Answer:
Step-by-step explanation:
To calculate the heat of the reaction in kJ/mol of AgCl formed, we can use the concept of calorimetry and the equation for heat transfer:
�
=
�
⋅
�
⋅
Δ
�
q=m⋅c⋅ΔT
Where:
�
q is the heat transfer (in Joules).
�
m is the mass of the solution (in grams).
�
c is the specific heat capacity of the solution (in J/°C·g).
Δ
�
ΔT is the change in temperature (in °C).
First, we need to calculate the change in temperature (
Δ
�
ΔT):
Δ
�
=
�
�
−
�
�
ΔT=T
f
−T
i
Where:
�
�
T
f
is the final temperature.
�
�
T
i
is the initial temperature.
Δ
�
=
23.68
°
�
−
22.88
°
�
=
0.80
°
�
ΔT=23.68°C−22.88°C=0.80°C
Next, we'll calculate the mass of the solution (
�
m):
Since you have 55.0 mL of 0.100 M AgNO3 and 55.0 mL of 0.100 M HCl, you have a total volume of 110.0 mL (0.110 L) of the solution.
The density of the solution is typically close to the density of water, which is approximately 1 g/mL.
So, the mass of the solution is:
�
=
110.0
�
m=110.0g
Now, we'll calculate the heat transfer (
�
q):
�
=
�
⋅
�
⋅
Δ
�
q=m⋅c⋅ΔT
�
=
110.0
�
⋅
4.18
�
/
°
�
⋅
�
⋅
0.80
°
�
q=110.0g⋅4.18J/°C⋅g⋅0.80°C
�
=
369.872
�
q=369.872J
Now, we need to convert the heat from Joules to kJ:
�
=
369.872
�
⋅
1
�
�
1000
�
=
0.369872
�
�
q=369.872J⋅
1000J
1kJ
=0.369872kJ
Now, we can calculate the heat per mole of AgCl formed. The balanced chemical equation shows that one mole of AgCl is formed from one mole of Ag+ and one mole of Cl-. Since the initial concentrations of AgNO3 and HCl were both 0.100 M, they are 1:1 in the reaction.
So, for every 0.100 moles of AgNO3 and 0.100 moles of HCl, we form 0.100 moles of AgCl.
Now, we can calculate the heat in kJ/mol of AgCl formed:
Heat per mole of AgCl
=
0.369872
�
�
0.100
�
�
�
�
�
=
3.69872
�
�
/
�
�
�
Heat per mole of AgCl=
0.100moles
0.369872kJ
=3.69872kJ/mol
So, the heat that accompanies this reaction in kJ/mol of AgCl formed is approximately 3.70 kJ/mol.