Semester 2 Review

In the formation of carbon dioxide from carbon monoxide and oxygen, how many moles of carbon monoxide are needed to react completely with 7.0 moles of oxygen gas?
2 CO (g) + O₂(g) → 2 CO₂ (g)
1. 14
2. 7
3. 3.5
4. 21
How many moles of oxygen are required to burn 22.4 liters of ethane gas, C₂H₆ at standard conditions?
2 C₂H₆ (g) + 7 O₂(g) → 4 CO₂ (g) + 6 H₂O (g)
1. 3.5
2. 7
3. 14
4. 11.2
How many grams of water can be prepared from 5 moles of hydrogen at standard conditions?
2 H₂ (g) + O₂(g) → 2 H₂O
1. 5
2. 10
3. 3.6
4. 90
How many grams of water can be prepared from 8 grams of hydrogen at standard conditions?
2 H₂ (g) + O₂(g) → 2 H₂O
1. 72
2. 18
3. 2
4. 8
A certain amount of glucose, C₆H₁₂O₆ burned in oxygen, and produced 22 grams of carbon dioxide, CO₂. How many grams of water was produced at the same time?
C₆H₁₂O₆ (s) + 6 O₂(g) → 6 CO₂ (g) + 6 H₂O (g)
1. 9
2. 18
3. 4.5
4. 22
How many grams of calcium will react with 44.8 liters of oxygen gas at standard conditions?
2 Ca + O₂ → 2 CaO
1. 160
2. 20
3. 10
4. 224
Gas pressure is caused by:
1. gas molecules hitting other gas molecules
2. gas molecules hitting the walls of a container
3. gas molecules reacting with other gas molecules
4. gas molecules heating up
"Absolute zero" is equal to:
1. 0 °C
2. 0 K
3. 0 °F
4. -273 °C
5. 100 °F
No temperature can be reached that is below:
1. 0 Celsius
2. 0 Kelvin
3. 0 Fahrenheit
4. 273 Kelvin
On the Kelvin scale, a temperature of 22 degrees celsius has a value of:
1. -251 kelvins
2. 0 kelvins
3. 295 kelvins
4. 259 kelvins
Convert 300 °C to Kelvins
1. 300 °C = 27 K
2. 300 °C = 573 K
3. 300 °C = -27 K
4. 300 °C = 1060 K
Convert 100 K to °C
1. 100 K = 373 °C
2. 100 K = -173 °C
3. 100 K = 473 °C
4. 100 K = 173 °C
Which pressures are equal to 1 atmosphere?
1. 273 torr
2. 760 atm
3. 760 torr
4. 101.3 kPa
5. 273 kPa
Standard Temperature is equal to
1. 0 ºC
2. 0 ºK
3. 0 ºF
4. 273 ºC
5. 273 K
Standard Pressure is equal to:
1. 273 kPa
2. 760 torr
3. 1 torr
4. 760 atm
5. 101.3 kPa
6. 1 atm
Which pairs represent Standard Temperature and Pressure (STP)?
1. 273 K and 1 atmosphere
2. 273 °C and 760 atmospheres
3. 273 °C and 1 atmosphere
4. 273 K and 101.3 kPa
5. 0 °C and 760 torr
6. 0 °C and 273 kPa
At standard pressure, a sample of nitrogen occupies 500 mL. What volume does the gas occupy when the pressure doubles?
1. 1000 mL
2. 250 mL
3. 380 mL
4. 2 mL
At a pressure of 5.0 atmospheres, a sample of gas occupies 40. liters. What volume will the same sample occupy at 1.0 atmosphere.
1. 8.0 liters
2. 200 liters
3. 0.13 liters
4. 0.0050 liters
At constant pressure and 25 °C a sample of gas occupies 4.5 liters. At what temperature will the gas occupy 9.0 liters?
1. 50 °C
2. 596 °C
3. 596 K
4. 50 K
A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL?
1. 125 K
2. 375 K
3. 500 K
4. 2250 K
In a closed container at 1.0 atmosphere, the temperature of a sample of gas is raised from 300 K to 400 K. What will be the final pressure of the gas?
1. 1.3 atmospheres
2. 100 atmospheres
3. 0.010 atmospheres
4. 0 atmospheres
A helium filled balloon has a volume of 4.0 L at 275 K and 800 mm Hg. What volume does the gas occupy at 550 K and 400 mm Hg?
1. 16 L
2. 8 L
3. 32 L
4. 1 L
As the volume of a confined gas decreases at constant temperature, the pressure exerted by the gas:
1. increases
2. decreases
3. stays the same
4. fluctuates
As the temperature of a confined gas increases, the pressure:
1. increases
2. decreases
3. stays the same
4. fluctuates
Organize the following gases in order of their rates of difusion, from slowest to fastest:
- oxygen, O₂
- ammonia, NH₃
- hydrogen, H₂
- carbon dioxide, CO₂
1. hydrogen, ammonia, oxygen, carbon dioxide
2. hydrogen, oxygen, ammonia, carbon dioxide
3. oxygen, hydrogen, carbon dioxide, ammonia
4. hydrogen, oxygen, carbon dioxide, ammonia
5. carbon dioxide, oxygen, ammonia, hydrogen
At which of the following temperatures will a gas diffuse through a room most rapidly?
1. 0 ºC
2. 10 ºC
3. 20 ºC
4. 30 ºC
At a temperature of 25 degrees celsius and a pressure of 1 atmosphere, which of the following molecules will have the highest average speed?
1. hydrogen chloride, HCl
2. oxygen, O₂
3. nitrogen, N₂
4. carbon dioxide, CO₂
A volume of gas at constant pressure experiences a temperature increase of 13 K. As a result of this temperature increase:
1. The volume of the gas will decrease.
2. The average kinetic energy of the gas molecules increases.
3. The mass of the gas increases.
4. The gas particles experience greater attractive forces.
Each of these flasks contains the same number of gas molecules. In which would the pressure be highest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Each of these flasks contains the same number of gas molecules. In which would the pressure be lowest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
If all of the following flasks are the same size, at the same temperature, and contain the same number of molecules, in which flask will the pressure be highest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
5. All have the same pressure
If all of the following flasks are the same size, at the same temperature, and contain the same number of molecules, in which flask will the molecules be moving fastest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
If all of the following flasks are the same size, at the same temperature, and contain the same number of molecules, in which flask will the molecules be moving slowest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Each of these flasks is the same size and at the same temperature. Which one contains the most molecules?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Each of these flasks is the same size and at the same temperature. Which one contains the fewest molecules?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Each of these flasks is the same size and at the same temperature. In which flask will diffusion occur most slowly?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Four different flasks contain gas samples at 298 K. In which of the following samples will the gas molecules be moving the fastest?
1. H₂
2. O₂
3. N₂
4. CO₂
Which of the following changes to a system WILL NOT result in an increase in pressure?
1. Decreasing the volume of the container
2. Adding more gas molecules
3. Raising the temperature
4. Increasing the volume of the container
Each of these flasks contains the same number of molecules. In which container is the pressure highest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Four different flasks contain gas samples at 298 K. In which of the following samples will the gas molecules be moving the slowest?
1. H₂
2. O₂
3. N₂
4. CO₂
Each of these flasks contains the same number of molecules. In which container is the pressure lowest?
1. Flask 1
2. Flask 2
3. Flask 3
4. Flask 4
Definite shape, definite volume, and a low rate of diffusion are characteristics of:
1. Gases
2. Liquids
3. Solids
4. Fluids
During the phase change from liquid to solid:
1. energy must be absorbed
2. energy must be removed
3. there is no change in energy
During the phase change from liquid to vapor:
1. energy must be absorbed
2. energy must be removed
3. there is no change in energy
During phase changes, the temperature of the substance undergoing change:
1. continues to increase
2. continues to decrease
3. stays the same
4. fluctuates
In a solution of sugar and water, the solvent is the:
1. sugar
2. water
In a solution of sugar and water, the solute is the:
1. sugar
2. water
A substance whose water solution does not conduct an electric current is a(n):
Which of the following substances, when dissolved in a water solution, will allow current to flow in the device pictured above, resulting in the lightbulb becoming lit?
1. Ethanol (ethyl alcohol)
2. sodium chloride
3. Sucrose (table sugar)
4. HCl - hydrochloric acid
5. sodium hydroxide
Gases dissolve best in liquids when:
1. the pressure is high and the temperature is high
2. the pressure is low and the temperature is high
3. the pressure is high and the temperature is low
4. the pressure is low and the temperature is low
The solubility of potassium nitrate in water at 35 °C is about 60 grams KNO₃ per 100 grams of water. How many grams of KNO₃ should dissolve in 300 grams of water at 35 °C?
1. 180 grams
2. 20 grams
3. 335 grams
Breaking up a solid speeds dissolving in a liquid by:
1. raising the temperature
2. decreasing the pressure
3. increasing surface area
4. slowing hydration
Most salts become more soluble in water as the:
1. pressure is increased
2. pressure is decreased
3. temperature is increased
4. temperature is decreased
Fats do not dissolve in water because:
1. Fats and water are both nonpolar
2. Fats are polar and water is nonpolar
3. Fats and water are both polar
4. Fats are nonpolar and water is polar
Calculate the concentration of the following solution in units of grams per liter:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 36 g/L
2. 0.250 g/L
3. 4 g/L
4. 15 g/L
Calculate the concentration of the following solution in units of molarity, M, moles per liter:

80 grams of NaOH is dissolved in 2 L of solution
1. 1 M NaOH
2. 40 M NaOH
3. 160 M NaOH
4. 82 M NaOH
Calculate the concentration of the following solution in units of parts per million, ppm:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 4000 ppm NaCl
2. .004 ppm NaCl
3. 4 ppm NaCl
4. 4 x 10⁶ ppm NaCl
Calculate the concentration of the following solution in units of percent composition:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 40% NaCl
2. 0.0068% NaCl
3. 0.4% NaCl
4. 25% NaCl
What two substances are always produced by a neutralization reaction?
1. an acid and a base
2. water and a base
3. water and a salt
4. water and an acid
According to the Brønsted-Lowry definition, a base is:
1. a proton donor
2. a proton acceptor
3. a proton
4. a proton destroyer
Acids taste:
1. Sweet
2. Salty
3. Bitter
4. Sour
Bases taste:
1. Sweet
2. Salty
3. Bitter
4. Sour
A positive test for an acid occurs when:
1. red litmus turns blue
2. red litmus remains red
3. blue litmus turns red
4. blue litmus remains red
A positive test for a base occurs when:
1. red litmus turns blue
2. red litmus remains red
3. blue litmus turns red
4. blue litmus remains red
Bases cause phenolphthalein to turn:
1. orange
2. green
3. violet
4. clear
Strong acids:
1. Ionize slightly and produce few hydrogen ions in solution
2. Ionize completely and produce many hydroxide ions in solution
3. Ionize completely and produce many hydrogen ions in solution
4. Ionize slightly and produce few hydroxide ions in solution
Indicator Results
Phenolphthalein Clear
Red litmus Remains red
Blue litmus Turns red
Methyl orange Turns deep red

An unknown substance produced the experimental results noted above. Based on this data, the unknown is:
1. a base
2. a sugar
3. an acid
4. impossible to identify
The strongest bases are hydroxides of:
1. halogens
2. noble gases
3. transition metals
4. group 1 and group 2 metals
Which of the following is a property of acids?
1. Feel slippery
2. Turn red litmus blue
3. taste bitter
4. react with metals to form hydrogen gas
Acids have a pH that is:
1. greater than 7
2. equal to 7
3. less than 7
Bases have a pH that is:
1. greater than 7
2. equal to 7
3. less than 7
Which of the following pH values indicates the strongest acid?
1. 1
2. 4
3. 7
4. 11
When 100 mL of 1 M HCl is added to 100 mL of 2 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
When 200 mL of 1 M HCl is added to 100 mL of 1 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
When 100 mL of 1 M HCl is added to 100 mL of 1 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
The specific heat of water is 4.18J/(g·ºC). How many joules are required to heat 100 grams of water from 25ºC to 35ºC?
1. 4180 J
2. 239 J
3. 14630 J
4. 10450 J
A 5 gram piece of a metal at 0ºC absorbs 1000 J of energy, after which the temperature of the metal is 400ºC. What is the specific heat of the metal?
1. 0.5 J/(g·ºC)
2. 2 J/(g·ºC)
3. 0.25 J/(g·ºC)
4. 2 x 10⁶ J/(g·ºC)
The specific heat of gold is 0.13 J/(g·ºC). How many joules are required to heat 40 grams of gold from 60ºC to 85ºC?
1. 130 J
2. 12.3 J
3. 4.8 J
4. 13 J
Ice has a specific heat of 2 J/(g·ºC). How many joules must be absorbed by a 50 gram piece of ice in order to raise the temperature from -18ºC to -10ºC?
1. 800 J
2. 12.5 J
3. 3.125 J
4. 0.32 J
The molar heat of fusion for water is 6 kJ/mol. How much energy is required to melt 3 moles of ice at 0ºC?
1. 18 kJ
2. 2 kJ
3. 0.50 kJ
4. 9 kJ
The molar heat of fusion for water is 6 kJ/mol. How much energy must be removed from 10 moles of water at 0ºC in order to convert it to ice at 0ºC?
1. 60 kJ
2. 0.6 kJ
3. 1.66 kJ
4. 16 kJ
The molar heat of vaporization for water is 41 kJ/mol. How much energy must be absorbed by 20 moles of water at 100ºC in order to convert it to steam at 100ºC?
1. 820 kJ
2. 4100 kJ
3. 82 000 kJ
4. 8.2 kJ
The process of converting ice to water by occurs by:
1. the addition of energy
2. the removal energy
3. no change in energy
Which of the following is written incorrectly?
1. liquid water + energy --> ice
2. liquid water + energy --> water vapor
3. water vapor --> liquid water + energy
4. ice + energy --> liquid water
Equal masses of each of the following substances absorb an equal amount of energy. Which substance experiences the greatest temperature increase?

Iron; specific heat = 0.449 J/(g·ºC)
Aluminum; specific heat = 0.897 J/(g·ºC)
Liquid water; specific heat = 4.18 J/(g·ºC)
Ice; specific heat = 2.06 J/(g·ºC)
1. Iron
2. Aluminum
3. Liquid water
4. Ice
Which of the following will always increase the rate of a chemical reaction?
1. An increase in pressure
2. An increase in concentration of reactants
3. An increase in temperature
4. A decrease in pressure
An increase in temperature increases the rate of a chemical reaction by what means
1. Increasing the concentration of reactants
2. Increasing pressure
3. Decreasing activation energy
4. Increasing collision energy
5. Increasing collision frequency
Catalysts increase the rate of a chemical reaction by what means?
1. Increasing collision energy
2. Increasing the concentration of reactants
3. Lowering activation energy
4. Increasing temperature
Which of the following will burn most rapidly?
1. Solid alcohol
2. Liquid alcohol
3. Vaporized alcohol
4. All burn at the same rate
In chemical reactions, electricity, a spark, and sunlight are all ways in which _______________ may be provided.
1. activation energy
2. reactants
3. products
4. catalysts
For an effective collision to take place, there must be:
1. A sufficiently hard collision
2. A correctly oriented collision
3. A catalyst present
4. No products present
5. High pressure
In this chemical reaction:

2 HCl(aq) + Mg(s) <--> MgCl₂(aq) + H₂(g) + heat
1. energy is given off, so the reaction is endothermic
2. energy is given off, so the reaction is exothermic
3. energy is absorbed, so the reaction is endothermic
4. energy is absorbed, so the reaction is exothermic
Given the following reaction:

P₄(s) + 5 O₂(g) --> 2 P₂O₅(s)

If the intial rate of the reaction consumes 1 mole of phosphorus, P₄, per second, what is the rate at which oxygen, O₂, is consumed initially?
1. 1 mole per second
2. 2 moles per second
3. 0.2 moles per second
4. 5 moles per second
Given the following reaction:

P₄(s) + 5 O₂(g) --> 2 P₂O₅(s)

If the intial rate of the reaction consumes 1 mole of phosphorus, P₄, per second, what is the rate at which diphosphorus pentoxide, P₂O₅, is formed initially?
1. 1 mole per second
2. 2 moles per second
3. 0.2 moles per second
4. 5 moles per second
Given the following reaction:

2 H₂(g) + O₂(g) --> 2 H₂O

As this reaction takes place:
1. the quantity of water vapor, H₂O(g), decreases
2. the quantities of hydrogen, H₂, and oxygen, O₂, decrease
3. the quantities of hydrogen, H₂, and oxygen, O₂, increase
4. the quantity of hydrogen, H₂, increases and the quantity of oxygen, O₂, decreases
When extra NH₃ is added to the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When N₂ is removed from the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When H₂ is added to the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
When the pressure is increased on the following system at equilibrium:

3 H₂(g) + N₂(g) <--> 2 NH₃(g)
1. In order to restore equilibrium, the reaction shifts right, toward products
2. In order to restore equilibrium, the reaction shifts left, toward reactants
3. No change occurs
Seven scientists you learned about this year were (OK, its not on the test!)
1. Sleepy, Dopey, Doc, Grumpy, Bashful, Sneezy, and Happy
2. Dalton, LeChatelier, Charles, Avogadro, Rutherford, Boyle and Einstein
3. Huey, Dewey, Luey, Manny, Moe, Jack, and Mr. Allan
4. Aurora, Cinderella, Mulan, Ariel, Snow White, Jasmin and Giselle

Indicator	Results
Phenolphthalein	Clear
Red litmus	Remains red
Blue litmus	Turns red
Methyl orange	Turns deep red