0
answers
0
watching
87
views
10 Nov 2019
Here are my lab notes from my different trials
![](https://prealliance-textbook-qa.oneclass.com/qa_images/homework_help/question/qa_images/99/9998361.png)
A.) Record thefollowing for each of the three trials:
Trial 1
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 34.9 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
Trail 2
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 43.8 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
Trail 3
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 52.7 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
B.) Calculate theheat released into the solution for the 3 reactions, according tothe formula:
qreaction = (Ccal * ?T) + (mcontents *Cpcontents * ?T)
Assume Cpcontents = Cpwater = 4.18 J/g�C
- Trial 1 (J):
- Trail 2 (J):
- Trail 3 (J):
C.) Find the molarheat of reaction for each experiment in units of kilojoules / (moleof Mg) by dividing the heat of reaction (converted to kJ bydividing by 1000) by the moles of Mg used.
- Trail 1 (kJ/mol):
- Trail 2 (kJ/mol):
- Trail 3 (kJ/mol):
D.) Calculate andrecord the average molar heat of reaction from the threeresults:
Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.15 g of magnesium (Mg) to the calorimeter (mass 68.738g, max temp. 34.9C) Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.25 g of magnesium (Mg) to the calorimeter (mass 68.829g, max temp. 43.8C) Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.35 g of magnesium (Mg) to the calorimeter (mass 68.921g, max temp. 52.7C)
Here are my lab notes from my different trials
A.) Record thefollowing for each of the three trials:
Trial 1
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 34.9 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
Trail 2
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 43.8 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
Trail 3
- Mass of the empty calorimeter (g):18.600g
- Initial temperature of the calorimeter (�C):21.5 C
- Maximum temperature in the calorimeter from thereaction (�C): 52.7 C
- Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
- Mass of the calorimeter and its contents after thereaction (g)
- Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
- Calculate the moles of Mg reacted (MW = 24.305g/mole)
B.) Calculate theheat released into the solution for the 3 reactions, according tothe formula:
qreaction = (Ccal * ?T) + (mcontents *Cpcontents * ?T)
Assume Cpcontents = Cpwater = 4.18 J/g�C
- Trial 1 (J):
- Trail 2 (J):
- Trail 3 (J):
C.) Find the molarheat of reaction for each experiment in units of kilojoules / (moleof Mg) by dividing the heat of reaction (converted to kJ bydividing by 1000) by the moles of Mg used.
- Trail 1 (kJ/mol):
- Trail 2 (kJ/mol):
- Trail 3 (kJ/mol):
D.) Calculate andrecord the average molar heat of reaction from the threeresults:
Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.15 g of magnesium (Mg) to the calorimeter (mass 68.738g, max temp. 34.9C) Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.25 g of magnesium (Mg) to the calorimeter (mass 68.829g, max temp. 43.8C) Clean, empty calorimeter has a mass of 18.600g and has a temp of 21.5 C Added 50 mL of 1.0 M hydrochloric acid (HCI) to the calorimeter (mass 68.600g, temp. 21.5 C) Added 0.35 g of magnesium (Mg) to the calorimeter (mass 68.921g, max temp. 52.7C)