A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C?

1 Answer
Jun 12, 2017

Answer:

#212# #"torr"#

Explanation:

Let's use the combined gas law:

#Rightarrow frac(P_(1) V_(1))(T_(1)) = frac(P_(2) V_(2))(T_(2))#

In our case, the temperature of #125^(@)# #"C"# is kept constant throughout the process, so #T_(1) = T_(2)#:

#Rightarrow frac(P_(1) V_(2))(T_(1)) = frac(P_(2) V_(2))(T_(1))#

#Rightarrow P_(1) V_(1) = P_(2) V_(2)#

Then, let's substitute the relevant values:

#Rightarrow 248# #"torr" times 275# #"L" = P_(2) times 321# #"L"#

#Rightarrow P_(2) = frac(248 " torr" times 275 " L")(321 " L")#

#therefore P_(2) = 212.46105919# #"torr"#

Therefore, the final gas pressure will be around #212# #"torr"#.