If 22.5L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?2. A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant? 3. What pressure is required to compress 196.0 litersof air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?4. A 40.0 L tank of ammonia has a pressure of 12.7 kPa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kPa while its temperature remains constant. 5.4. If a syringe is filled with 100 mL of air at 1 atm, how much pressure must be applied to reduce the volume to 60 mL?

Question

Chemistry

Billy Mccullough

2 June, 23:43

If 22.5L of nitrogen at 748 mm Hg are compressed to 725 mm Hg at constant temperature. What is the new volume?2. A gas with a volume of 4.0L at a pressure of 205kPa is allowed to expand to a volume of 12.0L. What is the pressure in the container if the temperature remains constant? 3. What pressure is required to compress 196.0 litersof air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters?4. A 40.0 L tank of ammonia has a pressure of 12.7 kPa. Calculate the volume of the ammonia if its pressure is changed to 8.4 kPa while its temperature remains constant. 5.4. If a syringe is filled with 100 mL of air at 1 atm, how much pressure must be applied to reduce the volume to 60 mL?

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Answers (1)

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River · Answer 1

a) 23.2 L

b) 68.3kPa

c) 7.5 atm

d) 60.5L

e) 1.67 atm

Explanation:

From Boyle's law:

P1V1=P2V2

P1 = 748mmHg

P2=725mmHg

V1 = 22.5L

V2?

V2 = P1V1/P2 = 748*22.5/725 = 23.2 L

b)

V1=4.0L

P1 = 205*10^3Pa

V2 = 12.0L

P2=?

P2 = P1V1/V2 = 205*10^3*4/12

P2 = 68.3*10^3 Pa or 68.3kPa

c)

P1 = 1 atm

V1 = 196.0L

P2=?

V2 = 26.0L

P2 = P1V1/V2=1*196.0/26.0

P2 = 7.5 atm

d)

V1 = 40.0L

P1 = 12.7*10^3Pa

V2=?

P2 = 8.4*103Pa

V2 = P1V1/P2 = 12.7*10^3*40.0/8.4*103

V2=60.5L

e)

V1 = 100mL

P1 = 1atm

V2 = 60mL

P2=?

P2 = P1V1/V2 = 1*100/60

P2 = 1.67 atm