CHEM 1B Lecture Notes - Lecture 2: Mole Fraction, Electric Light, Amedeo Avogadro

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13 Jan 2018

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Jacques charles studied the relationship between temperature and volume of gas. Example: a sample of carbon monoxide gas occupies at 3. 20 l at 125 c. Example: a gas occupies a volume of 946 ml of at a pressure of 726 mmhg. P2 = p1v1 = (726 mmhg)(946 ml) Amedeo avogadro observed a linear relationship between the amount of gas and volume it occupies at a constant temperature and pressure. The nature of gas doesn"t matter (ideal gas approximation) Boyle"s law: v 1/p (at constant t and n) Charles"s law: v t (at constant p and n) Avogadro"s law: v n (at constant p and t) V= constant x nt = rnt (r is gas constant; 0. 08205 lxatm/kmol or. Standard temperature = 273. 15 k = 0 c. Standard molar volume: volume occupied by 1 mole of a substance at stp. V= (1mol) x (0. 082057 atmxl/kmol) x (273. 15 k) Aso used: standard ambient temperature and pressure conditions (satp)

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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

1. A sample of gas in a balloon has an initial temperature of 8.0 ?C and a volume of 1.19Ã10³ L . If the temperature changes to 62 ?C , and there is no change of pressure or amount of gas, what is the new volume, V2, of the gas?

2. What Celsius temperature, T2, is required to change the volume of the gas sample in Part A (T1 = 8.0 ?C , V1= 1.19Ã10³ L ) to a volume of 2.38Ã10³ L ? Assume no change in pressure or the amount of gas in the balloon.

3. A sample of ideal gas is in a sealed container. The pressure of the gas is 525 torr , and the temperature is 45 ?C . If the temperature changes to 59 ?C with no change in volume or amount of gas, what is the new pressure, P2, of the gas inside the container?

4. Using the same sample of gas (P1 = 525 torr , T1 = 45 ?C ), we wish to change the pressure to 5250 torr with no accompanying change in volume or amount of gas. What temperature T2, in Celsius, is needed to reach this pressure?

5. A very flexible helium-filled balloon is released from the ground into the air at 20. ?C. The initial volume of the balloon is 5.00 L, and the pressure is 760. mmHg. The balloon ascends to an altitude of 20 km, where the pressure is 76.0 mmHg and the temperature is ?50. ?C. What is the new volume, V2, of the balloon in liters, assuming it doesn't break or leak?

6. Consider 4.60 L of a gas at 365 mmHg and 20. ?C . If the container is compressed to 2.60 L and the temperature is increased to 32 ?C , what is the new pressure, P2, inside the container? Assume no change in the amount of gas inside the cylinder.

.44 The compressed air tank of a scuba diver reads 3,200 psi at the beginning of a dive and 825 psi at the end of a dive. Convert each of these values to atm and mmHg. 6.48 If someone takes a breath and the lungs expand from 4.5 L to 5.6 L in volume, and the initial pressure was 756 mmHg, what is the pressure inside the lungs (in mmHg) before any additional air is pulled in? 6.52 How hot must the air in a balloon be heated if initially it has a volume of 750. L at 20.oC and the final volume must be 1,000. L? 6.56 If a plastic container at 1.0oC and 750. mmHg is heated in a microwave oven to 80.oC, what is the pressure inside the container (in mmHg)? 6.58 Assuming a fixed amount of gas, complete the following table: ï¿¼ ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ P1 V1 T1 P2 V2 T2 ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ a. 0.55 atm 1.1 L 340 K ? 3.0 L 298 K ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ 0.0oC b. 735 mmHg 1.2 L 298 K 1.1 atm ? ï¿¼ ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼ï¿¼Ì¶ 120oC c. 7.5 atm 230 mL 15 atm 0.45 L ? ï¿¼ï¿¼6.62 Calculate the volume of each substance at STP. a. 4.2 mol N2 b. 6.5 g He c. 22.0 g CH4 6.64 What volume does 1.50 ï´ 1024 molecules of CO2 occupy at STP? 6.66 How many moles of gas are contained in a compressed air tank for scuba diving that has a volume of 7.0 L and a pressure of 210 atm at 25oC? 6.68 If a cylinder contains 10.0 g of CO2 in 10.0 L at 325 K, what is the pressure? 6.74 If the pressure due to the striped spheres in the molecular art is 480 mmHg, what is the pressure due to the spotted spheres? What is the total pressure of the system? ï¿¼

CHEM 1B Lecture Notes - Lecture 2: Mole Fraction, Electric Light, Amedeo Avogadro

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