7 salt packs data sheet
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Evaluating salts for use in Hot-Packs or Cold-Packs based on Enthalpy of Solution Lab Jing Maniaci
31
st
October 2023 Results Data Table I: Temperature Change on Solution Formation
Salt 1: NH
4
NO
3
Salt 2: CaCl
2
Salt 1
Trial 1
Trial 2
Trial 3
Mass of Calorimeter, g
26.69
27.01
27.89
Mass of Salt, g
2.05
2.65
2.37
Mass of calorimeter + solution, g
126.93
127.69
126.88
Mass of Solution, g
100.24
100.68
98.99
T
water
, o
C
21.7
21.5
21.4
T
solution
, o
C
20.3
20.7
19.9
Change in temperature, ΔT, o
C
-1.4
-0.8
-1.5
Salt 2
Trial 1
Trial 2
Trial 3
Mass of Calorimeter, g
27.50
27.50
27.40
Mass of Salt, g
2.36
2.27
2.40
Mass of calorimeter + solution, g
127.51
127.30
128.0
Mass of Solution, g
100.01
99.8
100.6
T
water
, o
C
21.5
22.2
21.8
T
solution
, o
C
22.7
23.7
24.4
Change in temperature, ΔT, o
C
1.2
1.5
2.6
Data Table II: Determining the Most Effective Hot-Pack and Cold-Pack
Salt
Salt Name
q
sol
, J
q
rxn
, J
Δ
H
o , kJ/mol
q per gram of salt, J/g
1
NH
4
NO
3
-514.43
514.43
17.43
217.98
2
CaCl
2
754.17
-754.17
-35.74
-322.29
Based on the calculated enthalpy of solution for each of the salts in Data Table II identify the salt/s that would be used either in a hot pack or a cold pack below:
Hot pack:
CaCl
2
Cold pack
:
NH4NO3
Calculations NH
4
NO
3
:
Heat absorbed or released by the solution:
q
sol
= m
soln x Cs x ΔT
m
soln
: (100.24 +100.68 + 98.99)/3 = 99.96g
Cs: 4.184 J/g.K ΔT: -1.23 o
C
Q
sol
: 99.96 g x 4.184 x -1.23 o
C = -514.43 J
Heat absorbed or released by the reaction: Q
rxn
= -q
sol
Q
rxn
= 514.43 J
Enthalpy of solution formation:
ΔH
o
rxn
= q
rxn
/n: n: 2.36/80.04 = 0.0295
ΔH
o
rxn
:
0.51443/0.00295 = 17.43 kJ/mol
q per gram of salt: qrxn / mass of salt: = 514.43/2.36 = 217.98 J/g
CaCl
2
:
Heat absorbed or released by the solution:
q
sol
= m
soln x Cs x ΔT
m
soln
: (100.01 + 99.8 + 100.6)/3 = 100.14g
Cs: 4.184 J/g.K ΔT: 1.8 o
C
Q
sol
: 100.14 g x 4.184 J/g.K x 1.8
o
C = 754.17 J
Heat absorbed or released by the reaction: Q
rxn
= -q
sol
Q
rxn
= -754.17 J
Enthalpy of solution formation:
ΔH
o
rxn
= q
rxn
/n: n: 2.34/110.98 = 0.0211
ΔH
o
rxn
:
-0.75417/0.0211 = -35.74 kJ/mol
q per gram of salt: qrxn / mass of salt: = -754.17/2.34 = -322.29 J/g
Conclusions
In this lab, the calculated enthalpy of the solution for the assigned salts was 17.43 kJ/mol for NH
4
NO
3
and -35.05 kJ/mol for CaCl
2
. The q per gram for each salt came out to be 217.98 J/g for NH
4
NO
3 and -315.87 J/g. The salt that would best be used for a cold pack is NH
4
NO
3
. The reason for this is that the enthalpy is positive and endergonic. Heat is being absorbed into the solution. On the other hand, the salt that would best be used as a heat pack is CaCl
2
. The enthalpy
for this salt was negative making it exergonic and heat is being released making it a good heat pack. Overall, this experiment went smoothly, and the results found in the lab are important as they let us know which salt we should use for a cold pack vs a hot pack. Different salts give out different enthalpies and if you know how to calculate it you can figure out which is the best hot
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pack and cold pack to buy. Knowing enthalpy is also important because you can tell how much heat is in the system.
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q- mcAT
Substance aJ kgK Substance cIJ kg"K
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Carbon
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Hydrogen
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2400
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Nitrogen
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Update :
Question 32 of 37
Submit
What amount of heat, in kJ, would be involved in condensing 19.1 g of
CH;OH? (AHvap = 38.0 kJ/mol)
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29.0
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29.0
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