Question

How many moles of `NH_3` are in a 3.0 L vessel at `3*10^2` `K` with a pressure of 1.50 atm?

Answer 1

There are 0.18 mol of `"NH"_3` in the vessel.

Explanation:

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

`color(blue)(|bar(ul(PV = nRT)|)`,

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

`n = (PV)/(RT)`

`P = "1.50 atm"`
`V = "3.0 L"`
`R = "0.082 06 L·atm·K"^"-1""mol"^"-1"`
`T = 3×10^2 color(white)(l) "K"`

`n = (PV)/(RT) = (1.50 color(red)(cancel(color(black)("atm"))) × 3.0 color(red)(cancel(color(black)("L"))))/( "0.082 06" color(red)(cancel(color(black)("L·atm·K"^"-1"))) "mol"^"-1" × 3 × 10^2 color(red)(cancel(color(black)("K")))) = "0.18 mol"`