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 108 kJ 102 kJ 5.64 kJ 936 J none of the above

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 x m ...............................................1

where Q is the heat energy required;

           ΔH  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;

m = 0.9364 mole of ices

Now the parameters are complete, we are given;

ΔH  = 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

well clustered together.

points close on a scatter diagram

0 = 0.40 / 0 = 0

= 0.20 = 9.80 ⁄2 =?

=0 , = = 0.20 =0.50 0 0.40 ⁄

=0−122 =0−12(9.80 ⁄2)(0.50)2 =1.2