Answer : The correct option is, (B) 12.3 KJ
Solution :
First we have to calculate the moles of water.
\(\text{Moles of water}=\frac{\text{Mass of water}}{\text{Molar mass of water}}=\frac{36.8g}{18g/mole}=2.04mole\)
Now we have to calculate the amount of heat released.
Formula used :
\(q=n\times \Delta H_{fusion}\)
where,
q = heat released
n = number of moles = 2.04 mole
\(\Delta H_{fusion}\) = molar enthalpy of fusion of a substance = -6.01 KJ/mole
Now put all the give values in the above formula, we get the amount of heat released.
\(q=(2.04mole)\times (-6.01KJ/mole)=-12.3KJ\)
The negative sign indicate heat released.
Therefore, the amount of heat released is, 12.3 KJ
