of energy is required to melt the sample completely.
Further explanation:
Heat of fusion is the amount of energy needed to melt a solid at its melting point. It is represented by
.
Step 1: The ice at
is converted to water at
.
The formula to calculate the amount of energy is as follows:
...... (1)
Here,
Q is the amount of heat required.
n is the number of moles of water.
is the heat of fusion of ice.
The formula to calculate the moles of water is as follows:
...... (2)
Substitute 200 g for the given mass of water and 18 g/mol for the molar mass of water in equation (2).

Substitute 11.11 mol for n and 6.01 kJ/mol for
in equation (1).
Step 2: The temperature of water is raised from
to
.
The formula to calculate the heat energy of steam is as follows:
…… (3)
Here,
Q is the amount of heat transferred.
m is the mass of substance.
c is the specific heat of substance.
is the temperature change.
The temperature change for the above change can be calculated as follows:

Substitute 200 g for m,
for
and
for c in equation (3).
This energy is to be converted into kJ. The conversion factor for this is,

Therefore the energy can be calculated as follows:

The total amount of energy can be calculated as follows:
...... (4)
Here, Q is the total energy and
,and
are the values of energies calculated in first and second step respectively.
Substitute 66.77 kJ for
and 54.418 kJ for
in equation (4).

Learn more:
- What is the enthalpy of the given reaction? brainly.com/question/10412973
- Find the enthalpy of decomposition of 1 mole of MgO: brainly.com/question/2416245
Answer details:
Grade: Senior School
Chapter: Thermodynamics
Subject: Chemistry
Keywords: energy, Q1, Q2, Q, 54.418 kJ, 66.77 kJ, 121.88 kJ, m, c, temperature change, amount of heat, total energy.