What is the volume of #"0.220 mols"# of carbon monoxide gas found at STP?

1 Answer
Truong-Son N.
Jun 3, 2016

If we assume that carbon monoxide (#"CO"#) is an ideal gas, then we can use the ideal gas law:

#\mathbf(PV = nRT)#

where:

  • #P# is the pressure of the gas. We can use #"bars"# as our units.
  • #V# is the volume of the gas in #"L"#.
  • #n# is the #\mathbf("mol")#s of gas.
  • #R# is the universal gas constant, #"0.083145 L"cdot"bar/mol"cdot"K"#.
  • #T# is the temperature of the gas in #"K"#.

At STP, #T = 0^@ "C" = "273.15 K"#, and #P = "1 bar"#. So, to get the volume, just solve for #V#.

#color(blue)(V_"CO") = (nRT)/P#

#= ((0.220 cancel("mol CO"))("0.083145 L"cdotcancel("bar")"/"cancel("mol")cdotcancel("K"))(273.15 cancel("K")))/(1 cancel"bar")#

#=# #color(blue)("5.00 L")# to 3 sig figs.

Related questions
See all questions in Combined Gas Law
Impact of this question
1891 views around the world
You can reuse this answer
Creative Commons License