At Standard Temperature and Pressure, #"STP" (0^(@)"C" and "1 atm")#, #"1 mole"# of any ideal gas occupies #22.4" Liters of Volume"#.

#color(white)(aaaaaaaaaaaaaaaaa)(22.4" L")/(1" mol")#

Knowing this, we can think about this for a second without involving any math or calculations.

If we know #1" mole"# of a gas occupies #22.4" Liters of volume"# at #STP#, any number of moles more than #1# would occupy more than #22.4" Liters of volume"#. How much more volume? Well.

#color(white)(aaaaaaaaaaaaaaaaa)(1.78 cancel("moles"))/(1 cancel("mole")) = 1.78#

This means, there is #1.78"X"# more number of moles. So, since we know all else is held constant (#"Temperature and Pressure"#), #"moles"# and #"Volume"# are directly proportional here so #"Volume"# will increase by the same magnitude #("Avogadro's Law")#.

#1.78 * 22.4" L" = color(blue)(39.87" L"#

**Answer: 39.87 L**