CHEM 111A Chapter Notes - Chapter 5: Novella, Kinetic Theory Of Gases, Van Der Waals Equation

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coppermanatee242

4 May 2017

School

CSULB

Department

Chemistry and Biochemistry

Course

CHEM 111A

Professor

Andrea Chen

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Document Summary

Ideal gas equation: boyle"s law: p1v1 = p2v2, charles"s law: v1/t1 = v2/t2, avogadro"s law: v1/n1 = v2/n2. Zn(s) + 2hcl(aq) zncl2(aq) + h2(g: 1. 02 l of o2 collected over water at 293 k with a total pressure of 755. 2 mmhg. Find the mass of o2 (14: 0. 12 moles h2 is collected over water in a 10. 0 l container at 323 k. find the total pressure (15) Co(g) + 2h2(g) ch3oh(g) (16: what volume of o2 at 0. 750 atm and 313 k is generated by the thermolysis of 10. 0 g of. Hgo? (17: how many grams of water form when 1. 24 l of h2 gas at stp completely reacts with. O2? (18: stp eliminates the need to use pv = nrt. Properties of gases: expand to completely fill their container, take the shape of their container, have low density, much lower than solid or liquid states, are compressible, mixtures of gases are always homogenous, fluid.

Related Questions

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

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

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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.

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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

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Question 41 pts

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

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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

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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.

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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

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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.

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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

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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.

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