Taking into account the definition of calorimetry, sensible heat and latent heat, the amount of heat required is 2.243974 kJ or 2,243.974 J.
Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.
Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).
Latent heat is defined as the energy required by a quantity of substance to change state.
When this change consists of changing from a solid to a liquid phase, it is called heat of fusion and when the change occurs from a liquid to a gaseous state, it is called heat of vaporization.
In firts place, you know that the melting point is 0°C. So, first of all you must increase the temperature from -14 ° C (in solid state) to 0 ° C, in order to supply heat without changing state (sensible heat).
The amount of heat a body receives or transmits is determined by:
Q = c× m× ΔT
where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.
In this case, you know:
Replacing:
Q1= 2.09 [tex]\frac{J}{gC}[/tex] × 4.88 g× 14 °C
Solving:
Q1=142.7888 J= 0.1427888 kJ
The heat Q that is necessary to provide for a mass m of a certain substance to change phase is equal to
Q = m×L
where L is called the latent heat of the substance and depends on the type of phase change.
In this case, you know:
Replacing:
Q2= 0.2711 moles×6.02 [tex]\frac{kJ}{mol}[/tex]
Solving:
Q2= 1.632022 kJ
Similar to sensible heat previously calculated, you know:
Replacing:
Q3= 4.18[tex]\frac{J}{gC}[/tex] × 4.88 g× 23 °C
Solving:
Q3= 469.1632 J= 0.4691632 kJ
The total heat required is calculated as:
Total heat required= 0.1427888 kJ + 1.632022 kJ + 0.4691632 kJ
Total heat required= 2.243974 kJ= 2,243.974 J
In summary, the amount of heat required is 2.243974 kJ or 2,243.974 J.
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