Question

What quantity of energy, in joules, is required to raise the temperature of 425 g of tin from room temperature, 25.0 °C, to its melting point, 231.9 C, and then melt the tin at that temperature? (The specific heat capacity of tin is 0.227 J/g K, and the heat of fusion of this metal is 59.2 Jig) Energy required

Answer 1

Answer:

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is 45.249 kiloJoules.

Explanation:

Mass of the tin ,m= 425 g

Heat capacity of the tin ,c= 0.227 J/g K

Initial temperature of the tin ,$T_1$= 25.0 °C = 298.15 K

Final temperature of the tin, $T_2$= 231.9 °C = 505.05 K

Let the heat required to change the temperature of tin from 298.15 K to 505.05 K be Q.

$Q=mc\times (T_2-T_1)$

$=425 g\times 0.227 J/g K\times (505.05K - 298.15 K)=19,960.68 J=19.961 kJ$

Heat required to melt tin at 505.05 K be Q'

The heat of fusion of tin metal =$\Delta H_{fus}=59.2 J/g$

$Q'= m\times \Delta H_{fus}=425 g\times 59.2 J/g=25,287.5 J=25.288 kJ$

Total energy required to raise the temperature of 425 g of tin from 298.15 K to 505.05 K and to melt the tin at 505.05 K is:

= Q+Q' =  19.961 kJ + 25.288 kJ = 45.249 kJ