Question

What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C?

Answer 1

`1650 "bar"` or `165000kPa`

Explanation:

Ideal gas law:
`PV=nRT`
Rearrangement:
`P=(nRT)/V`
Calculate amount of `"CO"_2`:
`n("CO"_2)=m/M=(14.0g)/(28gmol^-1)=2mol`
Convert temperature to Kelvin:
`T=75+273=348K`
Volume of container:
`V=3.5L`
Ideal gas constant:
`R=8.314L"bar "K^-1 mol^-1`
Substitute values into ideal gas law:
`P=(2molxx8.314L "bar " K^-1 mol^-1xx348K)/(3.5L)=1650 "bar (3 s.f.)"=165000kPa`