Answer:
The enthalpy change of the reaction is -66.88 kJ/mol.
Explanation:
Mass of the solution = m = 100 g
Heat capacity of the solution = c = 4.18 J/g°C
Initial temperature of the solutions before mixing = [tex]T_1=22.60^oC[/tex]
Final temperature of the solution after mixing = [tex]T_2=23.40^oC[/tex]
Heat gained by the solution due to heat released by reaction between HCl and silver nitrate = Q
[tex]Q=m\times c\times (T_2-T_1)[/tex]
[tex]Q=100 g\times 4.18 J/g^oC\times (23.40^oC-22.60^oC)=334.4 J[/tex]
Heat released due to reaction = Q' =-Q = -334.4 J
Moles of silver nitrate = n
Molarity of silver nitrate solution = 0.100 M
Volume of the silver nitrate solution = 50.0 mL = 0.050 L ( 1 mL = 0.001 L)
[tex]Moles =Molarity\times Volume (L)[/tex]
[tex]n=0.100 M\times 0.050 L=0.005 mol[/tex]
Enthalpy change of the reaction = [tex]\Delta H[/tex]
[tex]=\Delta H=\frac{-334.4 J}{0.005 mol}=-66,880 J/mol=-66.88 kJ/mol[/tex]
1 J = 0.001 kJ
The enthalpy change of the reaction is -66.88 kJ/mol.
