1.
Reaction between NaOH and HCl.
Trial 1
–
Calorimeter #1
Trial 2
–
Calorimeter #2
Mass of entire solution, (g).
Hint: Assume the density of both
solutions = 1.0 g/mL
Initial temperature of HCl prior to
mixing, T
i
(ºC)
T
f
after mixing (highest or lowest T over
3 minutes) (ºC)
ΔT
(ºC)
q
soln
(kJ)
q
cal
(kJ)
q
rxn
(kJ)
ΔH
rxn
(kJ)
Average ΔH
rxn
(kJ)
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2.
Reaction between NaOH and NH
4
Cl.
Trial 1
–
Calorimeter #1
Trial 2
–
Calorimeter #2
Mass of entire solution, (g).
Hint: Assume the density of both
solutions = 1.0 g/mL
Initial temperature of NaOH prior to
mixing, T
i
(ºC)
T
f
after mixing (highest or lowest T over
3 minutes) (ºC)
ΔT
(ºC)
q
soln
(kJ)
q
cal
(kJ)
q
rxn
(kJ)
ΔH
rxn
(kJ)
Average ΔH
rxn
(kJ)
Show all calculations necessary to fill in the table above:

3.
Reaction between HCl and NH
3
.
Trial 1
–
Calorimeter #1
Trial 2
–
Calorimeter #2
Mass of entire solution, (g).
Hint: Assume the density of both
solutions = 1.0 g/mL
Initial temperature of HCl prior to
mixing, T
i
(ºC)
T
f
after mixing (highest or lowest T over
3 minutes) (ºC)
ΔT
(ºC)
q
soln
(kJ)
q
cal
(kJ)
q
rxn
(kJ)
ΔH
rxn
(kJ)
Average ΔH
rxn
(kJ)
Using Hess’s Law and your average
ΔH
rxn
for reactions 1 and 2, what would
you have expected ΔH
rxn
to equal
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4.
Heat of Solution for Dissolving Ammonium Nitrate.
Trial 1
–
Calorimeter #1
Trial 2
–
Calorimeter #2
Mass of water, (g) (density = 1.0 g/mL)
Initial temperature of water prior to
mixing, T
i
(ºC)
T
f
after mixing (highest or lowest T over
3 minutes) (ºC)
ΔT
(ºC)
q
soln
(kJ)
q
cal
(kJ)
q
rxn
(kJ)
ΔH
rxn
(kJ)
Average ΔH
rxn
(kJ)
Show all calculations necessary to fill in the table above: