Question

Question #db16f

Answer 1

`"0.11 moles"`

Explanation:

All you have to do here is to use the ideal gas law equation, which looks like this

`color(blue)(ul(color(black)(PV = nRT)))`

Here

• `P` is the pressure of the gas
• `V` is the volume it occupies
• `n` is the number of moles of gas present in the sample
• `R` is the universal gas constant, equal to `0.0821("atm L")/("mol K")`
• `T` is the absolute temperature of the gas

Notice that the problem provides the temperature of the gas in degrees Celsius, so make sure to convert this to Kelvin!

![http://www.howequipmentworks.com/international_units/]()

Rearrange the equation to solve for `n`

`PV = nRT implies n = (PV)/(RT)`

Plug in your values to find

`n = (11.2 color(red)(cancel(color(black)("atm"))) * 0.24 color(red)(cancel(color(black)("L"))))/(0.0821 (color(red)(cancel(color(black)("atm"))) * color(red)(cancel(color(black)("L"))))/("mol" * color(red)(cancel(color(black)("K")))) * (273.15 + 12)color(red)(cancel(color(black)("K"))))`

`n = color(darkgreen)(ul(color(black)("0.11 moles"))`

The answer is rounded to two sig figs.