What is the pressure in torr that a 0.44-g sample of carbon dioxide gas will exert at a temperature of 46.2°C when it occupies a volume of 5.00 L?

1 Answer
Jul 23, 2017

Answer:

#31.92#

Explanation:

To solve this problem we will use the ideal gas law equation:

#PV=nRT#

To find pressure we divided both sides by #V#

#(PcancelV)/cancelV=(nRT)/V#

#P=(nRT)/V#

First we need to convert the temperature to K so we add #212#

#46.2°C +212K=258.2K#

Now we also need to find the number of moles first we find the molar mass of #CO_2#, which is 44. We take our #.44# and divided by #44#.

#("gram sample of carbon dioxide")/("molar mass of " CO_2)#

#(.44 " grams")/(44 " Molar mass")=.01 " moles"#

Now we have:

#n=.01#

#R=0.0806# This is the universal gas constant

#T=258.2K#

#V=5.00L#

Let's plug it in:

#P=(.01"moles"(0.0806(Lxxatm)/(molxxK)(258.2K)))/(5.00L)#

#P=.042 " atm"#

To find the torr you multiply:

#.042xx760=31.92#