Answer:
527.68 mL
Explanation:
We will assume that nitrogen is behaving as ideal gas here.
For ideal gas the gas law is:
[tex]\frac{P_{1}V_{1}}{T_{1}}=\frac{P_{2}V_{2}}{T_{2}}[/tex]
Where
P1= initial pressure = 740 torr
V1= initial volume = 500mL
T1= initial temperature = 25â°C = 298 K
P2= final pressure = 760 torr
V2= final volume = ?
T2= final temperature = 50â°C = 323 K
Putting values in the gas law
Final volume = [tex]\frac{740X500X323}{298X760}= 527.68 mL[/tex]
