CHEM 24112 Lecture Notes - Lecture 34: Diborane, Torr, Gas Constant

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CHEMISTRY 112 – DAY 34 Chapter 13: Sections 3-5

4/13/18

CHARLES’ LAW, AVOGADRO’S LAW, IDEAL GAS LAW, AND COMBINED GAS LAW

Charles’s Law

Volume and Temperature (in Kelvin) are directly related (constant P and n).

V=bT (b is a proportionality constant)

K = °C + 273

0 K is called absolute zero.

TEMPERATURES ALWAYS MUST BE IN KELVIN WHEN USING THE GAS LAWS!!

EXAMPLE 1: A 2.0 L sample of air is collected at 298 K and then cooled to 278 K. The pressure is held constant

at 1.0 atm. Does the volume increase or decrease? Calculate the volume of the air at 278K.

EXAMPLE 2: A sample of gas at 15oC (at 1 atm) has a volume of 2.58 L. The temperature is then raised to 38oC

(at 1 atm) Does the volume increase or derease? Calculate the new volume.

EXAMPLE 3: Consider a gas that has a volume of 0.675 L at 35oC and 1 atm pressure. What is the temperature

(in units of oC) of a room where this gas has a volume of 0.535 L at 1 atm pressure?

Avogadro’s Law

Volume and number of moles are directly related (constant T and P).

V = an (a is a proportionality constant)

EXAMPLE 4: If 2.55 moles of helium gas occupies a volume of 59.5 L at a particular temperature and pressure,

what volume does 7.83 moles of helium occupy under the same conditions?

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Document Summary

Charles" law, avogadro"s law, ideal gas law, and combined gas law. Volume and temperature (in kelvin) are directly related (constant p and n). Temperatures always must be in kelvin when using the gas laws! Example 1: a 2. 0 l sample of air is collected at 298 k and then cooled to 278 k. the pressure is held constant at 1. 0 atm. Calculate the volume of the air at 278k. Example 3: consider a gas that has a volume of 0. 675 l at 35oc and 1 atm pressure. Volume and number of moles are directly related (constant t and p). V = an (a is a proportionality constant) Example 5: consider two samples of nitrogen gas (at the same temperature and pressure). 1. 5 moles of n2 and has a volume of 36. 7 l. sample 2 has a volume of 16. 5 l. calculate the number of moles in. Pv = nrt (where r = 0. 08206 l atm/mol k, the universal gas constant)

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

Breathing is an application of Boyleâs law (Figure 10.8). As the diaphragm muscle beneath our lungs contracts, the pressure inside our lungs decreases causing air to rush into our mouth and nasal passages to fill the lungs. When the diaphragm muscle relaxes, it increases the air pressure causing air to be expelled from the lungs. A typical lung volume is 3.50 L. Air pressure inside the lungs changes by approximately 0.040 atm. A sample of air has a volume of 3.50 L at 1.00 atm. What is the volume of this air sample if the pressure is changed to 0.960 atm at constant temperature? This question gives an initial gas pressure and volume then asks for the new gas volume at a different pressure at constant temperature and gas amount. These are indicators to use Boyleâs law.

What is the volume (in liters) of this air sample if the pressure is changed to 0.960 atm at constant temperature?

1)a volume (54.2 L) of gas at 115 K is heated to 345 K, at constant pressure. what volume does the gas occupy now.

2)The temperature of a 0.750-L gas sample at 25 Â°C and 2.00 atm is changed to 250 Â°C. What is the final pressure of the system, at constant volume?

3)A sample of neon gas has a volume of 7.2 mL at a pressure of 1.50 atm. What is the pressure exerted by the gas if the volume is increased to 28.8 mL, at constant temperature?

CHEM 24112 Lecture Notes - Lecture 34: Diborane, Torr, Gas Constant

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