Respuesta :
Answer:- [tex]\Delta H[/tex] = -[tex]\frac{52.52kJ}{mol}[/tex]
Solution:- Total volume of the solution = 5.0 mL + 50.0 mL = 100.0 mL
Density of solution is same as of water that is 1.0 g per mL. So, the mass of solution, m = [tex]100.0mL(\frac{1.0g}{mL})[/tex]
m = 100.0 g
change in temperature, [tex]\Delta T[/tex] = 26.3 - 20.2 = 6.1 degree C
specific heat, s of water is 4.184 J per g per degree C.
[tex]q=ms\Delta T[/tex]
where q is the heat energy. let's plug in the values in the equation:
[tex]q=100.0g(4.184\frac{J}{g.^0C})6.1^0C[/tex]
q = 2552.24 J
energy of calorimeter = change in temperature*heat capacity of calorimeter
energy of calorimeter = [tex]6.1^0C(\frac{12.1J}{^0C})[/tex]
= 73.81 J
Total heat = 2552.24 J + 73.81 J = 2626.05 J
Let's convert it to kJ and for this we divide by 1000 since, 1000 J = 1 kJ
[tex]2626.05J(\frac{1kJ}{1000J})[/tex]
= 2.626 kJ
0.05 moles of copper sulfate are used so the [tex]\Delta H[/tex] of the reaction = [tex]\frac{2.626kJ}{0.05mol}[/tex]
= [tex]\frac{52.52kJ}{mol}[/tex]
Since, there is an increase in temperature, the heat is released and so the sign of [tex]\Delta H[/tex] will be negative.
Hence, [tex]\Delta H[/tex] = -[tex]\frac{52.52kJ}{mol}[/tex]
The [tex]\rm \bold{\Delta H}[/tex] of the process is 2.626 kJ/0.05 mol which is equal to 52.52 kJ/mol.
The heat capacity formula,
[tex]\rm \bpld{ Q = mc \Delta T}[/tex]
Where,
Q - energy
m - mass = 100 mL
c - specific heat capacity = 4.184 [tex]\rm \bold { J/g/^oC}[/tex]
[tex]\rm \bpld{ \Delta T}[/tex] - temperature difference = [tex]\rm \bold { 6.1 ^oC}[/tex]
Put the value on equation we get
Q = 2552.24 J
Energy of calorimeter = 73.81 J
Total heat = 2552.24 J + 73.81 J = 2626.05 J = 2.626 kJ
Hence, the [tex]\rm \bold{\Delta H}[/tex] of the process is 2.626 kJ/0.05 mol which is equal to 52.52 kJ/mol.
To know more about specific heat capacity, refer to the link:
https://brainly.com/question/11194034?referrer=searchResults
