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using 50 mL of HCl and .25g of magnesium. Record the MAXIMUMtemperature displayed by the thermometer in the calorimeter.

1. Record the following for each of the three experiments:

(a) Mass of the empty calorimeter (g):

(b) Initial temperature in the calorimeter (C):

(c) Maximum temperature in the calorimeter from the reaction(C):

(d) Calculate deltaT as Tmaximum - Tinitial (C):

(e) Mass of the calorimeter and its contents after the reaction(g):

(f) Calculate the mass of the contents of the calorimeter(g):

(g) Calculate the moles of Mg reacted (MW=24.305 g/mole):

2. Calculate the heat released into the solution for the 3reactions, according to:

q(reaction) = Ccal * Delta T + mass(contents) * Cp (contents) *deltaT

(If you have not measured the calorimeter constant yet, assume thatit is zero for this experiment.)


3. Find the molar heat of reaction for each experiment in units ofJoules / (mole of Mg) by dividing the heat of reaction by the molesof Mg used.


4. Calculate and record the average molar heat of reaction from thethree results.

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Sixta Kovacek
Sixta KovacekLv2
28 Sep 2019

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Related questions

Hi, I am providing all of the information as it is probably needed to answer the last couple of questions. I need help answering the last three boxes.

1. Calculate the heat released into the solution for the 3 reactions, according to Reaction= Ccal*Delta T+ m contents * Cp contents * Delta T.

2. Find the molar heat of reaction for each experiment in units of Kilo-Joules / (mole of Mg) by dividing the heat of reaction by the moles of Mg used.

3. Calculate and record the average molar heat of reaction from the three results.

Thank you for your help.

The Effect of Substrate Concentration on Catalase Activity

A. Mass of the empty calorimeter (g):

18.600g

B. Initial temperature of the calorimeter (°C):

21.5C

C. Maximum temperature in the calorimeter from the reaction (°C):

34.5C

D. Calculate delta T by subtracting (b) from (c) (°C) delta T = Tmaximum – Tinitial:

34.5-21.5 = 13C

E. Mass of the calorimeter and its contents after the reaction (g):

68.738g

F. Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)

68.738-18.600=50.138g

G. Calculate the moles of Mg reacted (MW = 24.305 g/mole)

50.138/24.305=2.0628 moles

The Effect of Substrate Concentration on Catalase Activity 2

A. Mass of the empty calorimeter (g):

18.600g

B. Initial temperature of the calorimeter (°C):

21.5C

C. Maximum temperature in the calorimeter from the reaction (°C):

43.2C

D. Calculate delta T by subtracting (b) from (c) (°C) delta T = Tmaximum – Tinitial:

43.2-21.5= 21.7C

E. Mass of the calorimeter and its contents after the reaction (g):

68.829g

F. Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)

68.829-18.600=50.229g

G. Calculate the moles of Mg reacted (MW = 24.305 g/mole)

50.229/24.305=2.066moles

The Effect of Substrate Concentration on Catalase Activity 3

A. Mass of the empty calorimeter (g):

18.600g

B. Initial temperature of the calorimeter (°C):

21.5C

C. Maximum temperature in the calorimeter from the reaction (°C):

51.8C

D. Calculate delta T by subtracting (b) from (c) (°C) delta T = Tmaximum – Tinitial:

51.8-21.5= 30.3C

E. Mass of the calorimeter and its contents after the reaction (g):

68.921g

F. Calculate the mass of the contents of the calorimeter (g) by subtracting (a) from (e)

68.921-18.600=50.321g

G. Calculate the moles of Mg reacted (MW = 24.305 g/mole)

50.321/24.305=2.07moles

Calculate the heat released into the solution for the 3 reactions, according to: Reaction= Ccal*Delta T+ m contents * Cp contents * Delta T

Trial 1

Trial 2

Trial 3

Find the molar heat of reaction for each experiment in units of Kilo-Joules / (mole of Mg) by dividing the heat of reaction by the moles of Mg used.

Trial 1

Trial 2

Trial 3

Calculate and record the average molar heat of reaction from the three results.

Average

Here are my lab notes from my different trials

A.) Record thefollowing for each of the three trials:

Trial 1

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 34.9 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. Calculate the moles of Mg reacted (MW = 24.305g/mole)

Trail 2

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 43.8 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. Calculate the moles of Mg reacted (MW = 24.305g/mole)

Trail 3

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 52.7 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. 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

  1. Trial 1 (J):
  2. Trail 2 (J):
  3. 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.

  1. Trail 1 (kJ/mol):
  2. Trail 2 (kJ/mol):
  3. Trail 3 (kJ/mol):

D.) Calculate andrecord the average molar heat of reaction from the threeresults:

Here are my lab notes from my different trials

A.) Record thefollowing for each of the three trials:

Trial 1

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 34.9 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. Calculate the moles of Mg reacted (MW = 24.305g/mole)

Trail 2

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 43.8 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. Calculate the moles of Mg reacted (MW = 24.305g/mole)

Trail 3

  1. Mass of the empty calorimeter (g):18.600g
  2. Initial temperature of the calorimeter (�C):21.5 C
  3. Maximum temperature in the calorimeter from thereaction (�C): 52.7 C
  4. Calculate ?T by subtracting (b) from (c) (�C) ?T =Tmaximum � Tinitial
  5. Mass of the calorimeter and its contents after thereaction (g)
  6. Calculate the mass of the contents of the calorimeter(g) by subtracting (a) from (e)
  7. 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

  1. Trial 1 (J):
  2. Trail 2 (J):
  3. 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.

  1. Trail 1 (kJ/mol):
  2. Trail 2 (kJ/mol):
  3. Trail 3 (kJ/mol):

D.) Calculate andrecord the average molar heat of reaction from the threeresults:

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