Ten moles of a gas are contained in a 1.00 L container at 295 K. What is the pressure of the gas?

1 Answer
Aug 17, 2017

Answer:

#P = 242# #"atm"#

Explanation:

We're asked to find the pressure of a gas, given its temperature, and volume, and number of moles.

We can use the ideal-gas equation:

#ul(PV = nRT#

where

  • #P# is the pressure of the gas (what we're trying to find)

  • #V# is the volume occupied by the gas (given as #1.00# #"L"#

  • #n# is the number of moles of gas present (given as #10# #"mol"#)

  • #R# is the universal gas constant, equal to #0.082057("L"·"atm")/("mol"·"K")#

  • #T# is the absolute temperature of the gas (which must be in units of kelvin), given as #295# #"K"#

Let's rearrange the above equation to solve for the pressure, #P#:

#P = (nRT)/V#

Plugging in known values:

#color(red)(P) = ((10cancel("mol"))(0.082057(cancel("L")·"atm")/(cancel("mol")·cancel("K")))(295cancel("K")))/(1.00cancel("L")) = color(red)(ulbar(|stackrel(" ")(" "242color(white)(l)"atm"" ")|)#

The pressure is thus #color(red)(242color(white)(l)"atmospheres"#.