Question #ad885

1 Answer
May 9, 2017

Answer:

The pressure of the gas is 192 bar.

Explanation:

This looks like the time to apply the Ideal Gas Law:

#color(blue)(bar(ul(|color(white)(a/a)pV = nRTcolor(white)(a/a)|)))" "#

where

  • #p# is the pressure
  • #V# is the volume
  • #n# is the number of moles
  • #R# is the gas constant
  • #T# is the temperature

We can rearrange the Ideal Gas Law to get

#P = (nRT)/V#

In this problem,

#n = "4.35 mol"#
#R = "0.0831 4 bar·L·K"^"-1""mol"^"-1"#
#T = "(75 + 273.15) K" = "348.15 K"#
#V = "0.655 L"#

#P = (4.35 color(red)(cancel(color(black)("mol"))) × "0.083 14 bar"·color(red)(cancel(color(black)("L·K"^"-1""mol"^"-1"))) × 348.15 color(red)(cancel(color(black)("K"))))/(0.655 color(red)(cancel(color(black)("L")))) = "192 bar"#