Potential theory
Kinetic theory
Gas theory
An increase in temperature causes an increase in the pressure exerted by the gas.
An increase in temperature causes an decrease in the pressure exerted by the gas.
An decrease in temperature causes an increase in the pressure exerted by the gas.
Three basic assumptions of the potenial theory about the properties of gases.
Three basic assumptions of the kinetic theory about the properties of gases.
Three basic assumptions of the gas theory about the properties of gases.
Non compressibility of gases.
Compressibility of gases.
Gas particle compressibility
The gases used to inflate the airbag are compressible and are able to absorb a considerable amount of energy.
The gases used to inflate the airbag are not compressible and are able to absorb a considerable amount of energy.
The gases used to inflate the airbag are compressible and are not able to absorb a considerable amount of energy.
The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a liquids.
The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a gas.
The name, the symbol, and a common unit for the four variables that are generally used to describe the characteristics of a solids.
Feet, hands, legs,arms
Chair, table shoes,windows
Automobile tires,air compressors, air brakes,aerosol cans
Because air particles are added, the pressure increases inside the tire.
Because air particles are added, the pressure decreases inside the tire.
Because air particles are taken away, the pressure increases inside the tire.
The pressure inside the tire can increase beyond the strength of its walls, causing the tire to rupture or burst.
The pressure inside the tire can decrease beyond the strength of its walls, causing the tire to rupture or burst.
The pressure outside the tire can decrease beyond the strength of its walls, causing the tire to rupture or burst.
Same
Higher
Lower
The jar of pickles will closs tightly.
The garbage can lid will pop off.
The spray button on an aerosol spray can is pressed.
Increase
Decrease
Stay the same
Describes how gases behave when the temperature increases
Describes how gases behave when the temperature decreases
Describes how gases behave when the temperature istays the same
Explain why it is dangerous to bounce an aerosol can into a fire.
Explain why it is dangerous to open aerosol cans over a fire.
Explain why it is dangerous to throw aerosol cans into a fire.
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.
At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component liquid.
At constant volume and temperature, the total non pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.
Gases
Diffusion
Effusion
The same
Slower
Faster
CH 4 exponent at 100 °C
CH 4 exponent at 300 °C
CH 4 exponent at 200 °C
Gas particles are attracted to each other. k Gas particles have some volume.
Gas particles are not attracted to each other. k Gas particles have no volume.
Gas particles are attracted to each other. k Gas particles have alot volume.
Increase
Decrease
Stays the same
Boyle's hypothesis
Charles hypothesis
Avogadro's hypothesis
As long as the gas particles are not tightly packed, there is a great deal of occupied space between them, A container can easily accommodate the same number of relatively large or relatively small gas particles.
As long as the gas particles are not tightly packed, there is a great deal of empty space between them, A container can easily accommodate the same number of relatively large or relatively small gas particles.
As long as the gas particles are not tightly packed, there is a great deal of occupied space between them, A container can easily accommodate the same number of relatively large or relatively large gas particles.
6.02 x 1Q 30 exponents particles
6.02 x 1Q 25 exponents particles
6.02 x 1Q 23 exponents particles
Gas energy
Potential energy
Kenetic energy
Partial pressure
Complete pressure
No pressure
Potential theory
Kinetic theory
Gas theory
True about ideal gases and the potential theory.
True about ideal gases and the kinetic theory.
True about ideal gases and the gas theory.
Important
Possible
Impossible
Less than ideal behavior
Ideal behavior
No behavior
___(P x V)____ (n x R x T)
___(P x V)____ (n R x T)
__2_(P x V)____ (n x R x T)
30 000 kPa
20 000 kPa
10 000 kPa
CO 8 exponent at 40 °C
CO 4 exponent at 40 °C
CO 2 exponent at 40 °C
Not directly proportional
Directly proportional
Indirectly proportional
Multiply each side of the equation by the number of moles.
Divide each side of the equation by the number of moles.
Add the number of moles to each side of the equation.
An ideal volumn
An ideal mass
An ideal gas
The number of moles must be constant, n1 lower = n 2 lower , for all three of these gas laws.
The number of moles must be constant, n2 lower = n 2 lower , for all three of these gas laws.
The number of moles must be constant, n1 lower = n 3 lower , for all three of these gas laws.
Knowing the gas constant, T, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.
Knowing the gas constant, R, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.
Knowing the gas constant, n, and the ideal gas Saw, P x V = n x R x T lets you calculate the number of motes of gas at any specified values of P, V, and T.
Gas laws
Liquid laws
Solid laws
Solid
Liquid
Gas
The combined solid law
The combined liquid law
The combined gas law
Boy|e's law
Charles's law
Gay-Lussac's law
Boy|e's law
Charles's law
Gay-Lussac's law
Boy|e's law
Charles's law
Gay-Lussac's law
Temperature
Liquid
Solid
Pressure times volume is constant. This relationship illustratesGay-Lussac's law .
Pressure times volume is constant. This relationship illustrates Charles's law.
Pressure times volume is constant. This relationship illustrates Boyle's law.
Negative one
Absolute zero
zero
When one variable decrease, the other increases so that the ratio of the two variables remains constant.
When one variable increases, the other increases so that the ratio of the two variables remains constant.
When one variable increases, the other increases so that the amount of the two variables remains constant.
Mass
Volumn
Circumference
Boyle temperatue
Kelvin temperature
Chsrles temperature
Boyle's Scale
Kelvin's Scale
Gay's Scale
The average kinetic energy of gas particles and their Kelvin temperature are directly proportional.
The average kinetic energy of gas particles and their Gay temperature are directly proportional.
The average kinetic energy of gas particles and their Lussac temperature are directly proportional.
When the pressure increases, the volume increases. When the pressure decreases, the volume decreases.
When the pressure increases, the volume decreases. When the pressure decreases, the volume increases.
When the pressure decreases, the volume decreases. When the pressure icreases, the volume increases.
An inverse relationship occurs when one variable increases as the other increases.
An converse relationship occurs when one variable increases as the other decreases.
An inverse relationship occurs when one variable increases as the other decreases.
Boyles
Gay
Kelven