Question

A sample of nitrogen gas had a volume of 500. mL, a pressure in its closed container of 740 torr, and a temperature of 25 °C. What was the new volume of the gas when the temperature was changed to 50 °C and the new pressure was 760 torr?

Answer 1

527.68 mL

Step-by-step explanation:

We will assume that nitrogen is behaving as ideal gas here.

For ideal gas the gas law is:

`(P_(1)V_(1))/(T_(1))=(P_(2)V_(2))/(T_(2))`

Where

P1= initial pressure = 740 torr

V1= initial volume = 500mL

T1= initial temperature = 25⁰C = 298 K

P2= final pressure = 760 torr

V2= final volume = ?

T2= final temperature = 50⁰C = 323 K

Putting values in the gas law

Final volume =
`(740X500X323)/(298X760)= 527.68 mL`