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Example Questions
Example Question #1 : Phase Changes
What amount of heat must be added to a 20-gram sample of ice in order to raise the temperature from to
?
This question requires three steps:
1. We need to raise the temperature of the ice from to
degrees Celsius.
2. We need to melt the ice.
3. We need to raise the temperature of the water from to
degrees Celsius.
Steps one and three can use the equation:
Step 2 requires the enthalpy of fusion to be multiplied by the mass of the water sample.
Finding these three added heats will give us the total amount of heat needed to raise the temperature from to
.
Example Question #1 : Phase Diagrams
What is the process of converting a solid directly to a gas?
Freezing
Sublimation
Deposition
Condensation
Sublimation
Certain substances, such as carbon dioxide, are able to skip the liquid phase and go from a solid to a gas under standard conditions. This process is called sublimation.
Example Question #1 : Heat Capacity And Specific Heat
What is the specific heat capacity for a 50-gram sample of metal that increases in temperature by 10 degrees celsius when 2000 joules of energy is added?
Use the equation:
We can calculate the specific heat capacity for the unknown metal. Since we know the added heat , the mass of the sample
, and the change in temperature
, we can solve for
.
Example Question #1 : Heat Capacity And Specific Heat
A sample of an unknown metal at
is immersed in water and is allowed to reach equilibrium. If final temperature of the system is
and
of energy are released, what is the identity of the metal?
It is impossible to determine
Recall that the formula for specific heat is . Rearranging the equation for specific heat (c) yields
Remark: keep in mind that the release of energy and the cooling of the metal will give negative values for both and
.
Example Question #1 : Thermochemistry
The heat capacity of a bomb calorimeter assembly is . What is the heat of combustion of
of sucrose in a bomb calorimeter that results in the temperature rising from
to
?
A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as , is the negative of the thermal energy gained by the calorimeter:
The heat capacity of a calorimeter is:
Plugging the values given into the equation gives:
Using the relation provided earlier:
Because we are dealing with 1.1 grams of sucrose, the heat of combustion of sucrose is:
Example Question #21 : Thermochemistry And Thermodynamics
The heat capacity of a bomb calorimeter assembly is . What is the heat of combustion of
of caffeine in a bomb calorimeter that results in the temperature rising from
to
?
A bomb calorimeter is a device used to measure the quantity of heat change for a process. The heat of a reaction which is denoted as q, is the negative of the thermal energy gained by the calorimeter:
The heat capacity of a calorimeter is:
Plugging the values given into the equation gives:
Using the relation provided earlier:
Because we are dealing with 1.65 grams of sucrose, the heat of combustion of sucrose is:
Example Question #1 : Thermochemistry
Which of the following are endothermic?
Condensation
Melting
More than one of these are endothermic processes
Freezing
Melting
Endothermic processes involve a positive change in enthalpy. This means that the enthalpy of products is higher than the enthalpy of reactants and net heat energy is consumed. Phase changes that involve increasing the distance between particles (meaning conversion of solid to liquid (melting), liquid to gas (evaporation) and solid to gas (sublimation)) require an input of energy and are considered endothermic processes. On the other hand, phase changes that decrease the distance between particles (such as gas to liquid (condensation), liquid to solid (freezing), and gas to solid (deposition)) release energy and are considered exothermic processes.
Example Question #1 : Endothermic And Exothermic Reactions
Which of the following is true regarding an exothermic reaction?
I. Entropy always increases
II. It is always spontaneous
III. It can facilitate other energy-consuming reactions
I and III
I and II
III only
II only
III only
Exothermic reactions involve release of heat energy. This means that the energy of the products is lower than the energy of the reactants. Entropy is the measure of disorder in a system. It does not depend on the enthalpy and can increase or decrease during an exothermic process. Spontaneity is determined by looking at the change in Gibbs free energy, . Negative
corresponds to a spontaneous process and positive
corresponds to a nonspontaneous process. While the equation for Gibbs free energy,
, involves change in enthalpy, the spontaneity also depends on temperature and change in entropy. Exothermic reactions release energy in the form of heat. This heat energy can be used to power other processes that require energy; therefore, exothermic reactions can facilitate active processes that consume energy.
Example Question #2 : Thermochemistry
In an __________ reaction, the products are more stable than the reactants; in an __________ reaction the reactants are more stable than the products.
endergonic . . . exergonic
exergonic . . . exergonic
exergonic . . . endergonic
endergonic . . . endergonic
exergonic . . . endergonic
Exergonic reactions release energy; therefore, the energy of products is lower than that of the reactants. Endergonic reactions consume energy; therefore, the energy of products is greater than that of the reactants. In other words, exergonic reactions are spontaneous, while endergonic reactions are nonspontaneous, and require the net input of energy to drive the reaction.
Example Question #21 : Physical Chemistry
Consider the following spontaneous reaction:
What can you conclude about the enthalpy change in this reaction?
Cannot be determined from the given information
It is negative
It is zero
It is positive
It is negative
We need to use the following equation to answer this question:
Above, is change in Gibbs free energy,
is change in enthalpy,
is temperature, and
is change in entropy. The question states that the reaction is spontaneous; therefore,
is negative. We can also determine the
for this reaction by looking at the phases of the products and reactants. Recall that entropy is a measure of disorder. When it comes to phases, gases have the highest entropy and solids have the lowest entropy. This is because in gases the molecules are spread out and have more room for disorder while solids are compressed and well packaged, decreasing the disorder of the atoms/molecules. Liquids are intermediate in entropy. In this reaction, we are creating a liquid from two molecules of gas; therefore, we are decreasing the entropy of the system (going to a more ordered, liquid state). The change in entropy for this reaction is negative.
Rearranging and solving the equation above for gives us:
Since both and
are negative,
will always be negative (regardless of temperature). This is an exothermic reaction.
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