In A Nitrogen Gas Occupies Has A Volume Of 500ml At A Pressure Of 0.971 Atm. What Volume Will The Gas Occupies At A Pressure Of 1.50 Atm, Assuming The

In a nitrogen gas occupies has a volume of 500ml at a pressure of 0.971 atm. What volume will the gas occupies at a pressure of 1.50 atm, assuming the temperature remains constant?

 

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Problem:

In a nitrogen gas occupies has a volume of 500ml at a pressure of 0.971 atm. What volume will the gas occupies at a pressure of 1.50 atm, assuming the temperature remains constant?

Given Data:

V1 (initial volume) = 500 ml                    V2 (final volume) = unknown ?

P1 (initial pressure) = 0.971 atm             P2 (final pressure) = 1.50 atm

Solution:

This problem can be solve using Boyles Law in which volume is inversely proportional to pressure when temperature and the amount of gas are constant. When Pressure increases, volume decreases.

• The formula of Boyles Law is   P1V1 = P2V2
• To Solve for the V2 (final volume) we can use V2 = P1V1 / P2

V2 = P1V1 / P2

     = 0.971 atm × 500 ml / 1.50 atm   (cancel the unit atm)

     = 485.5 ml / 1.50

     = 323.67 ml

Answer:

the volume is 323.67

Hope it helps....=)