Answer:
[tex]21.994KJ[/tex]
Explanation:
The acetone has the following molecular formula :
C3H6O
The molar mass of the acetone is
μ(C3H6O) = [tex]58.08 \frac{g}{mole}[/tex]
You can find this value in any table.
The molar mass means the mass that has 1 mole of C3H6O
Now, the heat follows this equation :
[tex]Q=(n).(LHV)[/tex]
Where Q is the heat, n is the number of moles of the substance and LHV is the latent heat of vaporization of the substance.
Let's calculate n
If 1 mole of C3H6O has a mass of 58.08 g ⇒
x moles of C3H6O will have a mass of 43.9 g ⇒
[tex]x=\frac{(43.9)}{(58.08)}=0.7558mole[/tex]
In 43.9 g of C3H6O there is 0.7558 moles of C3H6O
The LHV for C3H6O is [tex]29.1\frac{KJ}{mole}[/tex]
You can find this value in any table
To find the amount of heat :
[tex]Q=(n).(LHV)=(0.7558mole)(29.1\frac{KJ}{mole})=21.994KJ[/tex]
We find out that 21.994 KJ are required to vaporize 43.9 g of acetone (C3H6O).
