# Question #624ba

##### 1 Answer

#### Explanation:

The idea here is that **one mole** of any ideal gas that is kept under **Standard Temperature and Pressure**, **STP**, conditions will occupy **molar volume of a gas at STP**.

This can be derived using the **ideal gas law** equation

#color(blue)(|bar(ul(color(white)(a/a)PV = nRTcolor(white)(a/a)|)))" "# , where

STP conditions are defined as a pressure of

#PV = nRT implies V/n = (RT)/P#

#V/n = (0.0821(color(red)(cancel(color(black)("atm"))) * "L")/("mol" * color(red)(cancel(color(black)("K")))) * 273.15color(red)(cancel(color(black)("K"))))/(1color(red)(cancel(color(black)("atm")))) = "22.4 L mol"^(-1)#

This tells you that **every mole** of an idea lgas that is being kept under STP conditions will occupy

So, if **one mole** of any ideal gas, it follows that

#67.2color(red)(cancel(color(black)("L"))) * overbrace("1 mole"/(22.4color(red)(cancel(color(black)("L")))))^(color(purple)("molar volume of a gas at STP")) = color(green)(|bar(ul(color(white)(a/a)"3.00 moles"color(white)(a/a)|)))#

**SIDE NOTE** *It's worth noting that the current STP conditions are defined as a pressure of*

*and a temperature of*

*Under these conditions for pressure and temperature, one mole of any ideal gas occupies*