CHM135H1 Lecture Notes - Lecture 7: Gas Constant, Ideal Gas Law, Intermolecular Force

104 views3 pages

Verified Note

limerhinoceros188

22 Sep 2018

School

UTSG

Department

Chemistry

Course

CHM135H1

Professor

Gilbert Walker, Eugenia Kumacheva, Kristine Quinlan

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

CHM135H1 verified notes

7/38View all

CHM135H1 Lecture 6: Lecture 5 Electronic Structure of Atoms Continued

CHM135H1 Lecture Notes - Lecture 7: Gas Constant, Ideal Gas Law, Intermolecular Force

CHM135H1 Lecture 8: Bonding+Gases-Notes(2018-09-21)

Document Summary

September 21, 2018 (relevant reading chemistry 7ed mcmurray/fay/robinson chapter 10. 1-10. 6, What determines the phase of matter: molecular level, structure, dynamics (motion) Intramolecular forces: macroscopic level, properties, solid, liquid, gas. Pressure: = (cid:4666)(cid:3040)(cid:3118)) force applied over an area. Units si: pa = n/m2; kpa = 103pa. Common: 1atm = 101. 3 kpa = 760 mmhg = 760 torr. P, t, v, n (number of moles) all interrelated. At standard temperature and pressure stp (273 k and 1atm): 1 mol gas = 22. 5l gas. Charles law at constant pressure, volume of a fixed amount of gas is proportional to absolute. Avogadro"s law at fixed temperature and pressure, volume of gas is proportional to amount of. Pv = nrt; r = universal gas constant 0. 08206 l atm mol-1k-1. A gas behaves ideally at high temperatures and low pressure (when molecules don"t interact and their molecular volume is negligible. Gas stoichiometry: o2 gas is made in the lab by the thermal decomposition of potassium chlorate.

Related Questions

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

Question 111 pts

Which statement is NOT true according to the ideal
gas law?

At constant P & T, V must increase when n increases.

At constant V & T, P must decrease when n decreases.

At constant V & n, P must increase when T increases.

At constant P & n, V must decrease when T increases

1. The number of molecules in 1atm of gas at constant pressure and temperature is identical,regardless of the identity of the molecules in the gas. Which ofthe following other statements are also true?

A) The molecules in a gas slow down with increasingtemperature.
B) The total number of atoms in the gas at standard temperature andpressure can vary depending on the identity of the gas
C) The volume of a gas is independent of the pressure of thegas.
D) The temperature of a gas is independent of the pressure of thegas.

2. In an ideal gas, P*V = n*R*T where P = pressure, V=volume,n=number of moles, R=gas constant, and T=temperature. Consider agas with pressure = 1 atm, 1 mole of molecules, and a temperatureof 295 K. R=0.082 atm*L/(mol * K). How much volume should this gasoccupy? Choose the closest answer.

A) 1.0 L
B) 30.6 L
C) Infinite space
D) 22.4 L

3. Suppose you conducted an experiment using Helium gas. Giventhat Helium is much lighter than Propane and Butane, you wouldexpect the relationship between the volume of helium and thepressure to be:

A) exponential, because Helium is lighter
B) inversely proportional, just like propane and butane
C) directly proportional, just like propane and butane
D) periodic, because Helium is lighter

4. What do you predict would happen if you conducted anexperiment using sulfur hexafluoride (SF6) which is much heavierthan methane or butane?

A) The volume of SF6 would be larger and this would affect thepressure in the flask
B) The relationship between temperature and volume would beinversely proportional for a gas of higher molecular weight
C) The speed of the SF6 gas molecules would be faster causing adifference in the temperature measurements
D) The relationship between temperature and volume would bedirectly proportional just as it was for methane and butane

Part 1 Boyle’s Law P1 V1 = P2 V2 when Temperature is constant; being 1 “initial” and 2 “final” A container of oxygen gas has a volume of 150 mL when its pressure is 0.947 atm. If the temperature remains constant. What will the volume of the gas be at a pressure of 0.987 atm? Using Boyle’s Law solve for V2 of final volume using P1 V1 = P2 V2 Match the correspondent given data, unknown data and resulted in data after solved

___1. Initial Volume or V1

___2. Final Pressure or P2

___3. Initial pressure or P1

___4. Final V2

___5 Temperature

A. does not change, remains constant

B. 144 mL of oxygen

C. 0.947 atm

D. 150 mL of oxygen

E. 130 mL of oxygen

F. 0.987 atm

Part 2 Charles’s Law V1/T1=V2/T2 when the Pressure is constant; being 1 “initial” and 2 “final A container with hydrogen gas has a volume of 349 mL, at a temperature of 22.0C (Change to K), What volume will the gas occupy at 50C(Change to K), if the pressure remains constant?

____6. Final Volume of gas

____7 Initial Temperature gas

____8. Final Temperature gas

____9. Initial Volume gas

____10. The pressure of hydrogen

G. It’s constant

H. 295 K

I. 349 mL

J. 382 mL

K. 323 K

L. 50 C

Part 3 Gay-Lussac Law P1/T1=P2 when the volume (V) is constant A cylinder of a gas has a pressure of 4.40 atm at 25C (Change to K). At what temperature in Celsius will it reach a pressure of 6.50 atm C= K-273

____11. Final Pressure of gas (P1)

____12. The initial temperature in K (T1)

____13. The initial Pressure of gas (P2)

____14. The volume of the gas

_____15. The final temperature of the gas

M. 6.50 atm

N. 298 K

O. 4.40 atm

P. 167 C

Q . 283 K

R. is constant

Part 4 Combined Gas Law P1 V1/ T1 = P2 V2/ T2 OR MORE EASY TO SOLVE P1 V1 T2= P2 V2 T1 A St. Valentine Helium-filled balloon for your love, has a volume of 50.0 mL at 25 C (change to K) and 1.08 atm. What volume(V2) will it have at 0.855 atm and 10.0C (change to K). K=C + 273

_____16. The Final Temperature in K (T1)

_____17. The initial Volume in mL (V1)

_____18. The final Pressure in atm (P2)

_____19. The initial temperature in C (T1)

_____20. The final volume (V2)

S. 298k

T. 50.0 mL

U. 0.855 atm

V. 25 C

W. 283 K

X. 60.00 mL

Part 5 Answer with the letter in the blank. A. Boyles’s Law B. Charles’s Law C. Gay-Lussac’s Law D. Combined Gas Law E. Avogadro’s Law

___21. One mol of any gas at Standard Temperature and Pressure contains 6.03 X10^23 molecules and occupy a volume of 22.4L

____22. The higher the pressure the lower the volume when the temperature is constant.

____23. The higher the temperature the higher the volume when the pressure is constant.

____24 The higher the temperature the higher is the pressure when the volume is constant.

____25. There is a relation between pressure, volume, and temperature of a fixed amount (moles)of gas

coffeeelephant81

CHM135H1 Lecture Notes - Lecture 7: Gas Constant, Ideal Gas Law, Intermolecular Force

CHM135H1 Lecture 6: Lecture 5 Electronic Structure of Atoms Continued

CHM135H1 Lecture Notes - Lecture 7: Gas Constant, Ideal Gas Law, Intermolecular Force

CHM135H1 Lecture 8: Bonding+Gases-Notes(2018-09-21)

Document Summary

Get access

Related Documents

CHM135H1 Lecture Notes - Lecture 8: Gas Constant, Chlorate, Intermolecular Force

CHM135H1 Chapter Notes - Chapter 9 - 11: De-Ice, Molality, Pennsylvania Route 100

CHM135H1 Lecture Notes - Lecture 6: Kelvin, Gas Constant, L Source

Related Questions