Question

What is the volume, in liters, occupied by 0.723 mol of a gas at 32.0°C if the pressure is 852 mm Hg?

Answer 1

the volume will be `V = 16.2L`

Explanation:

To solve for the volume we can use the Ideal Gas Law equation

`PV=nRT`

`P=` Pressure in `atm`
`V=` Volume in `L`
`n=` moles
`R=` the Gas Law Constant `0.0821 (atm*L)/(mol*K)`
`T=` Temperature in `K`

When using the Ideal Gas Law Constant we must convert the Pressure to `atm`
`P=852mmHg*(1atm)/(760mmHg)= 1.12 atm`

`V=?`

`n=0.723mol`

`R=0.0821 (atm*L)/(mol*K)`

When using the Ideal Gas Law Constant we must convert the Temperature to `K`
`T=32.0^oC+273 = 305K`

`V=(nRT)/P`

`V=((0.723cancel(mol))(0.0821 (cancel(atm)*L)/(cancel(mol)*cancel(K)))(305cancelK))/(1.12cancel(atm))`

`V = 16.2L`