Question

A sample of 0.500 kg of ice is held at a temperature of 0°C. How much energy

must be added to completely turn the ice into liquid water? (The latent heat of
vaporization for water is 2260 kJ/kg; the latent heat of fusion for water is 333
kJ/kg.)
A. 1130 kJ
B. 666 kJ
C. 167 kJ
D. 4520 kJ

Answer 1

C. 167 kJ

Step-by-step explanation:

The minimum amount of heat require to complete turn the ice into liquid water is equal to the latent heat of the ice, that is, the amount of heat needed by the ice to turn into water. This amount is calculated by:

`Q = m\cdot h_(f)` (1)

Where:

`m` - Mass of ice, measured in kilograms.

`h_(f)` - Latent heat of fusion, measured in kilojoules per kilogram.

`Q` - Latent heat, measured in kilojoules.

If we know that
`m = 0.500\,kg` and
`h_(f) = 333\,(kJ)/(kg)`, the latent heat of ice is:

`Q = (0.500\,kg)\cdot \left(333\,(kJ)/(kg) \right)`

`Q = 166.5\,kJ`

Therefore, the correct answer is C.