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Test: ACT Chemistry Research Summaries Questions - ACT MCQ


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10 Questions MCQ Test Science for ACT - Test: ACT Chemistry Research Summaries Questions

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Test: ACT Chemistry Research Summaries Questions - Question 1
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Both gases and liquids are considered to be fluids that have individual molecules that move around with kinetic and potential energy. Kinetic energy, defined as the energy related to motion, takes three forms: translational energy that occurs as a molecule moves from position A to position B, rotational energy that occurs as a molecule spins around an imaginary axis at its center of mass, and vibrational energy that occurs as individual atoms in a molecular bond move towards and away from each other. Usually, molecules possess varying combinations of kinetic energy forms. In contrast, potential energy is defined as stored energy that could be released to become kinetic energy. The total energy of a molecule is fixed, meaning that a molecule has some combination of kinetic and potential energies.

Varying amount of kinetic and potential energies define how molecules in a fluid interact with each other. For example, when the kinetic energy of a molecule is high (greater than 1000J), it can no longer interact with neighboring molecules strongly enough to remain a liquid. However, if the potential energies are too high (greater than 1000 J), molecules cannot escape a liquid to become a gas. If the kinetic energy is high and the potential energy is low, molecules tend to become a gas and can be modeled by an equation known as the Ideal Gas Law:

PV=nRT  

Where P is the pressure of a gas, V is the volume, n is the number of moles of a gas, R is a constant, and T is temperature in degrees Kelvin.

The Ideal Gas Law perfectly applies to particles with no mass, no intermolecular interactions, and no true volume. However, real molecules do not adhere perfectly to the Ideal Gas Law.

Q. As the potential energy of a molecule decreases, one would expect the kinetic energy to:

Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 1

Using the last few sentences of the first paragraph as a guide, we can see that the total energy of a molecule is fixed and contains a fixed combination of kinetic and potential energies. Thus, we can relate the combination to the total by the following formula: ET = EK + EP. Thus, if the potential energy decreases, the kinetic energy must increase in order to keep the total energy of the molecule constant.

Test: ACT Chemistry Research Summaries Questions - Question 2
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Both gases and liquids are considered to be fluids that have individual molecules that move around with kinetic and potential energy. Kinetic energy, defined as the energy related to motion, takes three forms: translational energy that occurs as a molecule moves from position A to position B, rotational energy that occurs as a molecule spins around an imaginary axis at its center of mass, and vibrational energy that occurs as individual atoms in a molecular bond move towards and away from each other. Usually, molecules possess varying combinations of kinetic energy forms. In contrast, potential energy is defined as stored energy that could be released to become kinetic energy. The total energy of a molecule is fixed, meaning that a molecule has some combination of kinetic and potential energies.

Varying amount of kinetic and potential energies define how molecules in a fluid interact with each other. For example, when the kinetic energy of a molecule is high (greater than 1000J), it can no longer interact with neighboring molecules strongly enough to remain a liquid. However, if the potential energies are too high (greater than 1000 J), molecules cannot escape a liquid to become a gas. If the kinetic energy is high and the potential energy is low, molecules tend to become a gas and can be modeled by an equation known as the Ideal Gas Law:

PV=nRT  

Where P is the pressure of a gas, V is the volume, n is the number of moles of a gas, R is a constant, and T is temperature in degrees Kelvin.

The Ideal Gas Law perfectly applies to particles with no mass, no intermolecular interactions, and no true volume. However, real molecules do not adhere perfectly to the Ideal Gas Law.

Q. The relationship between total energy, kinetic energy, and potential energy could best be described as:

Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 2

The end of the first paragraph helps us answer this question. We are told that a molecule contains a fixed amount of total energy and that some combination of kinetic and potential energy combines to create this sum total. Thus, the relationship that best depicts how the various forms of energy relate is ET = EK + EP.

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Test: ACT Chemistry Research Summaries Questions - Question 3
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Both gases and liquids are considered to be fluids that have individual molecules that move around with kinetic and potential energy. Kinetic energy, defined as the energy related to motion, takes three forms: translational energy that occurs as a molecule moves from position A to position B, rotational energy that occurs as a molecule spins around an imaginary axis at its center of mass, and vibrational energy that occurs as individual atoms in a molecular bond move towards and away from each other. Usually, molecules possess varying combinations of kinetic energy forms. In contrast, potential energy is defined as stored energy that could be released to become kinetic energy. The total energy of a molecule is fixed, meaning that a molecule has some combination of kinetic and potential energies.

Varying amount of kinetic and potential energies define how molecules in a fluid interact with each other. For example, when the kinetic energy of a molecule is high (greater than 1000J), it can no longer interact with neighboring molecules strongly enough to remain a liquid. However, if the potential energies are too high (greater than 1000 J), molecules cannot escape a liquid to become a gas. If the kinetic energy is high and the potential energy is low, molecules tend to become a gas and can be modeled by an equation known as the Ideal Gas Law:

PV=nRT  

Where P is the pressure of a gas, V is the volume, n is the number of moles of a gas, R is a constant, and T is temperature in degrees Kelvin.

The Ideal Gas Law perfectly applies to particles with no mass, no intermolecular interactions, and no true volume. However, real molecules do not adhere perfectly to the Ideal Gas Law.

Q. In an oxygen molecule, O2, the two oxygen atoms oscillate about a fixed central point. Which form of kinetic energy is best described here?

Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 3

In the first paragraph, the passage tells us that individual atoms in a bond that move towards and away from each other constitute vibrational energy. Based on the question, the two oxygen atoms oscillate around the central point (the mid-point of their bond). Thus, this is vibrational energy.

Test: ACT Chemistry Research Summaries Questions - Question 4
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Both gases and liquids are considered to be fluids that have individual molecules that move around with kinetic and potential energy. Kinetic energy, defined as the energy related to motion, takes three forms: translational energy that occurs as a molecule moves from position A to position B, rotational energy that occurs as a molecule spins around an imaginary axis at its center of mass, and vibrational energy that occurs as individual atoms in a molecular bond move towards and away from each other. Usually, molecules possess varying combinations of kinetic energy forms. In contrast, potential energy is defined as stored energy that could be released to become kinetic energy. The total energy of a molecule is fixed, meaning that a molecule has some combination of kinetic and potential energies.

Varying amount of kinetic and potential energies define how molecules in a fluid interact with each other. For example, when the kinetic energy of a molecule is high (greater than 1000J), it can no longer interact with neighboring molecules strongly enough to remain a liquid. However, if the potential energies are too high (greater than 1000 J), molecules cannot escape a liquid to become a gas. If the kinetic energy is high and the potential energy is low, molecules tend to become a gas and can be modeled by an equation known as the Ideal Gas Law:

PV=nRT  

Where P is the pressure of a gas, V is the volume, n is the number of moles of a gas, R is a constant, and T is temperature in degrees Kelvin.

The Ideal Gas Law perfectly applies to particles with no mass, no intermolecular interactions, and no true volume. However, real molecules do not adhere perfectly to the Ideal Gas Law.

Q. As the kinetic energy of a molecule increases, one would expect the potential energy to:
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 4

Using the last few sentences of the first paragraph as a guide, we can see that the total energy is fixed. Thus, some combination of kinetic and potential energies makes up the total energy. We can relate how the energies combine with the following formula: ET = EK + EP. Thus, if the kinetic energy increases, the potential energy would have to decrease to keep the sum total the same.

Test: ACT Chemistry Research Summaries Questions - Question 5
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Both gases and liquids are considered to be fluids that have individual molecules that move around with kinetic and potential energy. Kinetic energy, defined as the energy related to motion, takes three forms: translational energy that occurs as a molecule moves from position A to position B, rotational energy that occurs as a molecule spins around an imaginary axis at its center of mass, and vibrational energy that occurs as individual atoms in a molecular bond move towards and away from each other. Usually, molecules possess varying combinations of kinetic energy forms. In contrast, potential energy is defined as stored energy that could be released to become kinetic energy. The total energy of a molecule is fixed, meaning that a molecule has some combination of kinetic and potential energies.

Varying amount of kinetic and potential energies define how molecules in a fluid interact with each other. For example, when the kinetic energy of a molecule is high (greater than 1000J), it can no longer interact with neighboring molecules strongly enough to remain a liquid. However, if the potential energies are too high (greater than 1000 J), molecules cannot escape a liquid to become a gas. If the kinetic energy is high and the potential energy is low, molecules tend to become a gas and can be modeled by an equation known as the Ideal Gas Law:

PV=nRT  

Where P is the pressure of a gas, V is the volume, n is the number of moles of a gas, R is a constant, and T is temperature in degrees Kelvin.

The Ideal Gas Law perfectly applies to particles with no mass, no intermolecular interactions, and no true volume. However, real molecules do not adhere perfectly to the Ideal Gas Law.

Q. An oxygen molecule moving from the left side of a chamber to the right would display what type(s) of kinetic energy?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 5

In the first passage, after describing the different types of kinetic energy, the passage notes that a molecule would likely have varying combinations of kinetic energy. Thus, a molecule moving across the room would display translational, vibrational, and rotational motion.

Test: ACT Chemistry Research Summaries Questions - Question 6
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A student wants to perform an experiment that tests the relationship between the pressure of a gas and the volume it occupies. To perform this experiment, the student places a specific type of gas in a sealed chamber that can change pressure and that can adapt its volume to the gas within it. The chamber also adjusts to the changing pressure such that the temperature (which also has an effect on gas volume) does not change. The following data was obtained:

Q. In Trial 4, the chamber used in the experiment malfunctioned and there was a slight decrease in temperature, leading to a faulty reading of volume for Trial 4. Given this information, what can we say about the relationship between the temperature of a gas and its volume?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 6

This is a tricky question. First we must estimate what the correct reading for Trial 4 should have been to see how the decrease in temperature affected the volume. Using mental math, we can deduce that the volume reading for Trial 4 should have been about 22.4/2.5 or (multiplying both the denominator and numerator by 4) 89.6/10 or essentially 9. Since the actual reading was 8.2 Liters, we know that the decrease in temperature decreased the volume, implying a direct relationship. That is, as one goes up, the other goes up, and vice versa. However our work is not done. Since we do not know by how much the temperature changed, we cannot make a call as to whether the relationship is linear or exponential. Therefore, the correct answer is that it is simply directly related.

Test: ACT Chemistry Research Summaries Questions - Question 7
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A student wants to perform an experiment that tests the relationship between the pressure of a gas and the volume it occupies. To perform this experiment, the student places a specific type of gas in a sealed chamber that can change pressure and that can adapt its volume to the gas within it. The chamber also adjusts to the changing pressure such that the temperature (which also has an effect on gas volume) does not change. The following data was obtained:

Q. In a second experiment, the student tries the same experiment described in the pre-question text and uses a different gas for each trial. If the readings for volume yielded the same results, what could be said about the relationship between type of gas and volume?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 7

The correct answer is that there is no relationship. As type of gas was one of the variables held constant in the first experiment, once the type of gas was no longer held constant, we would expect different results than those that experiment one yielded; however, since the data came out the same, we can safely conclude that there is no observable relationship between type of gas and volume.

Test: ACT Chemistry Research Summaries Questions - Question 8
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Two scientists wanted to test the solubility of different substances. Solubility is a measure of how many moles of a given substance (known as the solute) can dissolve in a given volume of another substance (known as the solvent). The solvent can also be thought of as the substance present in greater amount, while the solute can be seen as the substance present in lesser amount. The scientists performed the following experiments to investigate this property.

Experiment 1

The scientists tested the number of moles of several substances that could be completely dissolved in 50mL of water at various temperatures. They made their solutions by slowly adding amounts of each substance to beakers sitting on a hot plate containing water and a stirring rod until no more of the substance dissolved in the solution. The beakers were weighed before and after the additions and the difference in mass was calculated to be the added mass of the substance. The researchers then calculated the number of moles that dissolved for each trial using the molecular mass and the recorded mass for each trial. Results are recorded in Table 1.

Table 1

Experiment 2

In this experiment, the scientists wanted to test the solubility of NaCl in a variety of liquids at several temperatures. Their procedure was similar to that of Experiment 1, but with a range of liquids and only one solid. The results are compiled in Table 2.

Table 2

Q. Which of the following correctly ranks the solutes from Experiment 1 in decreasing order of solubility in water at 50∘C?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 8

The introduction explains that solubility is a measure of how many moles of a substance can dissolve in a given volume of another substance. This is a very important clue that tells us we need to focus on the "moles added" column rather than the "grams added" column. We need to rank our substances in decreasing order, so we need start with the one with the highest solubility at 50∘C.

The number of moles dissolved at 50∘C are as follows.

NaCl: 0.04004

KNO3: 0.03412

CuSO4: 0.1603

AgCl: 1.6047∗10−5

So the correct order is:

NaCl,KNO3,CuSO4,AgCl

Test: ACT Chemistry Research Summaries Questions - Question 9
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Two scientists wanted to test the solubility of different substances. Solubility is a measure of how many moles of a given substance (known as the solute) can dissolve in a given volume of another substance (known as the solvent). The solvent can also be thought of as the substance present in greater amount, while the solute can be seen as the substance present in lesser amount. The scientists performed the following experiments to investigate this property.

Experiment 1

The scientists tested the number of moles of several substances that could be completely dissolved in 50mL of water at various temperatures. They made their solutions by slowly adding amounts of each substance to beakers sitting on a hot plate containing water and a stirring rod until no more of the substance dissolved in the solution. The beakers were weighed before and after the additions and the difference in mass was calculated to be the added mass of the substance. The researchers then calculated the number of moles that dissolved for each trial using the molecular mass and the recorded mass for each trial. Results are recorded in Table 1.

Table 1

Experiment 2

In this experiment, the scientists wanted to test the solubility of NaCl in a variety of liquids at several temperatures. Their procedure was similar to that of Experiment 1, but with a range of liquids and only one solid. The results are compiled in Table 2.

Table 2

Q. In Experiment 2, which of the following combinations of temperature and solvent dissolved the greatest number of moles of NaCl?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 9

To find the correct answer to this question, we need to look for it in Table 2. We are asked to find the greatest number of moles of  NaCl  that dissolved. Begin by searching in the last column until you find the largest value. Then, look at the temperature and solvent corresponding to that value and see if any answer choices match what you found.

In this case, the largest number of moles dissolved is 0.12029. This corresponds with HCl at 50∘C, which is in fact one of our answer choices.

Test: ACT Chemistry Research Summaries Questions - Question 10
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An experiment was carried out measuring the boiling point and freezing point of an unknown organic liquid (Sample X) with varying levels of salt dissolved within it. The experiment was conducted in the following manner:

First, the experimenter measured the boiling point and freezing point of Sample X. 

Next, a known quantity of salt was dissolved into the sample and then the boiling point and freezing points were measured again. 

The results of the experiment are outlined in the table below:

Q. What can we say is the relationship between concentration of salt in Sample X and the boiling point of Sample X?
Detailed Solution for Test: ACT Chemistry Research Summaries Questions - Question 10

The correct answer is that the boiling point of Sample X is positively and linearly correlated with the concentration of salt dissolved in Sample X. As we can see on the chart provided, every time the experimenter increased the concentration of the salt by 10 mg/L, the boiling point of Sample X increased by 1.4 degrees Celsius. Therefore, we can call this a positive linear correlation.

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