Chem Wk 14: Properties of Gas, KMT, ATMs, Gas Laws, Gases in Chemical Rxns, Mixtures of Gases, Real Gases

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760 760

1 atm = ____ mmHg = ___ torr

mole fraction units 1

1. The partial pressure of each component gas depends only on the component's ___ ___ and the total pressure of the gas mixture. It does not depend on the identity of the component gas or on the other gases in the mixture. 2. Mole fractions have no ___. This means they can be used when describing the behavior of any kind of homogeneous mixture. 3. Finally, the sum of the mole fractions of all the components in a mixture should always add up to __

Volume at STP

22.4 L/mol

Standard Temperature and Pressure (STP)

A temperature of 273 K and a pressure of 1.00 atm

volume pressure

All ideal gases are identical, in terms of their ___ and ____, so it does not matter if one gas is present, or several. The total pressure of a mixture of gases equals the sum of the pressure that each would exert if it were present alone.

molar mass

Although kinetic molecular theory tells us that all populations of gas particles at a given temperature have the same avg kinetic energy, they will not all have the same root-mean-square speed unless they have the same ___ ___

decreases

As M (molar mass) increases, Urms ____.

narrower

As mass increases, Urms decreases As mass increases, speed distribution gets ____.

particles decreases

As mass of gas increases, the # of ____ in a 1g sample ____

closer IMFs smaller

As pressure increases, particles are forced ___ together, so they interact through ___. (Pressure seems ___ than expected)

distribution

As temp increases, we have increased urms, and wider ____ of speeds. urms = square root(3RT/M) where M is molar mass

decreases

As volume increases, density ____.

100 g of gas mixture

Assume __ __ __ ___.

259 mL

At a constant temperature and pressure, the ideal gas law tells us that the volume of 1.00 mol of gas is the same, regardless of its identity. This means that we can compare the volumes of gases the same way we compare moles of gases. It is sometimes easier to measure the volumes of gases rather than their masses in reactions.

densities lower

At a given temperature and pressure, the ____ of gaseous substances are directly proportional to their molar masses and are much ____ than their densities as solids or liquids.

Boyle's law Reference Slide

Boyle's law Reference Slide

Calculating the Quantity of a Gas collected by Water Displacement (pt.1)

Calculating the Quantity of a Gas collected by Water Displacement (pt.1)

Calculating the Quantity of a Gas collected by Water Displacement (pt.2)

Calculating the Quantity of a Gas collected by Water Displacement (pt.2)

Combined Gas Law Example 1

Combined Gas Law Example 1

Combined Gas Law Example 2

Combined Gas Law Example 2

P1V1/n1T1 = P2V2/n2T2

Combined Gas Law Useful Rearrangements: PV=nRT = ____ = _____

Density Exam Type Question

Density Exam Type Question

directly

Density Vs Pressure of an ideal Gas are ____ proportional

Density of a gas reference slide

Density of a gas reference slide

Different Deviations in gases practice

Different Deviations in gases practice

Different gases deviating differently slide

Different gases deviating differently slide

different IMFs Size

Different gases will deviate from ideal behavior in ___ ways: Strength of ___ and the ___ of gas particles will influence this.

Different values of the Universal Gas Constant (R)

Different values of the Universal Gas Constant (R)

own

Each gas in air, or in any other mixture of gases, exerts its ___ pressure

composition

Even though pressure changes, the ___ of the gas does not.

Final Exam Notes

Final Exam Notes

changing

For a problem where there is a change involved, we must manipulate the ideal gas law to fit the given conditions. 1. Determine which variables are ____ and which are held constant

constants same side

For a problem where there is a change involved, we must manipulate the ideal gas law to fit the given conditions. 2. Rearrange the equation so that all the ___ are on the ___ ___ of the equals sign.

Get rid

For a problem where there is a change involved, we must manipulate the ideal gas law to fit the given conditions. 3. ___ ___ of all the constants

given numbers

For a problem where there is a change involved, we must manipulate the ideal gas law to fit the given conditions. 4. Plug the ___ ___ into the equation

Temp. in Kelvin (C + 273.15)

Gas calculations MUST have ___ ___ ___

ideally

Gases are more likely to behave ___ under low pressure and high temperature conditions.

entire

Gases expand to occupy the ____ volume of their containers

Gases in Chemical Rxns example Problem (pt.1)

Gases in Chemical Rxns example Problem (pt.1)

Gases in Chemical Rxns example Problem (pt.2)

Gases in Chemical Rxns example Problem (pt.2)

effuse molar masses smallest

Gases in inflated party balloons escape, or ___ , through the walls of the balloons at rates that are inversely proportional to the ___ ___ of the gases. Those with the ___ molar masses, such as helium, escape the most rapidly.

Ideal gases

Gases that behave in accordance with the combined gas law are called ideal gases

Ideal Gas Law Reference Slide moles K L

Ideal Gas Law Reference Slide: n must be in ___ Temp must be in ___ V in ___

high pressures low intermolecular attractions

Ideal Gas conditions don't hold true under extremely ___ ___ or when subjected to temperatures so ___ that they approach the temperature at which the gases condense. This is because these conditions allow for more _____ _____ to occur

moles volume temperature pressure stoichiometry

In chemical reactions involving a gas as either a reactant or product, the quantity of it (in ___) in the reaction mixture can be determined using the ideal gas law if we know the ___ of the gas and the ____ and ____ at which the reaction proceeds. Once we know the value of n, we can calculate the quantities of the other reactants or products, including the quantity of energy released or consumed, from the ____ of the reaction.

KMT Reference Slide

KMT Reference Slide

negligible no volume

KMT assumptions 1. gas molecules have very tiny volumes compared to the volume they occupy. Individual volumes are considered ____, allowing gas particles to be treated as point masses- masses with essentially ___ ___.

elastic

KMT assumptions 2. Gas molecules move constantly and randomly throughout the space they occupy, continually colliding with one another and their container walls. Collisions considered ____ (result in no net transfer of energy to the walls)

intermolecular

KMT assumptions 3. Because gas particles are so spread out, we assume ____ forces of attraction to one another are negligible. Assume particles don't interact at all

proportional avg. kinetic energy.

KMT assumptions 4. The average kinetic energy of the molecules in a gas is ____ to the absolute temperature of the gas. All populations of gas molecules at the same temperature have the same ___ ___ ___

continuous random

Kinetic Molecular Theory of Gases 1. Gas particles are in ___ ___ motion 2. Volume of gas particles is small relative to total volume in which gas is contained. Distances between particles is large 3. Attractive forces between molecules are zero 4. Collisions between molecules are perfectly elastic. The average kinetic energy is proportional only to temperature.

E=1/2mv^2

Kinetic energy equation

.08206

L*atm/mol*K common value of R

Mole Fraction Reference Slide

Mole Fraction Reference Slide

Mole ratio problems

Mole Ratio Problem

Amontons's Law Equation

P1/T1=P2/T2

Combined gas law

P1V1/T1=P2V2/T2

Boyles law equation

P1V1=P2V2

PV = nRT example 1

PV = nRT example 1

PV = nRT example 2

PV = nRT example 2

PV=nRT Algebra Exam type Question

PV=nRT Algebra Exam type Question

Particle Speed and temperature relationship

Particle Speed and temperature relationship

SW Warm-Up 35; Question 1 Answer 4.38 atm

Pressure Change within a rxn practice problem

inversely directly directly

Pressure and volume are ____ proportional Pressure and Temperature are ____ proportional Volume and Temperature are ____ proportional

less add greater subtract

Pressure is ___ than expected due to IMFs (we ___ in the equation). Volume is ___ than expected due to gas particle size (we ___ in the equation)

volume greater

Real gases have nonzero ____. (Volume seems ____ than expected)

Relative Rates of effusion equation

Relative Rates of effusion equation

Relative Rates of effusion problem

Relative Rates of effusion problem

Temperature

Remember: Average kinetic energy depends only on ____

Rxn Equation Exam Type Problem

Rxn Equation Exam Type Problem

273.15 one ideal 22.4L

Standard Temperature and Pressure: STP: ____ K (0 C)& 1.00 atm At STP, ___ mole of ___ gas occupies a volume of ____

colliding densely pressure

The average distance that a particle can travel through air or any gas before ____ with another one is called the mean free path of the particle. Mean free paths depend on how ____ the air particles are packed, and that depends on their ____.

higher Urms

The average speed of the particles (obtained by adding all the individual speeds and dividing by the total number of particles) is slightly ____ than the most probable speed. Because temperature is proportional to average kinetic energy, and kinetic energy is proportional to the square of speed, it is convenient to define another type of average:the root-mean-square speed. This is the speed of a molecule with average kinetic energy. ____ occurs at a higher speed than either um or uavg.

molar mass 22.4L/mol

The density of any gas at STP can be calculated by dividing its ___ ____ by the molar volume (____)

dipole-dipole stronger greater deviation

The different intermolecular forces experienced by different compounds affect how significantly a particular gas will deviate from ideal behavior under high-pressure and/or low-temperature conditions. For example, polar molecules such as chloromethane (CH3Cl) will experience ___-___ forces that result in attractions between the molecules. These forces are typically ____ than the attractive LDFs experienced by nonpolar molecules such as CH4, and we can predict ___ ____ form ideality for chloromethane than from methane.

spread through another.

The effusion of gases is closely related to their diffusion, which is defined as the ____ of one substance ___ ___

directly

The gas pressure inside a rigid container at constant temperature is ____ proportional to the quantity (number of moles) of gas in the container

temperature pressure 1

The molar volume of an ideal gas takes into account ____ in Kelvin, atm. ____, and number of moles (molar volume assumes ___ mol). Plug this into PV=nRT

abundant partial pressures

The most ___ gases in a mixture have the greatest ___ ___ and contribute the most to the total pressure of the mixture. The mathematical term used to express the abundance of a specific component "i" in a mixture of gases is its mole fraction (xi)

Pi = xiPtotal

The partial pressure of each component is the product of its mole fraction times the total pressure of the mixture.

directly

The pressure of a quantity of gas in a rigid container is ____ proportional to its absolute temperature

Amontons's law (also, Gay-Lussac's law)

The principle that the pressure of a fixed quantity of gas is proportional to its absolute temperature if its volume does not change

Boyle's Law

The principle that the volume of a fixed quantity of gas at constant temperature is inversely proportional to its pressure

Pressure (P)

The ratio of force, F , to surface area, A , defines ___ (_)

inversely

The speed of gas particles at a given temperature are ___ related to their masses.

increasing

The value of both van der Waals constants increase with ____ molar mass and with number of atoms per molecule. Makes sense because larger molecules both take up more space and experience larger LDFs leading to stronger intermolecular forces.

inversely

The volume of a gas is ____ proportional to the pressure we apply.

mole

There are 6.022E^23 gas particles in one ____ of every gas sample.

(3RT/M)^1/2

There is a relationship between the velocity of a gas and its molar mass shown by the equation Urms= ____. Where Urms is the root-mean-square speed of the gas in Meters/second. T is the temperature of the gas in Kelvin. M is the molar mass of the gas in kg/mol.

rxn equation

To determine Pressure and other variables "as reaction proceeds", must always write out ____ ____

high size space increases decreases

Two competing factors-intermolecular forces and the volume of gas-phase particles- can cause PV/RT to decrease or increase with increasing external pressure. At extremely ___ pressures, the ____ of the particles and the ___ they occupy become the dominant factor and PV/RT ___ with increasing P. At less extreme pressures, intermolecular forces may offset the incompressibility of particles and the value of PV/RT ____ with increasing P for some gases, including CH4 and CO2 as shown in figure 9.34

volumes do not masses

Under ideal conditions, the ____ of the individual gas particles are insignificant in comparison to the overall volume occupied by the gas and the particles ___ __ interact with one another. Instead they move independently with speeds that are related to their ____ and to the temperature of the gas.

Charles's Law equation

V1/T1 = V2/T2

Avogadro's Law Equation

V1/n1 = V2/n2

reacts dissolves

Water displacement can be used to collect and measure the volume of any gas that neither ___ with nor ___ appreciably in water.

MP/RT=d

We can use the ideal gas equation to calculate the density of a gas at any temperature and pressure. n/V = P/RT Mn/V=d _____

Weird Partial Pressure Question

Weird Partial Pressure Question

Which equations produce Constants

Which equations produce Constants

Pressure

___ is the amount of force applied to an area

Kinetic Molecular theory of gases (KMT)

a model that explains the behavior of gases on the basis of the motion of the particles that make them up

miscible

all gases are ____ with all other gases - that is, gas mixtures are homogeneous (unless the gases react with each other)

van der Waals equation

an equation describing how the pressure, volume, and temperature of a quantity of a real gas are related; it includes terms that account for the incompressibility of gas particles and interactions between them.

van der Waals forces

any interaction between neutral atoms and molecules, including hydrogen bonds, other dipole-dipole interactions, and London dispersion forces; the term does not apply to interactions involving ions

increasing

atmospheric pressure decreases with ____ altitude. Atmospheric pressure is related to the mass of the column of air above that location. As altitude increases, the mass of the column of air above that altitude decreases. Less mass means a smaller force exerted downward by the air at higher altitude which means less pressure.

Universal gas constant (R)

the constant R in the ideal gas equation; its value and units depend on the units used for the variables in the equation

partial pressure

the contribution to the total pressure made by a component in a mixture of gases. Atmospheric pressure is the sum of the partial pressures of all the gases in the air

Ideal gas equation (ideal gas law)

the principle relating the pressure, volume, number of moles, and temperature of an ideal gas, expressed by the equation PV=nRT where R is the universal gas constant. The value R, however, depends on the units used for pressure and volume (we always express gas in moles and use the Kelvin scale for temperature).

Dalton's Law of partial pressures

the principle that the total pressure of a mixture of gases is the sum of partial pressures of all the gases in a mixture

Charles's Law

the principle that the volume of a fixed quantity of gas at constant pressure is directly proportional to its absolute temperature.

effusion

the process by which a gas escapes from its container through a tiny hole into a region of lower pressure

Avogadro's Law

the prterm-39vinciple that the volume of a gas at constant temperature and pressure is proportional to the quantity (number of moles) of the gas

Graham's law of effusion

the rate of effusion of a gas is inversely proportional M (molar mass)

mole fraction (xi)

the ratio of the number of moles of a particular component "i" in a mixture to the total number of moles in the mixture

average speed.

the root-mean-square speed is a synonym for ___ ___

pressure volume

the van der Waals equation includes two terms to correct for (1) intermolecular forces that lower the number of independent particles and the ___ they create by colliding with the container walls [the a(n/V)^2 term] and (2) the ___ taken up by the particles of a gas, which are not compressible (the nb term)

temp

urms = the speed of a particle with average kinetic energy (will never have to calculate). If ___ is the same, will have the same urms

van der Waals constants practice

van der Waals constants practice

van der Waals constants practice 2

van der Waals constants practice 2

van der Waals constants slide

van der Waals constants slide


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