Answer:
How much energy does it take to melt a 16.87 g ice cube? ΔHfus = 6.02 kJ/mol How much energy does it take to melt a 16.87 g ice cube? = 6.02 kJ/mol
A. 108 kJ
B. 102 kJ
C. 5.64 kJ
D. 936 kJ
E. none of the above
5.64 kJ
Explanation:
The Heat of fusion is the heat energy required to dissolve a given mass of ice at melting point.
The heat energy required to dissolve ice can be calculated using the expression below;
Q = ΔH[tex]_{f}[/tex] x m ...............................................1
where Q is the heat energy required;
ΔH[tex]_{f}[/tex] is the heat of fusion for ice;
m is the mole
All the parameters above are provided in the question except m, so to get m we use the molar mass of water (also for ice) which is 18.01528 g/mol .
This means that 18.01528 g of ice is contained in one mole, therefore the mole for 16.87 g of ice is given as;
[tex]m = \frac{16.87g}{18.015g/mol}[/tex]
m = 0.9364 mole of ices
Now the parameters are complete, we are given;
ΔH[tex]_{f}[/tex] = 6.02 kJ/mol
m = 0.9364 mol
Q =?
Substituting into equation 1, we have
Q = 6.02 kJ/mol x 0.9364 mol
Q = 5.64 kJ
Therefore, the energy required to melt 16.87 g of ice is 5.64 kJ
