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WorksheetsChapter 6 - Pressure
Total questions: 69
Worksheet time: 35mins
Pressure is defined as:
The force applied per unit area
The amount of mass in a given volume
The energy possessed by an object
The rate of change of velocity
A molecule exerts pressure by:
colliding with the walls of the container
absorbing energy from the surroundings
changing its shape
losing mass
The concentration of gas molecules affects pressure in which of the following ways?
Higher concentration increases pressure.
Higher concentration decreases pressure.
Concentration has no effect on pressure.
Pressure only changes with temperature.
Altitude affects pressure in which of the following ways?
Pressure increases with altitude
Pressure decreases with altitude
Pressure remains constant with altitude
Pressure fluctuates randomly with altitude
Things allowable because of pressure are:
Walking on snow with snowshoes
Drinking juice with a straw
Writing with a pen
All of the above
The basic formula for pressure is:
Force/Area
Mass/Volume
Distance/Time
Work/Force
You might feel pain in your ears due to pressure change because:
The pressure inside and outside the ear becomes unequal
The temperature in the ear drops suddenly
The ear produces more wax
The ear drum gets stronger
Barometer is used to measure:
Temperature
Pressure
Humidity
Speed
Manometer is defined as:
A device used to measure pressure
A device used to measure temperature
A device used to measure speed
A device used to measure mass
Pressure changes affect the reading of a manometer in which of the following ways?
The reading increases with increasing pressure difference.
The reading decreases with increasing pressure difference.
The reading remains constant regardless of pressure changes.
The reading fluctuates randomly with pressure changes.
Blood pressure is measured in the body using which of the following methods?
Using a thermometer
Using a sphygmomanometer
Using a stethoscope
Using an otoscope
Blood pressure measurements indicate:
The force of blood against artery walls
The amount of oxygen in the blood
The number of red blood cells
The rate of breathing
What can happen if blood pressure is too high?
It can cause damage to organs.
It can improve digestion.
It can lower heart rate.
It can increase energy levels.
List the four basic properties of a gas sample with their abbreviations:
The four basic properties of a gas sample are: Pressure (P), Volume (V), Temperature (T), and Amount in moles (n).
The four basic properties of a gas sample are: Pressure (P), Density (D), Temperature (T), and Mass (m).
The four basic properties of a gas sample are: Pressure (P), Volume (V), Concentration (C), and Amount in grams (g).
The four basic properties of a gas sample are: Pressure (P), Volume (V), Temperature (T), and Density (D).
The simple gas laws do which of the following?
Describe the relationships between pressure, volume, and temperature of gases.
Explain the structure of atoms.
Predict the color of gases.
Determine the mass of solids.
Boyle’s Law states that, at constant temperature, the pressure and volume of a gas are inversely proportional. Which of the following is the correct working formula for Boyle’s Law?
P1V1 = P2V2
P1/T1 = P2/T2
V1/T1 = V2/T2
P1V1/T1 = P2V2/T2
Which of the following curves best represents the effect of Boyle’s Law on a graph of V vs P?
A straight line with positive slope
A straight line with negative slope
A hyperbolic curve
A parabolic curve
Boyle’s Law follows what you have learned about collisions and gases because:
As volume decreases, gas particles collide more frequently, increasing pressure.
As volume increases, gas particles move slower, decreasing pressure.
As temperature increases, gas particles stop colliding.
As pressure increases, the number of gas particles decreases.
Boyle’s Law affects scuba divers by:
Increasing the pressure as they ascend
Decreasing the volume of air in their tanks as they descend
Causing the volume of air in their lungs to decrease as they descend
Having no effect on the air in their bodies
Charles’s Law states that, at constant pressure, the volume of a gas is directly proportional to its absolute temperature. Which of the following is the correct formula for Charles’s Law?
V₁/T₁ = V₂/T₂
P₁V₁ = P₂V₂
PV = nRT
P₁/T₁ = P₂/T₂
Which of the following graphs best represents V vs T according to Charles Law?
A straight line passing through the origin
A parabola opening upwards
A horizontal line
A straight line not passing through the origin
The relationship between volume and temperature of gases is:
Directly proportional
Inversely proportional
No relationship
Constant
What happens when the V vs T line is extrapolated from the lowest measured temperature?
The line meets the temperature axis at absolute zero.
The line becomes parallel to the temperature axis.
The line curves upwards.
The line does not intersect any axis.
What assumption is always made in Charles Law?
The pressure is constant
The temperature is constant
The volume is constant
The amount of gas is constant
Charles Law describes the relationship between gas molecules and their collisions as:
The volume of a gas increases as temperature increases due to more frequent and energetic collisions.
The pressure of a gas decreases as temperature increases due to fewer collisions.
The number of gas molecules remains constant regardless of temperature changes.
The collisions of gas molecules decrease as temperature increases.
The second floor of a home is usually warmer than the first floor because:
Heat rises to higher levels.
The second floor has more windows.
The first floor is closer to the basement.
The second floor is smaller.
Charles Law explains hot air ballooning by stating that:
The volume of air increases as it is heated, causing the balloon to rise.
The pressure inside the balloon decreases as it is heated, causing it to fall.
The mass of the balloon increases as it is heated, causing it to sink.
The temperature of the air decreases as it is heated, causing the balloon to rise.
The general equation for Charles Law is:
V1/T1 = V2/T2
P1V1 = P2V2
PV = nRT
V = kP
Avogadro’s Law states that:
Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules.
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 rate of diffusion of a gas is inversely proportional to the square root of its molar mass.
Which of the following graphs best represents the curve of V vs # of moles according to Avogadro’s Law?
A straight line passing through the origin
A parabola opening upwards
A horizontal line
A curve increasing exponentially
To exhibit Avogadro’s Law, what must remain constant?
Temperature and pressure
Volume and temperature
Pressure and volume
Amount of gas and pressure
The relationships between the primary properties of gases are described by:
Boyle's Law, Charles's Law, and the Ideal Gas Law
Newton's Laws of Motion
Ohm's Law and Faraday's Law
Archimedes' Principle
The Ideal Gas Law can be defined as which of the following?
A law that relates the pressure, volume, temperature, and number of moles of an ideal gas, expressed as PV = nRT.
A law that states energy cannot be created or destroyed.
A law that describes the behavior of solids under pressure.
A law that explains the conservation of mass.
Section 6.4 - The Ideal Gas Law
Which of the following is a working formula for calculations resulting from its use?
PV = nRT
P = F/A
V = IR
E=mc2
The ideal gas constant R is:
8.314 J/(mol·K)
0.0821 L·atm/(mol·K)
1.00 J/(mol·K)
6.022 × 10²³ J/(mol·K)
The Ideal Gas Law incorporates all three of the simple gas laws by:
Combining Boyle's, Charles's, and Avogadro's laws into one equation
Ignoring the effects of temperature and pressure
Only applying to solids and liquids
Separating the laws into different equations
Molar volume (of a gas) is defined as:
The volume occupied by one mole of a gas at standard temperature and pressure
The mass of one mole of a gas at standard temperature and pressure
The pressure exerted by one mole of a gas at standard temperature and pressure
The temperature at which one mole of a gas occupies one liter
STP is defined as:
Standard Temperature and Pressure
Standard Time and Pressure
Standard Temperature and Power
Standard Test Procedure
The molar volume of an ideal gas is useful because:
It allows calculation of the volume occupied by one mole of gas at standard temperature and pressure.
It determines the color of the gas.
It measures the mass of the gas.
It predicts the solubility of the gas in water.
The formula for the density of a gas is:
d = m/V, where d is density (g/L), m is mass (g), and V is volume (L)
d = PV/nRT, where d is density (g/L), P is pressure (atm), V is volume (L), n is moles, R is gas constant, and T is temperature (K)
d = nRT/P, where d is density (g/L), n is moles, R is gas constant, T is temperature (K), and P is pressure (atm)
d = V/m, where d is density (g/L), V is volume (L), and m is mass (g)
The molar volume of a gas at STP is:
22.4 L
1.0 L
0.0821 L
273 L
Density is related to molar mass by which of the following equations?
Density = Molar mass / Volume
Density = Molar mass × Volume
Density = Volume / Molar mass
Density = Molar mass + Volume
The Ideal Gas Equation can be adapted to include density by expressing it as:
PV = nRT
P = ρRT/M
V = nRT/P
P = RT/ρ
The molar mass of a gas can be calculated using:
Boyle's Law
Avogadro's Law
Ideal Gas Equation
Dalton's Law
The composition of dry air is:
78% nitrogen, 21% oxygen, 1% other gases
50% nitrogen, 30% oxygen, 20% other gases
60% oxygen, 30% nitrogen, 10% other gases
90% oxygen, 5% nitrogen, 5% other gases
Ideal gases in mixtures behave according to which law?
Boyle's Law
Dalton's Law of Partial Pressures
Charles's Law
Avogadro's Law
Partial Pressure is defined as:
The pressure exerted by an individual gas in a mixture of gases
The total pressure of a gas mixture
The volume occupied by a gas in a mixture
The temperature of a gas in a mixture
The relationship between partial pressure and moles of a mixture of gases is:
Directly proportional
Inversely proportional
No relationship
Depends on temperature only
The mole fraction is:
the ratio of the number of moles of a component to the total number of moles in the mixture
the mass of solute per liter of solution
the number of particles in one mole of substance
the volume of solute per volume of solution
At what partial pressure of oxygen do we breathe?
0.21 atm (atmospheric pressure at sea level).
0.78 atm (partial pressure of nitrogen).
1.00 atm (total atmospheric pressure).
0.03 atm (partial pressure of carbon dioxide).
What happens to the partial pressure of Oxygen at high altitudes?
The partial pressure of oxygen decreases at high altitudes.
The partial pressure of oxygen increases at high altitudes.
The partial pressure of oxygen remains the same at high altitudes.
The partial pressure of oxygen fluctuates randomly at high altitudes.
Define: Hypoxia
Hypoxia is a condition in which there is a deficiency of oxygen in the tissues.
Hypoxia is a condition in which there is an excess of carbon dioxide in the tissues.
Hypoxia is a condition in which there is a deficiency of glucose in the blood.
Hypoxia is a condition in which there is an excess of oxygen in the tissues.
Oxygen toxicity
Oxygen toxicity is a condition resulting from the harmful effects of breathing molecular oxygen at increased partial pressures.
Oxygen toxicity is a deficiency of oxygen in the blood leading to hypoxia.
Oxygen toxicity is a genetic disorder affecting the hemoglobin structure.
Oxygen toxicity is a condition caused by the lack of oxygen in the environment.
What is nitrogen narcosis?
Nitrogen narcosis is a reversible alteration in consciousness that occurs while diving at depth, caused by the anesthetic effect of nitrogen under high pressure.
Nitrogen narcosis is a condition caused by lack of oxygen at high altitudes.
Nitrogen narcosis is a skin disorder resulting from exposure to nitrogen-based chemicals.
Nitrogen narcosis is a type of food poisoning caused by consuming nitrogen-rich foods.
Which of the following is a necessary precaution one must take with deep-sea diving?
Ignoring decompression stops
Ascending slowly to avoid decompression sickness
Holding your breath while ascending
Diving alone without a buddy
Define: Vapor pressure
Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid (or solid) phase at a given temperature.
Vapor pressure is the pressure exerted by a solid in equilibrium with its gaseous phase at any temperature.
Vapor pressure is the pressure exerted by a liquid in equilibrium with its solid phase at low temperature.
Vapor pressure is the pressure exerted by a vapor in equilibrium with its solid phase at high pressure.
What must one account for when collecting a gas over water?
One must account for the vapor pressure of water when collecting a gas over water.
One must account for the color of the gas when collecting a gas over water.
One must account for the density of the container when collecting a gas over water.
One must account for the temperature of the room when collecting a gas over water.
Stoichiometric relationships are applied when calculating with gaseous reactants or products by:
Using the ideal gas law to relate moles, volume, and temperature.
Ignoring the volume of gases in calculations.
Assuming all gases have the same density.
Only considering solid reactants.
The volume of 1 mole of an ideal gas at STP is:
22.4 L
1.0 L
0.0821 L
273 L
List the basic assumptions for the Kinetic Molecular Theory:
1. Gases consist of a large number of particles that are in constant, random motion. 2. The volume of the individual gas particles is negligible compared to the total volume of the gas. 3. Collisions between gas particles and with the walls of the container are perfectly elastic.
1. Gases are made up of particles that are stationary and do not move. 2. The volume of gas particles is significant compared to the total volume of the gas. 3. Collisions between gas particles are inelastic and energy is lost.
1. Gases consist of a small number of particles that move in a fixed pattern. 2. The volume of the gas particles is equal to the total volume of the gas. 3. Collisions between gas particles do not occur.
1. Gases consist of particles that attract each other strongly. 2. The volume of the individual gas particles is greater than the total volume of the gas. 3. Collisions between gas particles result in the particles sticking together.
The difference between an elastic and an inelastic collision is:
Elastic collisions conserve both kinetic energy and momentum, while inelastic collisions conserve only momentum.
Elastic collisions conserve only momentum, while inelastic collisions conserve both kinetic energy and momentum.
Both types of collisions conserve only kinetic energy.
Neither type of collision conserves momentum or kinetic energy.
The Kinetic Molecular Theory (KMT) explains pressure (P) and the simple Gas Laws by:
Describing gas particles as having strong intermolecular forces.
Stating that gas particles are in constant, random motion and collide with container walls, causing pressure.
Explaining that gas particles are stationary and do not interact with the container.
Suggesting that gas particles lose energy with every collision.
According to the Kinetic Molecular Theory (KMT), a gas is:
A substance with a definite shape and volume
A substance with a definite volume but no definite shape
A substance with neither definite shape nor definite volume
A substance that cannot be compressed
Boyle’s Law describes the relationship between pressure and volume of a gas according to the KMT. Which of the following best explains this relationship?
As volume decreases, pressure increases due to more frequent collisions of gas particles.
As volume decreases, pressure decreases because particles move slower.
As volume increases, pressure increases due to more space for particles to move.
Pressure and volume are not related according to the KMT.
Charles’s Law describes the relationship between which two variables according to the KMT?
Pressure and volume
Temperature and volume
Pressure and temperature
Volume and moles
Avogadro’s Law describes the relationship between the number of gas particles and volume according to the KMT. Which of the following best explains this relationship?
As the number of gas particles increases, the volume increases at constant temperature and pressure.
As the number of gas particles increases, the volume decreases at constant temperature and pressure.
As the number of gas particles increases, the pressure decreases at constant volume and temperature.
As the number of gas particles increases, the temperature decreases at constant volume and pressure.
Dalton’s Law can be explained by the KMT because:
Gas particles do not attract or repel each other, so each gas in a mixture exerts its own pressure independently.
Gas particles are in constant random motion, causing pressure to increase with temperature.
The volume of gas particles is negligible compared to the container, so total pressure is always constant.
Gas particles lose energy during collisions, affecting the total pressure.
KMT and the Ideal Gas Law: The KMT explains the behavior of gases described by the Ideal Gas Law by relating gas particle motion to pressure, volume, and temperature. Which of the following best describes this relationship?
KMT describes how gas particles' motion and collisions result in the pressure, volume, and temperature relationships in the Ideal Gas Law.
KMT only applies to solids and liquids, not gases.
The Ideal Gas Law contradicts the KMT.
KMT explains chemical reactions, not gas behavior.
KMT relates temperature and molecular velocities by stating that:
Temperature is directly proportional to the average kinetic energy of molecules, which depends on their velocities.
Temperature is inversely proportional to the average kinetic energy of molecules.
Molecular velocities are independent of temperature.
KMT does not relate temperature and molecular velocities.
