90 C?

a)

1400 J

b)

2800 J

c)

210,000 J

d)

1,400,000 J

48.
The specific heat of aluminum is 0.21 J/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
49.

For a skillet, used for cooking, do you want a high or low specific heat? and why?

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

50.
20 g of water. specific heat of water is 4.18 J/x°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
51.

There are four cups of hot cocoa. The cup sizes are shown. The temperature of the cocoa in each cup is 25 degrees celsius. Which cup has the MOST thermal energy?

a)

Largest cup (Trenta)

b)

Small cup (Tall)

c)

Venti

d)

All three are the same temperature so they have same thermal energy

52.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
53.

If the specific heat of water is 4,184 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

112,575.9 K

54.

Joules and calories are units of measurement for __________________.

a)

heat

b)

insulators

c)

conductors

d)

thermometers

55.

What must occur to have an effective reaction to occur? (Select all answers that apply).

a)

Sufficient energy

b)

Correct orientation

c)

Two different reactants.

d)

minimum activation energy

56.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
57.

What does a catalyst do to speed up a reaction?

a)

It reduces the surface area of the reactants

b)

It increases the surface area of the reactants.

c)

It reduces the required energy for a chemical reaction to occur and provides an alternative pathway.

d)

It increases the required energy for a chemical reaction to occur

58.
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
59.
Why does a higher concentration increase the rate of reaction?
a)
it increases the amount of reactants
b)
it lowers the activation energy
c)
it increases the energy of particle collisions
d)
it increases the frequency of particle collisions because there are more collision sites
60.

If the temperature is increased, then the rate is ........... and the time required for the reaction is  ............

a)

Increases, decreases

b)

Increases, increases

c)

decreases, increases

d)

decreases, decreases

61.

Increasing the number of collisions between reactants causes the rate to.........  This happens by ...... the concentration or by  ......the temperature.

a)

Increases, increase, increase

b)

increases, decrease, decrease

c)

decreases, increase, increase

62.
For the equilibrium reaction
2NH3(g) + 22 kJ ↔ N2(g) + 3H2(g),
which of the following changes would result in the formation of more N2 and H2 at equilibrium?

a)
increasing temperature
b)
adding N2
c)
removing NH3
63.
2.In the Haber process, gaseous ammonia is produced on an industrial scale by combining nitrogen and hydrogen gases, according to this equation: 
N2(g) + 3H2(g) ↔ 2NH3(g)
The process is exothermic. Which of the following actions will shift the reaction in the forward (product) direction?

a)
Increase the temperature of the reaction.
b)

Reduce ammonia (NH3) concentration by removing ammonia from the reaction chamber.

c)
Reduce hydrogen concentration by reducing the amount of hydrogen in the reaction chamber.
64.
The principle that states that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:
a)
The principle of equilibrium
b)
Priestley’s principle
c)
Le Chatelier’s principle
d)
Faraday’s principle
65.
A system at equilibrium means it is still reacting.
a)
True
b)
False
66.
For an endothermic reaction, heat can be thought of as:
a)
a reactant
b)
a product
c)
either it has no effect
d)
neither it effects both sides equally.
67.
Increasing the concentration of the reactants will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
68.
Increasing the temperature of an exothermic reaction will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
69.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
70.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse

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