Table 2-2: Data and Calculations for Metal + HCI (aq) Write all units next to the numerical values. Data should be reported to the correct number of significant figures. Show calculations for Trial 1 in the space provided. Trial 1, Trial 2 Mass of dry, empty calorimeter (centigram balance) 8.059 (Cup) 8.05g (Cup)

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Table 2-2: Data and Calculations for Metal + HCI (aq)
Write all units next to the numerical values. Data should be reported to the correct number of
significant figures. Show calculations for Trial 1 in the space provided.
Trial 1,
Trial 2
Mass of dry, empty calorimeter (centigram
balance)
8.059 (Cup)
8.059 (Cup)
Mass of calorimeter plus HCI (aq)
8.05g + 24.77g HC| = 8.05+24.73 HCI=
32.829
32.82g-8.059=
24.77g Hel
|(centigram balance)
32.829
Mass of HCl (aq) used
32.829-8.05g
24.779HCI
Mass of metal used (analytical balance)
0.3159 Mg
0,31lg Mg
Initial temperature of HCl (aq)
20,2°C
2 1. 2°C
Final (maximum) temperature of reaction
mixture
56,0°C
56.8°C
Total mass of mixture, m
m= HCI+ Mg
24.779 HCI +0.315g My
= 25,08 5g HMg CI
m=HCI + Mg
24.7 HCI+a31gMg
. = 25.0819 HNGČÍ
m= HCl+ Mg
%3D
| Temperature change of mixture, AT
56.0 – 20,2=
35.8°C
56.8-21,2 =
35.6°C
4.184 J/g•°C
Cspecific heat capacity of solution)
rieat absorbed by mixture, in J
(q =m C, AT): show calculations
4.184 J/g•°C
4.1845
(35.692)
=375 7,4119 J=3735,8249J
Transcribed Image Text:Table 2-2: Data and Calculations for Metal + HCI (aq) Write all units next to the numerical values. Data should be reported to the correct number of significant figures. Show calculations for Trial 1 in the space provided. Trial 1, Trial 2 Mass of dry, empty calorimeter (centigram balance) 8.059 (Cup) 8.059 (Cup) Mass of calorimeter plus HCI (aq) 8.05g + 24.77g HC| = 8.05+24.73 HCI= 32.829 32.82g-8.059= 24.77g Hel |(centigram balance) 32.829 Mass of HCl (aq) used 32.829-8.05g 24.779HCI Mass of metal used (analytical balance) 0.3159 Mg 0,31lg Mg Initial temperature of HCl (aq) 20,2°C 2 1. 2°C Final (maximum) temperature of reaction mixture 56,0°C 56.8°C Total mass of mixture, m m= HCI+ Mg 24.779 HCI +0.315g My = 25,08 5g HMg CI m=HCI + Mg 24.7 HCI+a31gMg . = 25.0819 HNGČÍ m= HCl+ Mg %3D | Temperature change of mixture, AT 56.0 – 20,2= 35.8°C 56.8-21,2 = 35.6°C 4.184 J/g•°C Cspecific heat capacity of solution) rieat absorbed by mixture, in J (q =m C, AT): show calculations 4.184 J/g•°C 4.1845 (35.692) =375 7,4119 J=3735,8249J
Chemistry 1A
Name
Lab Partner
Trial 1
Trial 2
25 J/C
255/°C
Calorimeter Constant (Ceal) from Part 1
9rxn (heat released by reaction, in J) = AH2m
=(heat absorbed by mixture + Ceai AT)
show calculations
Moles of metal used. show calculations
AHro1 in kJ/mol of metal used. show
calculations
Average AHn in k.J
Is this reaction exothermic or endothermic? What is your experimental evidence supporting this? Is
AHrn positive or negative? Make sure your Average AHrxn in kJ above shows the correct sign.
Transcribed Image Text:Chemistry 1A Name Lab Partner Trial 1 Trial 2 25 J/C 255/°C Calorimeter Constant (Ceal) from Part 1 9rxn (heat released by reaction, in J) = AH2m =(heat absorbed by mixture + Ceai AT) show calculations Moles of metal used. show calculations AHro1 in kJ/mol of metal used. show calculations Average AHn in k.J Is this reaction exothermic or endothermic? What is your experimental evidence supporting this? Is AHrn positive or negative? Make sure your Average AHrxn in kJ above shows the correct sign.
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