Gases

kinetic molecular, matter, motion, ideal, imaginary, assumptions, high, low

The Kinetic Molecular Theory • The ________ _______ Theory is based on the idea that particles of ______ are always in ______. • The theory provides a model of what is called an ______ gas. • An ideal gas is an ________ gas that perfectly fits all the _______ of the KMT. Ideal gases have _____ pressure & ______ temperature.

ideally, obey, real, assumptions, kmt

The Kinetic Molecular Theory • When particles are far enough apart and have enough kinetic energy, most gases behave _______. • Not all gases _____ the KMT. All ____ gases deviate to some degree from ideal gas behavior. • A real gas is a gas that does not behave completely according to the ________ of the _____.

temperature, pressure, volume, amount

The Kinetic Molecular Theory The KMT is based on 4 factors: _____________, ____________, ____________, and ___________

standard temperature and pressure (STP)

0 °C or 273 K Agreed upon standard conditions of exactly 1 atm and pressure of 0 c Standard temperature is equal to 0 °C, which is 273.15 K. Standard Pressure is 1 Atm, 101.3kPa or 760 mmHg or torr. STP is often used for measuring gas density and volume. At STP 1 mole of any gas occupies 22.4L.

a

As the pressure on a given sample of gas increases at constant temperature, the volume of the sample a) decrease b) cannot determine c) increases d) remains the same

d

At what temperature would the molecules of a gas have the greatest average kinetic energy? a) 10°C b) 50°C c) 0°C d) 100°C

K, P, V, n, kelvin, 273, atm, 1, kPa, 101.3, mmHg, 760, torr 760, liter, 22.4, moles

Symbol- Temperature: ___ Pressure: ___ Volume: ___ Amount: ___ Unit and Value standard: Temperature: __________ (_______) (conversion K= C° + 273) Pressure: ________ (________), _________ (________), _________ (_________), ___________ (___________) Volume: __________ (________) Amount: ___

5, small, volume, elastic, kinetic, constant, random, not, average, temperature

The Kinetic Molecular Theory (A ideal gas would follow all of these) The KMT is based on ___ assumptions: 1. Gas particles are _____; virtually no ______ 2. Gas particles have ______ (constant) collisions (no loss of ______ energy) 3. Gas particles are in _______, ________ motion 4. Gas particles do ______ attract or repel one another. 5. The ______ kinetic energy of gas particles depends on the _________

motion, directly

The Kinetic Molecular Theory • Kinetic Energy: Energy in ______ • The Kinetic Energy for gases is _________ proportional to temperature. ↑KE = ↑Temp

kinetic theory of gas

- Gases are made of very small particles, separated by large volumes of empty spac Matter is made up of tiny, invisible moving particles; particles of difference substances have different sizes; lighter particles move faster than heavier ones at a particular temperature; as the temperature rises, particles move faster. submicroscopic particles of matter are in constant, random motion

boyle, constant, inverse,

2. ________'s Law • Temperature is held ________ • _______ relationship between pressure & volume (↑V=↓P and ↓V=↑P) • P₁V₁=P₂V₂ 1) If the pressure of helium in a balloon has a volume of 4.0 L at 210 kPa, what will the pressure be at 2.5 L? a) V₁= 4.0 L P¹= 210 kPa V₂= 2.5 L P₂= ? b) P₁V₁= (P₂)V₂ looking for P₂, so divide by V₂ to get it alone c) P₁V₁=P₂V₂ ___________ V₂ d) P₁V₁=P ______ V₂ e) Plug in P₁, V₁, and V₂ and solve for P₂ f) P₂= 4.0 L X 210 kPa ___________________ 2.5 L g) P₂= 336 kPa

combined gas, gas

5. The _________ _____ Law • Amount of ____ (# molecules) is held constant • P₁V₁= P₂V₂ ⁻⁻⁻⁻⁻⁻⁻⁻⁻ ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ T₁ T₂ • Which three laws combine to make this law? Charles', Gay Lussac, Boyle A gas at 110kPa and 30°C fills a container at 2.0 L. If the temperature rises to 80oC and the pressure increases to 440 kPa, what is the new volume? a) V₁= 2.0L P₁= 110kPa T₁= 30°C---> 303K V₁=440kPa P₁= ? T₁= 80°C---> 353K b) Put in formula (110kPa)(2.0L) (440kPa) (V₁) ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ = ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ (303K) (353K) c) Multiply the side that has all its values 110 x 2= 220 divide by 303= .7260 d) .7260= (440kPa) (V₁) ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ Multiple both sides by→ (353K)← this would cross this out e) (353) .7260 =(440kPa) (V₁)= Now divide by 440 to get V₁ alone 256.303= (440kPa) (V₁) ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ (440kPa) f) V₁= .58L

c

A real gas would behave most like an ideal gas under considerations of a) low pressure and low temperature b) low pressure and high temperature c) high pressure and low temperature d) high pressure and high temperature

c

A sample of gas A was stored in a container at a temperature of 50ºC and a pressure of 0.50 atmosphere. Compared to a sample of gas B at STP, gas A had a A: 323K, .50 atm B: 273 K, 1 atm a) lower temperature and a lower pressure b) higher temperature and a higher pressure c) higher temperature and a lower pressure d) lower temperature and a higher pressure

torr

A unit of pressure equal to 1mmHg; 760 torr=1 atm A unit of measure for the pressure exerted by 1 mm of mercury, equal to 1/760th of standard atmospheric pressure

average kinetic energy

Gas particles at the same temperature have the same... Directly proportional to the Kelvin temperature of a substance

boyle's law

Pressure and volume have an inversly proportional relationship P₁V₁=P₂V₂ at a constant temperature the pressure of a fixed amount of gas is inversely proportional to its volume

ideal gas, presure, r, volume, moles, gas constant, temperature

The _______ ______ Law • Contains all variable • PV=nRT - P = ________ (depends on __) - V = _______ (liters) - n = number of ______ - R = ___ ________ (depends on P) - T = ________ (Kelvin) Gas Constant: Unit of pressure (R) atm: 0.0821 L X atm / Mol X K mmHg or Torr: 62.4 L X mmHg / Mol X K kPa: 8.314 L x kPa / Mol X K 1) Calculate the moles of a gas at STP with a volume of 238 L. a) P= 1 atm V= 238L n=? T=273K R= .0821 L X atm / Mol X K b) PV= n ⁻⁻⁻⁻⁻⁻⁻⁻⁻ RT c) Flip R so you can cancel out all the units execpt mole n= (1 atm) x (238L) mol x K ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ X ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ (273K) .0821 L x atm d) simplify 238 mol / 22.4133 c) n= 10.62 mol

c

The average kinetic energy of the molecules of an ideal gas is directly proportional to the a) number of moles present b) volume occupied by the individual gas mlcs c) temperature measured in Kelvin d) pressure at standard temperature

ideal gas

The theoretical gas that the Kinetic Molecular Theory centers around is the ___ ___ a mathematical relationship among pressure, volume, and temperature and number of moles of gas A law that combines the four properties of a gas - pressure (P), volume (V), temperature (T), and number of moles (n) in a single equation showing their interrelatedness PV=nRT

charles' law

V₁/T₁ = V₂/T₂ The volume of a fixed mass of gas at constant pressure varies directly with the Kevin temperature

volume

What does v represent? If the pressure and temperature of a gas are held constant and some gas is added to the container or some is allowed to escape, a change is which of the following can be observed?

b

When a sample of a gas is heated at constant pressure, the average kinetic energy of its molecules a) dec, and the volume inc b) inc, and the volume of the gas inc c) inc, and the volume of the gas dec d) dec, and the volume of the gas dec Why:average kinetic energy= temperature When pressure is constant, then temperature and volume are directly related

gay lussac

Whose law shows a directly proportional relationship between pressure and temperature?

gay lussac, volume, direct

_____ _________'s Law • _______ is held constant • _______ relationship between pressure & temperature • P₁/ T₁ = P₂/T₂ (Like Charles' law if you have to find T you would take the bottom and divide by the top, even though it seems weird) 1) The pressure of a gas in a tank is 3.2 atm at 22°C. If the temperature rises to 60°C, what will be the pressure in the tank? a) P₁= 3.2atm T₁=22°C<--- (+273)= 295 K P₂=? T₂=60°C<-----(+273)= 333K b)(T₂/1) P₁ = P₂ Look for P₂ ________ T₁ T₂ <---- Cross multiply to cross out T₂ c) P₁ X T₂ __________= P₂ T₁ d) 3.2 atm X 333K ______________= P₂ ------> 3.61atm 295K

dalton's law of partial pressure,pressure, unit

______'s ______ ___ ________ __________: • Contains only _______ • All pressure values must be in the same _____ • PT = P1 + P2 + P3... 1)If the total pressure of a mixture of oxygen & nitrogen gases was 820 mmHg, how much pressure would nitrogen exert if oxygen had 580 mmHg? Total- 820 mmHg Oxygen- 580 mmHg Nitrogen- ? 820-580= 240 Nitrogen= 240 mmHg 2) A mixture of oxygen, hydrogen, and nitrogen gases exert total pressure of 278 kPa. If the partial pressures of the oxygen and the hydrogen are 112 kPa and 101 kPa respectively, what would be the partial pressure exerted by the nitrogen? O + H= 112 + 101= 213 278- 213= 65 Nitrogen= 65 kPa 3) A container hold three gases: oxygen, carbon dioxide, and helium. The partial pressures of the three gases are 200 torr, 300 torr, and 400 torr respectively. What is the total pressure inside the container? 200 + 300 + 400= 900 PT= 900 Torr

charles, pressure, direct

_______' Law • _________ is held constant • _______ relationship between temperature & volume • V₁/T₁ = V₂/ T₂ 1) A gas sample at 40°C occupies a volume of 2.32 L. If the temperature is increased to 75°C, what will be the final volume? a) V₁= 2.32L T₁= 40°c--> (+273)= 313 V₂= ? T₂= 75°C---> (+273)= 348 b) (T₂/1) V₁ = V₂ Look for V₂ by cross multiplying. __________ T₁ T₂ <--- cross this out c) T₂ x V₁ = V₂ _______ T₁ d) 348 X 2.32 = V₂ ----------> 2.58L ___________ 313 2) A gas system has an initial volume and temperature of 14000L and 366.4K. If the volume changes to 200mL, what will the resultant temperature be in K? a) V₁= 14000L T₁= 366.4K V₂= 200mL T₂= ? b) V₁ = V₂ <--- Cross multiple to get T₂ alone ___________ (1/V₂) T₁ T₂ Look for T₂ by cross multiplying. c) V₁ _____=V₂ V₂ X T₁ D) 14000mL _____________= 14000/ 73280 366.4K X 200mL E) Even though 14000 is above 73280 you divide 73280 by 14000= 5.23 K If it asks for °C, you would take the K and subtract 273 to get °C

real gas

a gas that does not behave completely according to the assumptions of the kinetic-molecular theory (particles exert attractive forces on each other)