Respuesta :
Answer:
The enthalpy of solution for one mole of solid is 4.003 kilojoules per mole.
Explanation:
Heat lost by the resultant solution that is content of calorimeter= [tex]q_1[/tex]
[tex]\Delta T[/tex] = change in temperature = -1.11°C
[tex]q_1=m_1c_1\times \Delta T[/tex]
[tex]q_1=60.0 g\times 4.06J/g^oC\times (-1.11)^oC=-270.396 J[/tex]
Heat lost by the calorimeter = [tex]q_2[/tex]
[tex]\Delta T[/tex] = change in temperature = -1.11°C
[tex]q_2=c_2\times \Delta T[/tex]
[tex]q_2=-5.661 J[/tex]
Heat absorbed by the reaction = Heat lost by solution + Heat lost by the calorimeter
[tex]Q=[-q_1+(-q_2)][/tex]
[tex]Q=[-(m_1c_1\times \Delta T)+(-c_2\times \Delta T)][/tex]
where,
Q = heat absorbed by the reaction or heat change due to solution process
[tex]c_1[/tex] = specific heat of solution = [tex]4.06J/^oC[/tex]
[tex]c_2[/tex] = specific heat of calorimeter= [tex]5.10J/g^oC[/tex]
[tex]m_1[/tex] = mass of solution= 60.0 g
[tex]\Delta T[/tex] = change in temperature = -1.11°C
Now put all the given values in the above formula, we get:
[tex]Q=[-(60.0 g\times 4.06J/g^oC\times (-1.11)^oC)+(- 5.10J/^oC\times (-1.11)^oC)][/tex]
[tex]Q=276.057 J[/tex]
Heat change due to solution process is 276.057 J.
Now we have to calculate the enthalpy change for dissolving this salt on a energy per mole
[tex]\Delta H=\frac{Q}{n}[/tex]
where,
[tex]\Delta H[/tex] = enthalpy change = ?
q = heat absorbed = 276.057 J
m = mass of salt = 10.0 g
n = mole of salt = [tex]\frac{10.0 g}{145.0 g/mol}=0.06896 moll[/tex]
[tex]\Delta H=\frac{276.057 J}{0.06896 mo}=4,002.82 J/mol=4.003 kJ/mol[/tex]
The enthalpy of solution for one mole of solid is 4.003 kilojoules per mole.
