Respuesta :
Answer:
Enthalpy change for the reaction is -67716 J/mol.
Explanation:
Number of moles of [tex]AgNO_{3}[/tex] in 50.0 mL of 0.100 M of [tex]AgNO_{3}[/tex]
= Number of moles of HCl in 50.0 mL of 0.100 M of HCl
= [tex]\frac{0.100}{1000}\times 50.0[/tex] moles
= 0.00500 moles
According to balanced equation, 1 mol of [tex]AgNO_{3}[/tex] reacts with 1 mol of HCl to form 1 mol of AgCl.
So, 0.00500 moles of [tex]AgNO_{3}[/tex] react with 0.00500 moles of HCl to form 0.00500 moles of AgCl
Total volume of solution = (50.0+50.0) mL = 100.0 mL
So, mass of solution = ([tex]100.0\times 1.00[/tex]) g = 100 g
Enthalpy change for the reaction = -(heat released during reaction)/(number of moles of AgCl formed)
= [tex]\frac{-m_{solution}\times C_{solution}\times \Delta T_{solution}}{0.00500mol}[/tex]
= [tex]\frac{-100g\times 4.18\frac{J}{g.^{0}\textrm{C}}\times [24.21-23.40]^{0}\textrm{C}}{0.00500mol}[/tex]
= -67716 J/mol
[m = mass, c = specific heat capacity, [tex]\Delta T[/tex] = change in temperature and negative sign is included as it is an exothermic reaction]
