# Question #db16f

##### 1 Answer

Jul 4, 2017

#### Explanation:

All you have to do here is to use the **ideal gas law equation**, which looks like this

#color(blue)(ul(color(black)(PV = nRT)))#

Here

#P# is the pressure of the gas#V# is the volume it occupies#n# is the number of moles of gas present in the sample#R# is theuniversal gas constant, equal to#0.0821("atm L")/("mol K")# #T# is theabsolute temperatureof the gas

Notice that the problem provides the temperature of the gas in *degrees Celsius*, so make sure to **convert** this to *Kelvin*!

Rearrange the equation to solve for

#PV = nRT implies n = (PV)/(RT)#

Plug in your values to find

#n = (11.2 color(red)(cancel(color(black)("atm"))) * 0.24 color(red)(cancel(color(black)("L"))))/(0.0821 (color(red)(cancel(color(black)("atm"))) * color(red)(cancel(color(black)("L"))))/("mol" * color(red)(cancel(color(black)("K")))) * (273.15 + 12)color(red)(cancel(color(black)("K"))))#

#n = color(darkgreen)(ul(color(black)("0.11 moles"))#

The answer is rounded to two **sig figs**.