Respuesta :
Answer:
The correct answer is option e.
Explanation:
Total volume of the mixture of solution= 50.0 mL + 50.0 mL = 100.0 mL
Total mass of the solution = M
Density of the mixture of solution = density of pure water = d = 1 g/mL
[tex]Mass =Density\times Volume[/tex]
[tex]m=1 g/mL\times 100.0 mL = 100.0 g[/tex]
Specific heat of mixture of solution = Specific of water = c
c = 4.184 J/g°C
Change in temperature = ΔT = 31.77°C - 25.10°C =6.67°C
Heat gained by the mixture of solution = Q
[tex]Q=mc\Delta T[/tex]
[tex]Q=100.0 g\times 4.184 J/g^oC\times 6.67^oC=2,790.73 J[/tex]
[tex]2KOH+H_2SO_4\rightarrow K_2SO_4+2H_2O[/tex]
Moles of KOH = n
Volume of KOH solution = 50.0 mL = 0.050 L
Molarity of the solution = 1.00 M
[tex]n=1.00M\times 0.050 L=0.050 mol[/tex]
The ΔH of this reaction:
[tex]\Delta H=\frac{-Q}{n}=\frac{-2,790.73 J}{0.050 mol}=-55,814.56 J/mol=-55.8kJ/mol[/tex]
The ΔH of this reaction is -55.8 kJ/mol.
