Answer :
Answer : The quantity of heat released is -11.30 kJ
Explanation :
First we have to calculate the number of moles of water.
[tex]\text{Moles of water}=\frac{\text{Mass of water}}{\text{Molar mass of water}}[/tex]
Molar mass of water = 18 g/mole
[tex]\text{Moles of water}=\frac{5.00g}{18g/mole}=0.278mole[/tex]
Now we have to calculate the amount of heat released.
[tex]\Delta H=-\frac{q}{n}[/tex]
where,
[tex]\Delta H[/tex] = heat of vaporization = 40.66 kJ/mol
q = heat released = ?
n = number of moles of water = 0.278 mole
[tex]40.66kJ/mol=-\frac{q}{0.278mol}[/tex]
[tex]q=-11.30kJ[/tex]
In vaporization process, the amount of heat is absorbed but in the process of condensation the amount of heat is released.
Therefore, the quantity of heat released is -11.30 kJ