Question

g An ice cube has a mass of 54 g and is initially at a temperature of 0°C . The ice cube is heated until 47.4 g has become water at 100°C and 6.6 g has become steam at 100°C. How much energy (in kJ) was transferred to the ice cube to accomplish the transformation?

Answer 1

55536.6 J

Step-by-step explanation:

Given:

Mass of the ice = 54g

Initial temperature = 0°C

Final Temperature = 100°C

Mass of the steam = 6.6g

Now the energy required for the transformation of the ice to vapor will involve the heat requirement in the following stages as:

1) The energy required to melt ice = mass of ice × heat of fusion of water = 54g × 334 J/g = 18036 J

(because heat of fusion for water = 334 J/g)

2) The energy to heat water from 0 to 100 = mass of water × specific heat of water × change in temperature = 54g × 4.186 J/g°C × 100 °C = 22604.4 J

lastly,

3) the energy required to vaporize 6.6g of water = mass of water × heat of vaporization of water = 6.6 × 2257 J/g = 14896.2 J

Thus,

the total energy required to transform the ice cube to accomplish the transformation = 18036 + 22604.4 + 14896.2 = 55536.6 J.