WorksheetsChemistry Sem 2 Review
Total questions: 64
Worksheet time: 32mins
What might happen that indicates a chemical reaction is happening?
The temperature changes
A gas is formed
The mass of the reactants increases
The color of the substance changes
How does balancing chemical equations relate to the Law of Conservation of Mass?
It ensures the number of atoms is the same on both sides of the equation
It increases the mass of the products
It changes the type of elements present
It allows for the creation of new atoms
What is oxidation?
Gain of electrons
Loss of electrons
Formation of a precipitate
Increase in temperature
What is reduction?
Loss of electrons
Gain of electrons
Formation of a gas
Decrease in temperature
Which of the following is NOT one of the general types of chemical reactions?
Synthesis
Decomposition
Combustion
Evaporation
How can the activity series for metals be used in predicting chemical reactions?
It tells you the color of the products
It helps determine if a metal will react with a given substance
It shows the melting points of metals
It lists the boiling points of metals
In a redox reaction, what is the oxidizing agent?
The substance that loses electrons
The substance that gains electrons
The substance that forms a precipitate
The substance that changes color
What does theoretical yield tell you in a chemical reaction?
The actual amount of product formed
The maximum amount of product that could be formed
The amount of reactant left over
The percent of reactant used
What is temperature, and how is it related to internal energy?
Temperature is a measure of the average kinetic energy of particles and is related to internal energy as a component of it.
Temperature is the total energy of a system and is unrelated to internal energy.
Temperature is the amount of heat transferred and is not related to internal energy.
Temperature is the pressure exerted by a gas and is not connected to internal energy.
What does the Maxwell-Boltzmann distribution tell us about the particles in a gas?
It shows the distribution of speeds among particles in a gas.
It describes the color of gases.
It explains the chemical composition of gases.
It measures the volume of a gas.
Which of the following is NOT a characteristic of the Kinetic-Molecular Theory of Gases?
Gas particles are in constant, random motion.
Gas particles have significant attractive forces between them.
The volume of gas particles is negligible compared to the container.
Collisions between gas particles are elastic.
Which of the following best describes an ideal gas?
A gas that follows the gas laws under all conditions of temperature and pressure.
A gas that only exists at absolute zero.
A gas that cannot be compressed.
A gas that is always visible.
How does a barometer work?
It measures atmospheric pressure by balancing the weight of mercury in a column against atmospheric pressure.
It measures temperature by expanding liquid.
It measures humidity by absorbing water vapor.
It measures wind speed using rotating cups.
What is the standard unit for pressure in a gas?
Pascal (Pa)
Joule (J)
Kelvin (K)
Newton (N)
What causes gases to increase in pressure?
Increasing the temperature or decreasing the volume.
Decreasing the temperature or increasing the volume.
Adding more liquid to the container.
Removing gas particles from the container.
Which of the following lists the four basic states of matter?
Solid, liquid, gas, plasma
Water, air, fire, earth
Metal, nonmetal, metalloid, noble gas
Ice, steam, vapor, mist
What is diffusion?
The movement of particles from an area of high concentration to an area of low concentration.
The process of water boiling.
The condensation of gas into a liquid.
The separation of mixtures by filtration.
What information can you obtain from a P-T (Pressure-Temperature) diagram?
The phase of a substance at different pressures and temperatures.
The color of a substance.
The mass of a substance.
The electrical conductivity of a substance.
What is the triple point in a phase diagram?
The temperature at which a substance boils
The point where solid, liquid, and gas phases coexist in equilibrium
The pressure at which a gas condenses into a liquid
The temperature at which a solid melts
What is the critical point in the context of phase changes?
The temperature and pressure at which a substance can exist as a solid
The highest temperature and pressure at which a liquid and its vapor can coexist
The point where a solid turns directly into a gas
The lowest temperature at which a liquid can exist
Which of the following is an example of evaporative cooling?
Ice melting in a glass of water
Water boiling on a stove
Sweat evaporating from your skin and cooling you down
Condensation forming on a cold glass
What is vapor pressure?
The pressure exerted by a vapor in equilibrium with its liquid at a given temperature
The pressure required to freeze a liquid
The pressure at which a solid melts
The pressure of a gas at absolute zero
Which of the following best describes Boyle’s Law?
The pressure of a gas is inversely proportional to its volume at constant temperature.
The volume of a gas is directly proportional to its temperature at constant pressure.
The number of moles of a gas is directly proportional to its volume at constant temperature and pressure.
The pressure of a gas is directly proportional to its temperature at constant volume.
According to Charles’ Law, which quantity remains constant?
Pressure
Volume
Temperature
Number of moles
Avogadro’s Law relates which two quantities?
Volume and number of moles
Pressure and temperature
Volume and pressure
Temperature and number of moles
What does STP stand for in chemistry?
Standard Temperature and Pressure
Standard Time and Pressure
Standard Temperature and Power
Standard Test Procedure
Which equation represents the ideal gas law?
PV = nRT
P = k/V
V = kT
P = nVT/R
When does the ideal gas law best apply?
At high temperature and low pressure
At low temperature and high pressure
At all temperatures and pressures
Only at STP
What are absolute units in the context of gas laws?
Units that start from zero, such as Kelvin for temperature and Pascals for pressure
Units that can be negative, such as Celsius for temperature
Units used only in the metric system
Units used only in the imperial system
How do you obtain absolute pressure from gauge pressure?
Add atmospheric pressure to gauge pressure
Subtract atmospheric pressure from gauge pressure
Multiply gauge pressure by atmospheric pressure
Divide gauge pressure by atmospheric pressure
What is the law of partial pressures?
The total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.
The pressure of a gas is inversely proportional to its volume.
The pressure of a gas is directly proportional to its temperature.
The total pressure of a mixture of gases is equal to the product of the partial pressures.
What is a mole fraction?
The ratio of the number of moles of a component to the total number of moles in a mixture
The number of moles in one liter of solution
The number of moles in one gram of substance
The ratio of the mass of a component to the total mass of the mixture
What is effusion?
The process by which gas particles pass through a tiny opening.
The process of a liquid turning into a gas.
The process of a gas mixing with another gas.
The process of a solid dissolving in a liquid.
What is dissociation?
The process where molecules combine to form a compound
The process where a compound breaks into ions in solution
The process of heating a substance
The process of cooling a substance
What are the solute and solvent?
Solute is the liquid, solvent is the solid
Solute is the substance being dissolved, solvent is the substance doing the dissolving
Solute is always water, solvent is always salt
Solute and solvent are both gases
What is hydration? Describe the process.
The process of removing water from a compound
The process of adding heat to a solution
The process where water molecules surround and interact with ions or molecules
The process of freezing water
What is the difference between endothermic and exothermic processes?
Endothermic absorbs heat, exothermic releases heat
Endothermic releases heat, exothermic absorbs heat
Both absorb heat
Both release heat
What is the heat of solution? What does this value tell us about a reaction?
The amount of light produced in a reaction
The amount of heat absorbed or released when a solute dissolves in a solvent
The amount of gas produced in a reaction
The amount of pressure in a solution
What is entropy?
The measure of energy in a system
The measure of disorder or randomness in a system
The measure of temperature in a system
The measure of mass in a system
In nature, what generally happens to energy? What happens to entropy? Do they increase or decrease?
Energy and entropy both decrease
Energy increases, entropy decreases
Energy decreases, entropy increases
Both energy and entropy increase
What does the Gibbs free energy value represent?
The total mass of a system
The amount of usable energy available to do work
The temperature of a system
The volume of a solution
What is an electrolyte? What differentiates a weak from strong electrolyte?
A substance that does not conduct electricity; strong electrolytes conduct less
A substance that conducts electricity in solution; strong electrolytes dissociate completely, weak electrolytes do not
A substance that only exists as a solid
A substance that only exists as a gas
What is a saturated solution? How is this an example of chemical equilibrium?
A solution that can dissolve more solute; it is not at equilibrium
A solution that cannot dissolve more solute; the rate of dissolving equals the rate of crystallization
A solution with no solute
A solution with only solvent
What does the saying, "like dissolves like" mean?
Only solids dissolve in liquids
Polar substances dissolve polar substances, nonpolar dissolve nonpolar
All substances dissolve in water
Only gases dissolve in liquids
What does it mean for something to be volatile?
It is very stable
It evaporates easily
It is always a solid
It does not react with anything
What do we call the process of making soap?
Fermentation
Saponification
Distillation
Sublimation
What affects the solubility of gases in liquids?
Temperature and pressure
Color and odor
Volume and mass
Shape and size
What is the difference between molarity and molality? What do they measure?
Molarity measures moles of solute per liter of solution, while molality measures moles of solute per kilogram of solvent.
Molarity measures grams of solute per liter of solution, while molality measures grams of solute per kilogram of solvent.
Molarity measures moles of solute per kilogram of solvent, while molality measures moles of solute per liter of solution.
Molarity and molality are the same and measure the same thing.
What is a precipitate?
A solid that forms and settles out of a liquid mixture
A gas that forms in a reaction
A liquid that evaporates quickly
A solution that conducts electricity
What is a spectator ion?
An ion that does not participate in the chemical reaction
An ion that forms a precipitate
An ion that changes color during the reaction
An ion that increases the temperature of the solution
What is a colligative property?
A property that depends on the number of solute particles, not their identity
A property that depends on the color of the solution
A property that depends on the type of solvent used
A property that depends on the temperature only
Why does vapor pressure lower if you add a nonvolatile solute to a solution?
The nonvolatile solute decreases the number of solvent molecules at the surface, reducing evaporation.
The nonvolatile solute increases the temperature of the solution.
The nonvolatile solute reacts with the solvent to form a gas.
The nonvolatile solute increases the vapor pressure.
Which of the following is a property of acids?
They taste sour
They feel slippery
They turn red litmus paper blue
They are always solid at room temperature
According to Arrhenius’ theory, what defines an acid?
A substance that increases the concentration of H3O+ ions in water
A substance that donates an electron pair
A substance that increases the concentration of OH- ions in water
A substance that accepts a proton
According to Brønsted-Lowry theory, what is a base?
A substance that donates a proton
A substance that accepts a proton
A substance that donates an electron pair
A substance that increases H+ concentration in water
What does Lewis’ theory say about acids and bases?
Acids donate protons, bases accept protons
Acids accept electron pairs, bases donate electron pairs
Acids increase H+ concentration, bases increase OH- concentration
Acids are always liquids, bases are always solids
What determines if an acid or base is weak or strong?
The color of the solution
The degree of ionization in water
The temperature of the solution
The mass of the acid or base
Why do oxyacids become stronger acids as they have more oxygen atoms?
More oxygen atoms increase the polarity of the O-H bond, making it easier to lose H+
More oxygen atoms make the acid less soluble
More oxygen atoms decrease the acidity
More oxygen atoms make the acid taste sweeter
What is the pH scale used for?
To measure the temperature of a solution
To measure the concentration of hydrogen ions in a solution
To measure the mass of a solution
To measure the color of a solution
If the pH of a solution is 3, what can you say about the solution?
It is strongly acidic
It is neutral
It is strongly basic
It is a solid
Given the pOH of a solution is 4, what is the pH?
10
7
4
14
What is the difference between the endpoint and the equivalence point in a titration?
The endpoint is when the indicator changes color; the equivalence point is when stoichiometric amounts of acid and base have reacted
The endpoint is when all acid is neutralized; the equivalence point is when the solution is neutral
The endpoint is when the solution turns blue; the equivalence point is when the solution turns red
There is no difference
What does a pH indicator do?
Changes color depending on the pH of the solution
Measures temperature
Increases the acidity of a solution
Neutralizes the solution
Which of the following is a main point of the titration process?
Adding a solution of known concentration to a solution of unknown concentration until the reaction is complete
Heating the solution until it boils
Freezing the solution
Mixing two solids together
