Question #db16f

1 Answer
Jul 4, 2017

Answer:

#"0.11 moles"#

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 the universal gas constant, equal to #0.0821("atm L")/("mol K")#
  • #T# is the absolute temperature of the gas

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

http://www.howequipmentworks.com/international_units/

Rearrange the equation to solve for #n#

#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.