At 22.0 degrees Celsius an \"empty\" 30-ml syringe had a volume of 5.0 ml. After

Question

At 22.0 degrees Celsius an "empty" 30-ml syringe had a volume of 5.0 ml. After a liquid is introduced and the temperature is raised to 32.0 degrees Celsius, the volume becomes 10.2 ml. The barometer pressure is 745.8 mmHg, 1. what was the pressure of the air inside the syringe when the syringe was "empty"? 2. What is the pressure of the air inside the syringe after the liquid has been introduced and the temperature raised to 32.0 degrees Celsius? 3. What is the vapor pressure of the liquid at the higher temperature?

Explanation / Answer

P1*V1/T1=P2*V2/T2

initial conditions = final conditions.

then:

P1=T1*(P2*V2/T2)/V1

P1=22*(745.8*10.2/32)/5
P1=1045.98mmHg

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