Respuesta :
Explanation:
Given temperatures are as follows.
Heat capacity for acetic acid = [tex]2.06 J/g^{o}C[/tex]
Melting point of acetic acid = [tex]16.64^{o}C[/tex]
Enthalpy of fusion for acetic acid = 11.73 kJ/mol
Number of moles of acetic acid = [tex]\frac{154 g}{60.05 g/mol}[/tex]
= 2.564 mol
Now, conversion of solid acetic acid at [tex]16.64^{o}C[/tex] to liquid acetic acid at [tex]16.64^{o}C[/tex]
We know that,
[tex]q_{1} = m \times \Delta H_{f}[/tex]
= [tex]2.564 mol \times 11.73 kJ/mol[/tex]
= 30.075 kJ
Also, conversion of liquid acetic acid at [tex]16.64^{o}C[/tex] to gas at [tex]39.5^{o}C[/tex]
[tex]q_{2} = m \times C \times \Delta T[/tex]
= [tex]154 g \times 2.06 J/g^{o}C \times (39.5 - 16.64)^{o}C[/tex]
= 7252.1064 J
= 7.252 kJ (as 1 kJ = 1000 J)
Total heat energy required = [tex]q_1 + q_2[/tex]
= 30.075 + 7.252
= 37.327 kJ
Thus, we can conclude that the amount of heat required is 37.327 kJ.
