CHM 111 Lecture Notes - Lecture 12: Van Der Waals Equation, Ideal Gas Law, Kinetic Theory Of Gases

44 views1 pages

Verified Note

bronzeclam342

28 Sep 2018

School

Department

Course

Professor

For unlimited access to Class Notes, a Class+ subscription is required.

CHM 111 verified notes

12/31View all

CHM 111 Lecture 11: CHM 111 lecture #11

CHM 111 Lecture Notes - Lecture 12: Van Der Waals Equation, Ideal Gas Law, Kinetic Theory Of Gases

CHM 111 Lecture Notes - Lecture 13: Valence Electron, Lewis Acids And Bases, Nonmetal

Document Summary

Definition: volume of 1 mole at stp (ideal gas equation results in 22. 4 l) Density at standard conditions: density calculation: d=m/v or d=pmm/rt. Mm= molar mass: molar mass calculation: mm=drt/p. Mixture of gases: where v and t are constant, the gas molecules behave independently when mixed together, ptotal = p1 + p2. (p stands for pressure) Reactions involving gases: think back to stoichiometry and combine it with the ideal gas law, the ideal gas law can be used to convert from the amount of gas (volume) to moles. Kinetic energy and molecular velocities: equation for kinetic energy: ke= . 5mv2. If gases have different masses, the average velocity must be the same in order to have the same kinetic energy. This equation accounts for molecular volume and intermolecular attraction: [p + (a(n/v)2)] x [v nb] = nrt.

Related Questions

Boyles Law

a) A10.0 L sample of a gas at 25oC and 1.5 atm iscompressed at constant temperature to a volume of 1.0 L. What isthe new pressure?

b) A3.5 L sample of a gas at 1.0 atm is expanded at constanttemperature until the pressure is 0.10atm. What is the volume of the gas?

Charless Law

a) A2.5 L sample of gas at 25oC is heated to50oC at constant pressure. What is the finalvolume?

b) Whattemperature would be required to increase the volume from 2.5 L to6.0 L?

Avogadros Law

a) Assumingno change in temperature and pressure, how many moles of methane(CH₄) need to be added to 0.50 moles of methane todouble the volume?

b) 50g of solid carbon dioxide evaporates to carbon dioxide gas atstandard temperature and pressure. What isthe volume of carbon dioxide gas?

Combined Gas Laws

Calculate the temperature when a 0.50 L sample of gas at 1.0 atmand 25oC is compressed to 0.05 L of gas at 5.0atm.

Ideal Gas Law

a) Whatis the volume of gas occupied by 10.0 g CH4 at37oC and 4 atm?

b) Whatis the mass of N2 required to occupy 5.0 L at80oC and 560 mmHg?

Molar Density of Gases

a) Whatis the density of He at STP?

b) Whatis the density of carbon dioxide at 120^oC and 1.5atm?

Application of Gas Laws:

a) How many grams ofNO₂, nitrogen dioxide, are contained in 0.500 L of thegas at STP?

b) Calculate thedensity of NO₂ gas, in grams per liter, at 110C and 12atm.

c) Calculate the molarmass of a gas if 0.125 g of the gas occupies 93.3 mL at STP.

d) On a spring morning(15C) you fill your tires to a pressure of 2.25 atmospheres. As youride along, the tire heats up to 45C from the friction on the road.What is the pressure in your tires now?

e) What volume ofH₂ is formed at STP when 6.0 g of Al is treated withexcess NaOH?

2NaOH+ 2Al + 6H₂O 2NaAl(OH)₄ +3H₂(g)

Application of Gas Law

a) Whatis the effect on the volume of an ideal gas when the temperature isdecreased from 700K to 350K at constant pressure?

b) Whatis the effect on the volume of an ideal gas when both the pressureand temperature are reduced by half?

c) Whatis the effect on the volume of an ideal gas when the pressure ischanged from 722 torr to 0.950 atm, and the temperature is changedfrom 5^oC to 273 K?

Stoichiometric Relationships

a) Howmany grams of phosphorus react with 35.5 L of O₂ at STPto form tetraphosphorus oxide, according to the following reactionequation?

P₄ (s) + 5 O₂ (g)P₄O₁₀ (s)

b) Ammonia decomposes to nitrogen and hydrogen when in thepresence of heated steel wool. What is thefinal volume of the gas when 45 g of ammonia decomposes at150^oC and 1 atm pressure. Writea balanced equation before you start your calculations!

Daltons Law of Partial Pressures

a) A sample of a natural gas contains 8.24 moles of methane(CH₄), 0.421 mole of ethane(C₂H₆), and 0.116 mole of propane(C₃H₈). If the totalpressure of the gases is 1.37 atm, what are the partial pressuresof the gases?

b) Earths atmosphere consist of 78% N₂and 20%O₂, and other gases. What is the partial pressure ofN₂ and O₂intorr, when the atmospheric pressure is 1 atm?

c) Ammonia is completely decomposed to nitrogen and hydrogen, asin question 9b). At the end of theexperiment the pressure of the gas mixture is 866mmHg. Calculate the partial pressures ofN₂ and H₂.

Question 11 pts

Which general statement about gases is NOT correct?

The molecules of a pure gas are distributed evenly throughout the container.

Gases are much less dense than liquids or solids

Molecules in a gas mixture can form layers according to their densities

Gases can be compressed, even to the point of liquefaction

Flag this Question

Question 21 pts

Which example is the greatest pressure?

1.00 atm

101 kPa

760 mm Hg (= 760 torr)

All of the above pressures are equal.

Flag this Question

Question 31 pts

Which example is the greatest pressure?

850 mm Hg (= 850 torr)

1.5 atm

All of the above pressures are equal.

96 kPa

Flag this Question

Question 41 pts

Assuming all other variables are held constant, a graph of which of the following will NOT yield a straight line?

Flag this Question

Question 51 pts

A sealed vessel contains 0.250 mol of oxygen gas. Which of the following will result in a decrease in the pressure of the oxygen gas?

increasing the number of moles of oxygen

increasing the temperature of the vessel

increasing the volume of the vessel

adding some helium to the vessel

Flag this Question

Question 61 pts

According to Charlesâs law, which change will cause the pressure of a gas to double? Pressure and amount of gas are constant.

The temperature decreases from 650 K to 325 K.

The temperature of the sample decreases fromï¿½88 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½22 Â°C to 44 Â°C.

The temperature of the sample increases fromï¿½250 K to 500 K.

Flag this Question

Question 71 pts

Which set of units for P, V, and T can be used for combined gas law calculations?

torr, L, and Kelvins

tm, g/L, and Kelvins

atm, mL, and degrees Celsius

inches of mercury, g/mL, and degrees Celsius

Flag this Question

Question 81 pts

The vapor pressure of a gas is

the atmospheric pressure at which the boiling point is determined.

the pressure at a Kelvin temperature exactly two times the boiling point.

impossible to determine experimentally without knowing the temperature and volume.

the pressure above a gas sample when evaporation and condensation are balanced.

Flag this Question

Question 91 pts

In a chemistry experiment where CO2 is collected over water, the atmospheric pressure is 755 mm. The partial pressure of water at the temperature in the lab is 24.2 mm. What is the pressure of the CO2?

779 mm

731 mm

More information is needed to answer this question

755 mm

Flag this Question

Question 101 pts

Which statement is NOT true according to the kinetic molecular theory of gases?

Molecules undergo elastic collisions

Molecules move in straight-line paths.

Molecules of different gases have differentï¿½kinetic energies at the same temperature

Molecules occupy a negligible volume.

Flag this Question