Chem 11.1-11.8
Which pressure is the greatest? 760 psi 760 torr 760 mmHg 760 atm 760 Pa
760 atm
A sample of a gas has a volume of 52 L at a pressure of 1.2 atm. What volume will the gas occupy if the pressure is changed to 0.75 atm? 33 L 48 L 58 L 83 L
83 L
In which phase do the individual particles (atoms or molecules) remain much farther apart and have the ability to move freely? Liquid Gas Solid
Gas
Carefully view the attached images. The can collapses when the air in the container is removed using a vacuum pump because: atmospheric pressure = pressure inside the can atmospheric pressure < pressure inside the can atmospheric pressure > pressure inside the can
atmospheric pressure > pressure inside the can
Phosphorus reacts with H2 according to the balanced equation P4(s) + 6H2(g) → 4PH3(g). What would be the final pressure in a 5.0 L reaction vessel if 6 mol hydrogen gas completely reacts with phosphorus at 298 K? 29 atm 44 atm 4.89 atm 20. atm
20
What volume of gas is generated when 58.0 L of oxygen gas reacts at STP according to the following balanced equation? CH3CH2OH (l) + 3O2 (g) → 2CO2 (g) + 3H2O (l) 48.3 L 58.0 L 220. L 38.7 L
38.7 L
The relationship between the pressure and volume of a gas sample at constant temperature (PV = k) is described by ______ law, while the relationship between the volume and amount of a gas sample at constant temperature and pressure (VnVn = k) is described by ______ law. Boyle's; Avogadro's Avogadro's; Boyle's Boyle's; Charles's Charles's; Avogadro's
Boyle's; Avogadro's
Which molecules are gases at room temperature? HCl NH3 SiO2 CO2
HCl NH3 CO2
Which is the best equation to solve the following problem? At what temperature would a gas sample occupy a volume of 100. L at 1 atm if it originally occupied 75 L at 2 atm and 300. K? PV = nRT P1V1n1T1P1V1n1T1 = P2V2n2T2P2V2n2T2 P1V1T1P1V1T1 = P2V2T2P2V2T2
PV/T=PV/T
How does a gas exert pressure? The weight of the gas particles pressing on each other creates the pressure. The gas particles repel each other, creating pressure. Pressure arises as the gas particles try to avoid contact with each other. The moving gas particles strike each other and the walls of the container, exerting a force.
The moving gas particles strike each other and the walls of the container, exerting a force.
Examine the image and select the statements that correctly describe this molecular depiction. The squiggly arrows pointing toward the interior of the container imply heat is added to the gas. This image is a molecular level description of Charles's law. The volume of the gas is the same in each of the three containers. The number of moles of gas is different in each of the three containers. This image depicts the relationship between P and T at constant n and V. The gas pressure decreases when T increases (heat is added to the system).
The volume of the gas is the same in each of the three containers. This image depicts the relationship between P and T at constant n and V.
When converting a pressure from units of atmosphere (atm) to millimeters of mercury (mmHg), the numeric value will _____. increase stay the same decrease
increase
Fill in the blank question. The gas laws summarize the relationships between the parameters pressure, volume, temperature, and ___________ of a gas.
moles
Which of the following parameters affect the root-mean-squared (rms) speed of a sample of a pure substance in the gas phase? temperature of the sample number of particles in the sample molar mass of the substance pressure of the sample
temperature of the sample molar mass of the substance
Examine the visual of the J-shaped tube containing a gas sample confined by a Hg column. In illustrating Boyle's law, the parameters of this gas sample that remain constant in all three experiments are the____________ and the number of _____________ of the gas.
temperature, moles
A mixture of gases contains 8.00 g of He, 29.96 g of Ar, and 48.00 g of O2. What is the mole fraction of He in this mixture? Multiple choice question. 0.471 47.1 2.00 0.0931
0.471
Calculate the density of NO2 (g) at 50°C and 0.85 atm. 0.128 g/L 1.46 × 10-2 g/L 1.47 g/L 19.0 g/L
1.47 g/L
Which of the following correctly describes an ideal gas? A gas that flows like a liquid A gas that suits a particular application perfectly A gas that is classified as a noble gas A gas that obeys the gas laws under all conditions
A gas that obeys the gas laws under all conditions
The pressure in a gas arises because the particles of a gas strike each other and the walls of their container, exerting a(n) _________. The greater the number of gas particles in a particular volume, the _________ the pressure within the gas. Listen to the complete question
force, greater
Baking soda and vinegar are mixed to form carbon dioxide gas according to the reaction below; the gas is collected at 21oC in an inverted graduated cylinder over water. NaHCO3(s) + HC2H3O2(aq) → CO2(g) + H2O(l) + NaC2H3O2(aq) In order to determine the pressure of CO2 in the cylinder, the vapor pressure of water at 21oC must be ______. subtracted from the measured barometric pressure considered to be the same as the CO2 pressure added to the measured barometric pressure
subtracted from the measured barometric pressure
The abbreviation STP indicates a temperature of _____ and a pressure of _____. 0oC, 1 atm 0oC, 1 torr 0 K, 1 atm 25oC, 1 atm
0oC, 1 atm
Fluorine gas (F2) and chlorine gas (Cl2) combine to form chlorine trifluoride, ClF3. According to Avogadro's law, when 3 volumes of fluorine gas combine with 1 volume of chlorine gas, __________ volume(s) of ClF3 is/are formed at constant T and P.
2
At constant pressure and volume, the density of a gas _____ as the molar mass increases. A gas made of larger particles will have a _____ density than a gas composed of smaller particles under the same conditions of temperature and pressure. decreases; higher increases; lower increases; higher decreases; lower
increases; higher
How is pressure defined mathematically? Area/Force Force × Area Force/Area Force
Force/Area
Which temperature units may be used for gas law calculations? Select all that apply. oC oF K
K
Which of the following factors determine whether a given substance exists as a solid, liquid, or gas? Select all that apply. Pressure Temperature Type of container
Pressure Temperature
Pressure is defined as the ______ exerted per unit of surface ______.
force, area
The root-mean-square (rms) speed of a gas is _____ proportional to the square root of its molar mass. H2 therefore has a _____ rms speed compared to O2 at the same temperature. directly, higher inversely, lower inversely, higher directly, lower
inversely, higher
The pressure exerted by each individual gas in a mixture of gases is called its ________ pressure. This pressure is proportional to the _________ fraction of the gas in the mixture.
partial, mole
The SI unit for pressure is the _____. kilopascal (kPa) pascal (Pa) millimeter of mercury (mmHg) atmosphere (atm)
pascal (Pa)
The density of a gas sample in a balloon is 1.50 g/L at 75°C. What is the density of this gas when the temperature is changed to 25°C at constant pressure? 1.75 g/L 1.28 g/L 4.50 g/L 0.500 g/L
1.75 g/L
When 429 mmHg of argon, 1.2 atm of neon, and 225 mmHg of helium are mixed, what is the total pressure? 774 mmHg 1287 mmHg 1566 mmHg 655 mmHg
1566 mmHg
Gases tend to have _____ densities than either liquids or solids, and their _____ change greatly with changes in temperature or pressure. lower, masses higher, volumes higher, masses lower, volumes
lower, volumes
Which temperature and pressure correspond to STP? 0°C 1 kPa 0 K 1 mmHg 25°C 1 atm
0°C 1 atm
Arrange the following gases in order of increasing density (highest density at the bottom of the list) under the conditions given. Assume that the volume of the container is not fixed.
1. Helium at 1 atom and 273 Neon at 1 atm and 273 Neon at 2 atm and 273 Neon at 2 atm and 73
At STP the volume of 1 mole of an ideal gas is always equal to ___________L (given to three significant figures.). This quantity is called the standard __________ volume.
22.4, molar
Select all the statements that correctly describe the mole fraction of a component in a mixture. A mole fraction is dimensionless. In a mixture of gases, the partial pressure of each gas is proportional to its mole fraction. The mole fraction of a component can range from 0 to 100. A mole fraction can be converted to a mole percent by multiplying by 100. A mole fraction can be calculated only when there are two components in the mixture.
A mole fraction is dimensionless. In a mixture of gases, the partial pressure of each gas is proportional to its mole fraction. A mole fraction can be converted to a mole percent by multiplying by 100.
Select all the statements that describe the particles in a sample containing a mixture of gases at a given temperature. All the particles have the same average kinetic energy. All the particles have the same mass. On average, the lighter particles move faster than the heavier particles. All the particles have the same most probable speed.
All the particles have the same average kinetic energy. On average, the lighter particles move faster than the heavier particles.
Helium effuses 3.16 times faster than an unknown gas under identical conditions. Predict the identity of the unknown gas. Oxygen Argon Neon Nitrogen
Argon
Select all the statements that correctly describe a gas contained in a rigid cylinder fitted with a moveable piston. Refer to the visual provided. At the particulate level, the gas particles are pushed closer together as the piston moves down. The gas may be compressed by increasing the external pressure. The gas may be compressed by decreasing the external pressure. At the particulate level, the gas particles are forced farther apart as the piston moves down.
At the particulate level, the gas particles are pushed closer together as the piston moves down. The gas may be compressed by increasing the external pressure.
Which of the following are postulates of the kinetic molecular theory of gases? The average kinetic energy of the gas particles is inversely proportional to the absolute temperature. Collision of gas particles are assumed to be elastic. The volume of gas particles is negligible compared to the volume occupied by the gas. The gas particles do not exert attractive or repulsive forces on each other. The gas particles are in constant, random motion although they do move in straight lines.
Collision of gas particles are assumed to be elastic. The volume of gas particles is negligible compared to the volume occupied by the gas. The gas particles do not exert attractive or repulsive forces on each other. The gas particles are in constant, random motion although they do move in straight lines.
Select all the statements that correctly describe the properties of gases. Gases have relatively low densities. Temperature changes have a large effect on the volume of a gas. Gases are much more compressible than liquids or solids. Gases mix with other gases only if their molecules are of the same type.
Gases have relatively low densities. Temperature changes have a large effect on the volume of a gas. Gases are much more compressible than liquids or solids.
Select all the diatomic elements that exist as gases at room temperature. Halogens such as F2 and Cl2 Hydrogen gas Noble (or inert) gases Nitrogen and oxygen
Halogens such as F2 and Cl2 Hydrogen gas Nitrogen and oxygen
Select all the statements that correctly describe what happens when a gas is heated in a flexible container at constant pressure. The gas particles move faster. The surface area of the walls of the container decreases. The gas particles collide with the walls of the container with a greater force. The volume of the gas container increases. The gas increases in volume because the particles increase in size.
The gas particles move faster. The gas particles collide with the walls of the container with a greater force. The volume of the gas container increases.
Two tables that are equal in mass are resting on the same rug. The four legs of one table each have a 2" x 2" cross-section, while the four legs of the second table each have a 4" x 4" cross-section. Which table is exerting greater pressure on the rug? The table with the thinner legs is exerting greater pressure. Both tables are exerting the same pressure. The table with the thicker legs is exerting greater pressure.
The table with the thinner legs is exerting greater pressure.
What happens to the volume of a gas when the number of moles is doubled at constant T and P? The volume decreases by a factor of 2. The volume does not change. The volume increases by a factor of 2.
The volume increases by a factor of 2.
Charles's law states that for a gas at constant pressure, the volume occupied by a fixed amount of the gas is _____ proportional to the absolute temperature, i.e., the temperature measured in kelvins. This means that as the temperature increases the volume will _____. inversely; increase inversely; decrease directly; decrease directly; increase
directly; increase
Each component in a mixture contributes a fraction to the total number of moles in the mixture. This fraction is called the _________ fraction of the component. In a mixture of gases, this fraction is proportional to the _________ pressure for each gas present.
mole, partial
As the temperature of a gas increases _____. (Select all the options that complete this sentence correctly.) the speed of individual gas particles increases but the average speed remains the same the average speed of a gas particle increases the average kinetic energy of the gas particles increases the distribution of the speeds of the gas particles narrows
the average speed of a gas particle increases the average kinetic energy of the gas particles increases
A sample of gas has a volume of 32 L at 75°C. At what temperature will the volume be equal to 16 L? 1.47°C -99°C 423°C 38°C
-99
A sample of nitrogen gas has a volume of 5.0 mL at a pressure of 1.50 atm. What is the pressure exerted by the gas if the volume increases to 30.0 mL, at constant temperature? 0.25 atm 9.0 atm 1.5 atm 7.5 atm
0.25 atm
If 1.0 mole of neon, 2.0 moles of helium, and 3.0 moles of argon are mixed, what is the mole fraction of helium? 0.17 0.50 0.33 33
0.33
Examine the image depicting the reaction of hydrogen and nitrogen gases to form ammonia. The colors used for H atoms and N atoms are white and blue, respectively. According to Avogadro's law, ____ volume(s) of H2 combine with ____ volume(s) of N2. 3, 1 1, 3 1, 1 2, 1
3, 1
Aqueous Na2SO3 may be used to remove SO2(g) due to the reaction: Na2SO3(aq) + SO2(g) + H2O(l) → 2NaHSO3(aq). When aqueous Na2SO3 was placed in a room containing 3.5 × 104 L of SO2-contaminated air at 25°C, the pressure changed from 0.9955 atm to 0.9900 atm. How many moles of SO2 were removed by the chemical reaction with Na2SO3(aq)? 7.9 mol 0.13 mol 0.65 mol
7.9 mol
Potassium chlorate is decomposed to produce potassium chloride and oxygen gas, which is collected over water. 2KClO3(s) → 2KCl(s) + 3O2(g) What is the partial pressure of oxygen (in torr) if the total pressure at 25oC was 748.6 torr? 748.6 772.4 724.8 760.0
724.8
Potassium chlorate is decomposed to produce potassium chloride and oxygen gas, which is collected over water. 2KClO3(s) → 2KCl(s) + 3O2(g) What is the partial pressure of oxygen (in torr) if the total pressure at 25oC was 748.6 torr? 760.0 748.6 724.8 772.4
724.8
A small piece of Cr metal reacts with dilute HNO3 to form H2 (g), which is collected over water at 25oC in a large flask. The total pressure in the flask is 762 torr. Use the table provided to determine the partial pressure of the H2 present. 786 torr 738 torr 23.8 torr 737 torr
738 torr
Calculate the volume occupied by 2.0 moles of an ideal gas at 25°C and 380 mmHg. 98 L 8.2 L 0.13 L 0.010 L
98L
Which of the following is the statement of Dalton's law of partial pressures? Ptotal = ΣPi d = PℳRTPℳRT PV = nRT urms = 3RT/ℳ‾‾‾‾‾‾‾‾√
Ptotal = ΣPi
Using postulates of kinetic molecular theory, select the statement(s) that correctly describe(s) the assumptions used to define an ideal gas as distinct from a real gas. Gas particles are separated by relatively large distances. The actual volume of the gas particles is negligible compared to the container volume. Gas particles do not exert attractive or repulsive forces on one another.
The actual volume of the gas particles is negligible compared to the container volume. Gas particles do not exert attractive or repulsive forces on one another.
A sample of gas is heated steadily in a closed rigid container. Which of the following correctly describes the result? The volume of the gas will increase. The pressure in the container will decrease. The volume of the gas will decrease. The pressure in the container will increase.
The pressure in the container will increase.
At constant T and P, 2.0 L of nitrogen gas are combined with 6.0 L of hydrogen gas to form ammonia. Which of the following statements correctly describe the outcome of the reaction, assuming it goes to completion? Select all that apply. Multiple select question.
The product occupies a volume of 4.0 L under these conditions. When the reaction is completed, only NH3 is present. N2 combines with H2 in a 1:3 ratio.
Phosphorus reacts with hydrogen according to the balanced equation P4 (s) + 6H2 (g) → 4PH3 (g). If 8.50 g of phosphorus reacts with hydrogen gas at 2.00 atm in a 10.0-L container at 298 K, calculate the moles of PH3 produced as well as the total number of moles of gas present at the conclusion of the reaction. Multiple select question. 0.817 mol of PH3 are produced. The total amount of gas present is 0.679 mol. 0.274 mol of PH3 are produced. The total amount of gas present is 0.545 mol.
The total amount of gas present is 0.679 mol. 0.274 mol of PH3 are produced.
A reaction may be carried out so that a gaseous product is collected over water. Which statement describes how to calculate the pressure due to the product gas alone? The vapor pressure of the water must be subtracted from the barometric pressure. The vapor pressure of the water at 25oC must be subtracted from the barometric pressure. The vapor pressure of the water must be added to the barometric pressure. The pressure due to the water is very small and can be ignored.
The vapor pressure of the water must be subtracted from the barometric pressure.
What happens to the volume (V2) of a gas sample when the pressure (P1) is doubled and the Kelvin temperature (T1) is tripled? V2 = 3V123V12 = 1.5V1 V2 = V1 V2 = 2V132V13 = 0.67V1 V2 = 6V1
V2 = 3V123V12 = 1.5V1
Examine the graphical depiction of the volume of a gas sample as a function of pressure at constant T. Which statement is correct? Volume remains constant as pressure changes. Volume decreases as pressure increases. Volume increases as pressure increases.
Volume decreases as pressure increases.
The kinetic energy of gas particles is _____. directly proportional to the square of the speed of the gas particles directly proportional to the square of the mass of the gas particles directly proportional to the speed of the gas particles directly proportional to the square root of the mass of the gas particles
directly proportional to the square of the speed of the gas particles
At a fixed T and P, the volume occupied by a gas is __________ proportional to the number of moles of gas present. For any ideal gas at constant temperature and pressure, equal _________ of gas contain equal numbers of particles or moles. Listen to the complete question
directly, volume
The atmosphere exerts a pressure on you; however, you do not feel the pressure and you are not crushed by it. This observation is explicable because the pressure inside your body is _____ the atmospheric pressure outside. equal to greater than less than
equal to
The equation PV = nRT expresses the ideal gas equation. In this equation, the symbol R indicates the __________ gas constant, which may have different values depending on the units used to express ________ and pressure.
ideal, volume
In the form of the combined gas law shown, the subscript 1 refers to _____ conditions while the subscript 2 refers to _____ conditions for a sample of gas. initial, final final, initial
initial, final
The root-mean-square (rms) speed (urms) of a gas particle is _____. (Select all that apply.) the speed of all the gas particles in a given sample proportional to the square root of the absolute temperature of the gas particles inversely proportional to the square root of the molar mass the speed of gas particles that have the average kinetic energy
proportional to the square root of the absolute temperature of the gas particles inversely proportional to the square root of the molar mass the speed of gas particles that have the average kinetic energy
Dalton's law of partial pressures states that the __________ pressure exerted by a gas mixture is the _________ of the partial pressures of the component gases in the mixture.
total, sum
At STP, the density of argon is _____. one-half the density of neon the same as the density of neon twice the density of neon ten times the density of neon
twice the density of neon
Which equation correctly represents the effects of the absolute temperature and molar mass of the gas on the root-mean-square (rms) speed? ℳ denotes the molar mass of the gas. urms = 3Rℳ/T‾‾‾‾‾√ urms = 3RT/ℳ‾‾‾‾√ urms = 3RT/ℳ urms = 3Rℳ/T
urms = 3RT/ℳ‾‾‾‾√
The images shown illustrate the effect of pouring liquid N2 over a balloon. At constant pressure, the ___________ of the gas in the balloon is proportional to its __________.
volume, temperature
What is the correct relationship between the number of moles of gas consumed and the change in pressure in the reaction vessel, at constant V and T? (Δn)(ΔP) = (VRTVRT) Δn = ΔP(VRTVRT) ΔP = Δn(VRTVRT)
Δn = ΔP(VRTVRT)
How many moles of an ideal gas will occupy a volume of 33.6 L at 0°C and 1 atm? 0.667 mol 1.50 mol 0.123 mol
1.50 mol
A particular hydrocarbon with the empirical formula CH2 has a density is 1.84 g/L at STP. Select the correct molecular formula of the gas. C3H6 C4H8 C2H4 C5H10
C3H6
Absolute zero is the temperature at which an ideal gas would have _____ volume. This temperature corresponds to _____ °C Celsius and _____ K. Multiple choice question. real; 0; 273.15 real; -273.15; 0 zero; 273.15; 0 zero; -273.15; 0
zero; -273.15; 0
A mixture of gases contains 1.50 mol of O2, 0.75 mol of He, and 2.25 mol of N2. The total pressure exerted by the mixture is equal to 2.50 atm. What is the partial pressure of the He? 1.88 atm 0.418 atm 1.75 atm 3.33 atm
0.418 atm
A gas cylinder with a moveable piston initially contains 0.25 moles of neon in 5.0 L. If 0.50 moles of helium are added to this gas cylinder, what will be the final volume at constant P and T? 2.5 L 15 L 10. L 1.7 L
15L
When the temperature of a 3.0-L sample of a gas is dropped from 200°C to 100°C, what will be the final volume of the gas sample? 2.4 L 1.5 L 3.8 L 6.0 L
2.4L
The density of a gas is 2.49 g/L at 3.00 atm and 25°C. Calculate the molar mass of the gas. 24.9 g/mol 2.0 g/mol 18.3 g/mol 20.3 g/mol
20.3 g/mol
What is the volume occupied by 1 mole of an ideal gas at STP? Multiple choice question. 0 L 22.4 L 273 L 1 L
22.4
Which of the following are equivalent to 652 mmHg? Select all that apply. 1.17 atm 86.9 kPa 5.66 × 103 kPa 0.858 atm
86.9 kPa 0.858 atm
Why does pressure rise as the volume of a piston filled with gas is reduced at constant temperature? Hint: Use a molecular view of gases to guide your reasoning. Gas particles move faster in a smaller volume. Collisions with the walls are more frequent. Collisions of gas particles with each other are more frequent.
Collisions with the walls are more frequent.
Compare the molecular speeds for N2 at a constant temperature using the image provided. The greatest fraction of gas molecules with the most probable speed is observed at the _____ temperature. lowest highest
lowest
Dalton's law of partial pressures states that for a mixture of gases, the __________ pressure is the _________ of the partial pressures of the individual gases. (Assume that the gases do not react with each other.)
total, sum
Select all statements that correctly describe the relationship between the parameters investigated in the Boyle's law experiment shown in the visual. The variable parameters are volume and temperature. As pressure increases from (a) to (b) to (c), the volume of the gas decreases. The variable parameters are pressure and volume. The number of moles of gas remains constant. The temperature increases from (a) to (b) to (c).
As pressure increases from (a) to (b) to (c), the volume of the gas decreases. The variable parameters are pressure and volume. The number of moles of gas remains constant.
Which of the following options correctly express the relationship between the volume and temperature of a gas at constant pressure? Select all that apply. As the temperature of the gas increases, the volume will increase. VT is a constant value. The volume of the gas is directly proportional to the absolute temperature. There is an inverse relationship between volume and temperature.
As the temperature of the gas increases, the volume will increase. The volume of the gas is directly proportional to the absolute temperature.
True or false: At the same temperature, the rms speed of H2 is twice that of O2. True false question.
False
Select all the statements that correctly describe the arrangement of individual particles in the three physical states of matter. Relate these particulate views to the observable properties of matter. Gases occupy the entire volume of the container. The particles in a solid move quite freely. The particles in a solid occupy fixed positions. Liquids take the shape of the container. Liquids have the same fixed arrangement of particles as observed in solids. The particles in a gas move quite freely.
Gases occupy the entire volume of the container. The particles in a solid occupy fixed positions. Liquids take the shape of the container. The particles in a gas move quite freely.
Which of the following is the correct mathematical expression for the relationships between pressure, volume, and temperature for a fixed amount of gas? P1V1T1P1V1T1 = P2V2T2P2V2T2 P1T1V1P1T1V1 = P2T2V2P2T2V2 P1V1T1P1V1T1 = P2V2T2P2V2T2 P1V1T1 = P2V2T2
PV/T=PV/T
Which of the following options correctly describe the gas constant, R? Select all that apply. R may have different values depending on the units used to express volume and pressure. R = 8.314 if pressure is in atm and volume is in L. R is a proportionality constant used in gas law calculations. R is only used for calculations at STP.
R may have different values depending on the units used to express volume and pressure. R is a proportionality constant used in gas law calculations.
Using the general trends in the images provided, select all the statements that correctly describe the distribution of molecular speeds. At the same T, the most probable speed of a He atom is greater than that of a H2 molecule. SF6 molecules moves more slowly than SO2 molecules at the same T. For any gas, the most probable speed decreases as T increases. Most gas particles have speeds higher or lower than the most probable speed at a given T.
SF6 molecules moves more slowly than SO2 molecules at the same T. Most gas particles have speeds higher or lower than the most probable speed at a given T.
Consider a sample containing 1 mol of an ideal gas in a flexible, closed container. Which of the following changes will cause the volume to decrease? Select all that apply. Temperature increases and external pressure decreases. External pressure decreases while temperature remains constant. Temperature decreases while external pressure remains constant. Temperature decreases and external pressure increases.
Temperature decreases while external pressure remains constant. Temperature decreases and external pressure increases.
Select all the statements that correctly describe the image presented. Assume that the temperature remains constant during the process depicted. The image shows that the pressure of a gas decreases as volume decreases. The number of gas particles remains constant. This image represents a molecular view of Boyle's law. The image shows a decrease in the volume of the system.
The number of gas particles remains constant. This image represents a molecular view of Boyle's law. The image shows a decrease in the volume of the system.
The images shown illustrate the effect of pouring liquid N2 over a balloon. Which statements correctly describe the changes observed in image (b) compared to image (a)? Select all that apply. Multiple select question. The number of moles of air in the balloon remains constant. The volume of air in the balloon decreases. The pressure of air in the balloon increases. The addition of liquid N2 decreases T.
The number of moles of air in the balloon remains constant. The volume of air in the balloon decreases. The addition of liquid N2 decreases T.
True or false: A linear plot is obtained when volume is plotted against reciprocal pressure for a gas sample at constant temperature.
True
True or false: Temperatures must always be converted to the Kelvin temperature scale for gas law calculations.
True
Select all the parameters that describe the physical state of a gas sample. Volume Number of moles Color of gas Temperature Pressure
Volume Number of moles Temperature Pressure
Examine the plot of the volume of a sample of gas versus temperature at three different pressures. Select all the correct statements derived from and/or related to this graphical presentation. When the lines are extrapolated to V = 0, they all meet at a single temperature. When the lines are extrapolated to V = 0, they all meet at a temperature of -273.15ºC. This temperature at which a gas could hypothetically have zero volume is called absolute zero. The temperature corresponding to V = 0 is 0ºC. When the lines are extrapolated to V = 0, they all meet at a temperature of 273.15ºC.
When the lines are extrapolated to V = 0, they all meet at a single temperature. When the lines are extrapolated to V = 0, they all meet at a temperature of -273.15ºC. This temperature at which a gas could hypothetically have zero volume is called absolute zero.
At constant temperature and volume, gas pressure is ______ to the number of moles in the sample. directly proportional not mathematically related inversely proportional
directly proportional
The particles in a gas have a _____ distance between them than the particles of a liquid or a solid and their movement is random. Gas particles therefore move _____ freely than the particles of solids or liquids. smaller, more greater, less smaller, less greater, more
greater, more
As the temperature of a gas sample at constant pressure increases, the volume of the gas will _____ and there will be _____ gas particles in the same space. The density of a gas at constant pressure therefore _____ as the temperature increases. decrease; fewer; decreases increase; more; increases decrease; more; increases increase; fewer; decreases
increase; fewer; decreases
A sample of a gas is compressible; i.e., its volume can be significantly decreased. This is because ______ there are attractive forces between particles in the gas phase, whereas in the liquid and solid phases there are not. particles in the gas phase are smaller than they are in the liquid and solid phases. particles in the gas phase are separated by relatively large distances.
particles in the gas phase are separated by relatively large distances.
When walking on powdery snow, snowshoes keep you from sinking into the snow because _____. Remember, pressure is force per unit area. the mass of a snowshoe is less than the mass of a boot snowshoes repel snow the area of a snowshoe is greater than that of a boot
the area of a snowshoe is greater than that of a boot