Heat enthalpy of reaction and calorimetry lab report

Lab Report Chemistry 1

Determining the Enthalpy of a Chemical Reaction

Introduction

Thermochemistry is the study of energy and its transformations. As chemical bonds break and

form in a chemical reaction, energy in the form of heat (qrxn) is either released or absorbed by the

reaction (the system). At constant pressure (coffee cup calorimetry), the heat released or absorbed

is equal to the enthalpy change (ΔHrxn) of the reaction. The heat exchanged between the system

and surroundings can be measured if the reaction is performed in a container, known as a

calorimeter which insulates the reaction from its surroundings. If heat is released, the reaction is

exothermic and ΔH will be negative. If heat is absorbed, the reaction is endothermic and ΔH will

be positive.

In this experiment, you will determine enthalpy changes (ΔHrxn) of chemical reactions by coffee

cup calorimetry. It is difficult to directly measure heat exchange between reactants and products

(the system) directly. Therefore, we measure the heat change that occurs in the surroundings by

monitoring temperature changes at constant pressure. If we conduct a reaction between two

substances in aqueous solution, then the heat gained or lost by the solution can be calculated with

the following equation:

qsoln = Cp x m x ∆T

qsoln represents the heat that is gained or lost by the solution; Cp is the specific heat of water (4.18

J / g ºC); m is the mass of water, and ∆T is the temperature change of the solution.

The Styrofoam cups used to carry out the reactions are good insulators; however, they still absorb

some of the heat exchange involved in the reaction. Therefore, the heat of the calorimeter (qcal)

must also be taken into consideration to accurately calculate qrxn. Therefore, the heat gained/ lost

by the solution and the calorimeter is equal to the heat lost/ gained by the reaction:

(qcal + qsoln) = - qrxn qrxn = ΔHrxn (at constant pressure)

In this experiment, you will determine the calorimeter constant (Ccal) of two Styrofoam cup

calorimeters. You will also measure ΔHrxn for a series of reactions and use Hess’s Law to compare

calculated ΔHrxn values to experimental values.

This is a 2 week lab. Part A will be completed during week 1 and Part B will be completed

during week 2.

Week 1

Part A: You will be given two Styrofoam cups and some aluminum foil to make two calorimeters.

You will need to determine the heat capacity of your calorimeter (Ccal). By definition, Ccal is

defined as the amount of heat required to raise the temperature of the calorimeter 1 oC. To

determine Ccal you will measure the temperature change associated with mixing warm water with

room temperature water. The heat lost by the warm water is equal to the heat gained by both the

room temperature water and the calorimeter apparatus. The heat gained by the room temperature

water and the calorimeter is equal to the heat lost by the warm water. ΔT will be (Tfinal – Tinitial).

Therefore,

qlost = (specific heat of water) x (grams of warm water) x (ΔTlost)

qgain = (specific heat of water) x (grams of room temperature water) x (ΔTgain)

The heat gained by the calorimeter, qcal, is the difference between the heat lost by the warm water

and the heat gained by the room temperature water. Since qlost is negative, qcal is

qcal = - (qlost + qgain)

Therefore, to calculate the Ccal, the heat gained by the calorimeter (qcal) is divided by the change

in the temperature of the calorimeter. Since the room temperature water was in the calorimeter to

start and the temperature of the calorimeter increased, the change in temperature of the calorimeter

will be equal to ΔTgain.

Ccal = qcal / ΔTgain

You will need to take the heat capacity of the calorimeter into consideration for each of your

enthalpy calculations in this experiment.

Objectives

In this experiment, you will

• Determine the heat capacity of two Styrofoam cup calorimeters.

• Determine ΔHrxn for three neutralization reactions

• Use Hess’s law to determine the enthalpy change of an acid-base reaction and compare your

calculated value to your experimental results.

• Determine the heat of solution for dissolving a salt in water.

• Determine the heat of reaction for a redox reaction.

Equipment, Chemicals and Supplies

You will need a 50mL graduated cylinder from your drawer. The stockroom will provide all other

materials for weeks 1 and 2. You will need to keep the Styrofoam cups used as calorimeters in the

experiment between weeks 1 and 2. Make sure they are clearly labeled. YOU MUST RECORD

YOUR BOX NUMBER AND MAKE SURE YOU GET THE SAME BOX NUMBER NEXT WEEK.

Vernier Lab Quest Ring stand

Temperature probe Utility clamp

4 Styrofoam cups Aluminum foil/or cup lid

Stir plate Small stir bar

Safety

Wear goggles and lab coat throughout the experiment.

Procedure Week 1:

Part A: Determining the Heat Capacity of the Calorimeter

Your team of four will split into two teams of two to perform this part of the experiment.

You will complete 3 trials with your partner, then exchange data with the other two members

of the group to get two sets of calorimeter constants. Make sure the calorimeters are clearly

labeled as 1 and 2.

1. Nest two Styrofoam cups inside of each other to make your calorimeter. Add the magnetic

stir bar to the calorimeter (inner cup).

2. Cover the opening of the calorimeter with the aluminum foil /or cup lid. With a pencil tip,

pierce a small hole close to the edge of the cup (Figure 1). The hole should be small to

avoid heat loss.

Figure 1 Figure 2

3. Assemble the ring stand, utility clamp, and stir plate as seen in Figure 2. Place your

calorimeter inside the ring holder and rest it on the stir plate.

4. Measure 25 mL of room temperature water with a graduated cylinder. Remove the

aluminum foil and pour the water into the calorimeter.

5. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

6. Carefully insert the temperature probe through the punctured hole in the aluminum foil

(Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be careful not

to puncture the bottom of the calorimeter.

7. Connect the temperature probe to Channel 1 of the Vernier LabQuest. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

8. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

9. Stir the room temperature water in the calorimeter for 3 minutes to allow the apparatus to

reach thermal equilibrium. After 3 minutes, record the temperature as the initial

temperature of the room temperature water on your data sheet.

10. Use a graduated cylinder to measure 25 mL of warm water. Remove the temperature probe

from the calorimeter and measure the temperature of the warm water. The initial reading

of the warm water should be over 70 ºC. Record the temperature of the warm water on your

data before mixing.

11. Place the temperature probe back in the calorimeter which contains the room temperature

water.

12. Start the LabQuest.

13. Lift the side of the aluminum foil and add the warm water into the calorimeter that contains

the room temperature water. Tightly re-cover the opening of the calorimeter with the

aluminum foil and allow to stir for 3 minutes.

14. After 3 minutes, record the maximum temperature observed on the LabQuest unit on your

data sheet (Tfinal).

15. Empty your calorimeter, dry all parts completely, and allow all equipment to return to room

temperature.

16. Repeat steps 4-15 to complete the remaining 2 trails for the calorimeter.

17. Calculate the calorimeter constant (Ccal) using the values for the heat gained or lost by the

calorimeter and the change in temperature.

18. For your calculations in Part B, you should use the average Ccal value for each of your

calorimeters.

Week 2

Part B: In Part B of this experiment you will experimentally determine the enthalpy change of

five reactions. The first three reactions are the acid-base reactions listed below.

1. NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

2. NaOH(aq) + NH4Cl(aq) → NaCl(aq) + NH3(aq) + H2O(l)

3. HCl(aq) + NH3(aq) → NH4Cl(aq)

In addition to experimentally determining the ΔHrxn for each of these reaction, you can use Hess’s

Law to determine the enthalpy change of reaction 3 above by manipulating reactions 1 and 2. You

will compare your calculated value of ΔHrxn for 3 to your experimentally determined value.

You will also determine the heat of reaction for two additional reactions: (1) dissolving ammonium

nitrate in water and (2) the redox reaction that results from dissolving magnesium powder in

hydrochloric acid.

Equipment, Chemicals and Supplies

Vernier LabQuest 2.0 M hydrochloric acid solution

Fume hood 2.0 M sodium hydroxide solution

Temperature Probe 2.0 M ammonium chloride solution

2 Styrofoam cup calorimeter 2.0 M ammonium hydroxide solution

400 mL beaker Ammonium nitrate salt

50 mL graduated cylinder Magnesium powder

Thermometer aluminum foil/or cup lid

Stir plate and small magnetic stir bar Electronic balance

Ring stand Utility clamp

Safety : ALL REACTIONS SHOULD BE PERFORMED IN THE HOOD

● Goggles and lab coat must be worn throughout the experiment.

● These reactions will be performed in the fume hoods to avoid inhaling hazardous gases.

● Handle all reagents with care to avoid coming in contact with the skin. They may cause

painful burns.

● If any chemicals get on your skin, rinse thoroughly for at least 15 minutes.

Procedure Week 2: ALL REACTIONS SHOULD BE PERFORMED IN THE HOOD

Failure to perform these reactions in the fume hood will result in dismissal from lab and a

zero for this experiment.

Part B: Determining Heat of Reactions

You must collect all reaction solutions in a waste beaker at your bench and discard in waste

container A at the end of the experiment.

Reaction between HCl and NaOH

NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)

1. Add the magnetic stir bar to the calorimeters (inner cup) used in Part A.

2. Cover the opening of the calorimeter with the aluminum foil. With a pencil tip, pierce a

small hole close to the edge of the cup (Figure 1). The hole should be small to avoid heat

loss.

3. Assemble the ring stand, utility clamp, and stir plate as seen in Figure 2. Place your

calorimeter inside the ring holder and rest it on the stir plate.

4. Measure 25 mL of 2.0 M HCl solution with a graduated cylinder. Remove the aluminum

foil/or cup lid and pour the HCl solution into the calorimeter.

5. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

6. Carefully insert the temperature probe through the punctured hole in the aluminum foil/or

cup lid (Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be careful

not to puncture the bottom of the calorimeter.

7. Connect the temperature probe to Channel 1 of the LabQuest unit. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

8. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

9. Stir the HCl solution in the calorimeter for 3 minutes to allow the apparatus to reach thermal

equilibrium.

10. While stirring the HCl solution, measure 25 mL of 2.0 M NaOH solution with a clean

graduated cylinder. Do not add it to the HCl solution yet.

11. After the HCl solution has been stirred for 3 minutes, record the temperature as the initial

temperature of the HCl solution on your data sheet.

12. Start the LabQuest. Lift the side of the aluminum foil and add the NaOH solution to the

calorimeter. Tightly re-cover the opening of the calorimeter with the aluminum foil/or cup

lid and allow to stir for 3 minutes.

13. After 3 minutes, record the maximum temperature observed on the LabQuest on your data

sheet.

14. Rinse and dry the temperature probe, calorimeter, and the stir bar. Dispose of the solution

in your waste beaker.

15. Calculate ΔHrxn.

Reaction between NaOH and NH4Cl

NaOH(aq) + NH4Cl(aq) → NaCl(aq) + NH3(aq) + H2O(l)

1. Add the magnetic stir bar to of the calorimeters (inner cup) used in Part A.

2. Measure 25 mL of 2.0 M NaOH solution with a graduated cylinder. Remove the aluminum

foil/or cup lid and pour the NaOH solution into the calorimeter.

3. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

4. Carefully insert the temperature probe through the punctured hole in the aluminum foil/or

cup lid (Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be

careful not to puncture the bottom of the calorimeter.

5. Connect the temperature probe to Channel 1 of the LabQuest unit. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

6. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

7. Stir the NaOH solution in the calorimeter for 3 minutes to allow the apparatus to reach

thermal equilibrium.

8. While stirring the NaOH solution, measure 25 mL of 2.0 M NH4Cl solution with a clean

graduated cylinder. Do not add it to the NaOH solution yet.

9. After the NaOH solution has been stirred for 3 minutes, record the temperature as the initial

temperature of the NaOH solution on your data sheet.

10. Start the LabQuest. Lift the side of the aluminum foil/or cup lid and add the NH4Cl solution

to the calorimeter. Tightly re-cover the opening of the calorimeter with the aluminum

foil/or cup lid and allow to stir for 3 minutes.

11. After 3 minutes, record the maximum temperature observed on the LabQuest on your data

sheet.

12. Rinse and dry the temperature probe, calorimeter, and the stir bar. Dispose of the solution

in your waste beaker.

13. Calculate ΔHrxn.

Reaction between HCl and NH4OH

HCl(aq) + NH3(aq) → NH4Cl(aq)

1. Add the magnetic stir bar to the calorimeters (inner cup) used in Part A.

2. Measure 25 mL of 2.0 M HCl solution with a graduated cylinder. Remove the aluminum

foil/or cup lid and pour the HCl solution into the calorimeter.

3. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

4. Carefully insert the temperature probe through the punctured hole in the aluminum foil /or

cup lid (Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be careful

not to puncture the bottom of the calorimeter.

5. Connect the temperature probe to Channel 1 of the LabQuest unit. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

6. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

7. Stir the HCl solution in the calorimeter for 3 minutes to allow the apparatus to reach thermal

equilibrium.

8. While stirring the HCl solution, measure 25 mL 2.0 M NH3 solution (NH3 = NH4OH in

solution), with a clean graduated cylinder. Do not add it to the HCl solution yet.

9. After the HCl solution has been stirred for 3 minutes, record the temperature as the initial

temperature of the HCl solution on your data sheet.

10. Start the LabQuest. Lift the side of the aluminum foil /or cup lid and add the NH3 solution

to the calorimeter. Tightly re-cover the opening of the calorimeter with the aluminum

foil/or cup lid and allow to stir for 3 minutes.

11. After 3 minutes, record the maximum temperature observed on the LabQuest on your data

sheet.

12. Rinse and dry the temperature probe, calorimeter, and the stir bar. Dispose of the solution

in your waste beaker.

13. Calculate ΔHrxn.

Heat of Solution for Dissolving Ammonium Nitrate

1. Add the magnetic stir bar to the calorimeters (inner cup) used in Part A.

2. Measure 50 mL of deionized room temperature water with a graduated cylinder. Remove

the aluminum foil and pour the water into the calorimeter.

3. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

4. Carefully insert the temperature probe through the punctured hole in the aluminum foil/or

cup lid(Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be careful

not to puncture the bottom of the calorimeter.

5. Connect the temperature probe to Channel 1 of the LabQuest unit. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

6. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

7. Stir the water in the calorimeter for 3 minutes to allow the apparatus to reach thermal

equilibrium.

8. While waiting, use the electronic balance to weigh 2.5 g of ammonium nitrate in a plastic

weigh boat.

9. After 3 minutes, record the temperature as the initial temperature of the water on your

data sheet.

10. Start the LabQuest. Lift the side of the aluminum foil/or cup lid and add the ammonium

nitrate to the calorimeter. Tightly re-cover the opening of the calorimeter with the

aluminum foil/or cup lid and allow to stir for 3 minutes.

11. After 3 minutes, record the maximum temperature observed on the LabQuest on your data

sheet.

12. Rinse and dry the temperature probe, calorimeter, and the stir bar. Dispose of the solution

in your waste beaker.

13. Calculate ΔHrxn.

Heat of Reaction for a Redox Reaction

1. Add the magnetic stir bar to the calorimeters (inner cup) used in Part A.

2. Measure 50 mL of 2.0 M HCl solution with a graduated cylinder. Remove the aluminum

foil and pour the HCl solution into the calorimeter.

3. Tightly cover the top of the calorimeter with the aluminum foil/or cup lid.

4. Carefully insert the temperature probe through the punctured hole in the aluminum foil/or

cup lid (Figure 1). Secure the temperature probe with the utility clamp (Figure 2). Be careful

not to puncture the bottom of the calorimeter.

5. Connect the temperature probe to Channel 1 of the LabQuest unit. Plug in the LabQuest,

turn it on, and set the data collection time to 180 seconds (3 minutes).

6. Turn on the stir plate. **The temperature probe is placed carefully to the side of the cup

to avoid collisions with the magnetic stir bar, carefully adjust probe if this happens**

7. Stir the HCl solution in the calorimeter for 3 minutes to allow the apparatus to reach thermal

equilibrium.

8. While waiting, use the electronic balance to weigh 0.5 g of magnesium in a plastic weigh

boat.

9. After 3 minutes, record the temperature as the initial temperature of the HCl solution on

your data sheet.

10. Start the LabQuest. Lift the side of the aluminum foil/or cup lid and add the magnesium to

the calorimeter. Tightly re-cover the opening of the calorimeter with the aluminum foil/or

cup lid and allow to stir for 3 minutes.

11. After 3 minutes, record the maximum temperature observed on the LabQuest on your data

sheet.

12. Rinse and dry the temperature probe, calorimeter, and the stir bar. Dispose of the solution

in your waste beaker.

13. Calculate ΔHrxn.

Pour the contents of the waste beaker in waste container A. Rinse all

Styrofoam cups thoroughly and return them to the stockroom.

Report: A Template for the report is provided on Canvas. Be sure to follow the instructions in the

template for each section of the report.

Discussion Questions

Answer the following questions in the Discussion section of your report. You should consider

these questions as you are performing your experiment. Take enough notes so that you can answer

the questions after you have finished the experiment.

1. Using Hess’s Law, manipulate your ΔHrxn values for reaction 1 and 2 to calculate an

expected ΔHrxn value for reaction 3. How does your calculated value compare to your

experimental value? Include the calculations and the balanced equations for determining

Hess’s Law. (5 pts.)

2. For each of the reactions performed in this experiment, identify each of them as either

exothermic or endothermic. (5 pts.)

3. Why do you use a Styrofoam cup calorimeter instead of a glass beaker for these reactions?

(5 pts.) (Hint: Compare heat capacities)

4. Write down the balanced equation for reaction between HCl and Mg? What is the gas

released in this reaction? (5 pts.)

5. What do you expect to see if you use Mg strips instead of Mg powder? Comment on the

similarity and/or differences in the rate and heat of the reaction (5 pts.)

Data Sheet Calorimetry (Part A)

Names: ________________________________________________________________

Section: _______________ Date: ______________________________

Heat Capacity of Calorimeter #1:

Trial 1 Trial 2 Trial 3

Initial temperature of room temperature water from

temperature probe, Ti (ºC)

Mass (g) room temperature water (density = 1.0 g/mL)

Initial temperature of warm water from thermometer, Ti (ºC)

Mass (g) warm temperature water (density = 1.0 g/mL):

Maximum temperature observed over 3 minutes, Tf (ºC)

ΔTlost (warm water) (ºC)

qlost (warm water) (J)

ΔTgain (room T water) (ºC)

qgain (room T water) (J)

qcal (J)

Ccal (J/oC)

Average Ccal for calorimeter #1 (J/ oC)

Show sample calculations done on one of the trials for one Calorimeter. Define the variables

of the equations and include units.

Heat Capacity of Calorimeter #2:

Trial 1 Trial 2 Trial 3

Initial temperature of room temperature water from

temperature probe, Ti (ºC)

Mass (g) room temperature water (density = 1.0 g/mL)

Initial temperature of warm water from thermometer, Ti (ºC)

Mass (g) warm temperature water (density = 1.0 g/mL):

Maximum temperature observed over 3 minutes, Tf (ºC)

ΔTlost (warm water) (ºC)

qlost (warm water) (J)

ΔTgain (room T water) (ºC)

qgain (room T water) (J)

qcal (J)

Ccal (J/oC)

Average Ccal for calorimeter #1 (J/ oC)

Data Sheet Calorimetry (Part B)

Names: _______________________________________________________________

Section: ___________ Date: _____________________________

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, Ti (ºC)

Tf after mixing (highest or lowest T over 3 minutes) (ºC)

ΔT (ºC)

qsoln (kJ)

qcal (kJ)

qrxn (kJ)

ΔHrxn (kJ)

Average ΔHrxn (kJ)

Exothermic or Endothermic?

Show sample calculations done on one of the trials for any of the reactions.

2. Reaction between NaOH and NH4Cl

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, Ti (ºC)

Tf after mixing (highest or lowest T over 3 minutes) (ºC)

ΔT (ºC)

qsoln (kJ)

qcal (kJ)

qrxn (kJ)

ΔHrxn (kJ)

Average ΔHrxn (kJ)

Exothermic or Endothermic?

3. Reaction between HCl and NH4OH

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, Ti (ºC)

Tf after mixing (highest or lowest T over 3 minutes) (ºC)

ΔT (ºC)

qsoln (kJ)

qcal (kJ)

qrxn (kJ)

ΔHrxn (kJ)

Average ΔHrxn (kJ)

Exothermic or Endothermic?

Using Hess’s Law and your average ΔHrxn for reactions 1

and 2, what would you have expected ΔHrxn to equal

Show all calculations done to determine Hess’s Law. Define the variables of the equations

and include units.

4. Heat of Solution for Dissolving Ammonium Nitrate

Trial 1 – Calorimeter #1 Trial 2 – Calorimeter #2

Mass of entire solution, (g) (density = 1.0 g/mL)

Initial temperature of water prior to mixing, Ti (ºC)

Tf after mixing (highest or lowest T over 3 minutes) (ºC)

ΔT (ºC)

qsoln (kJ)

qcal (kJ)

qrxn (kJ)

ΔHrxn (kJ)

Average ΔHrxn (kJ)

Exothermic or Endothermic?

5. Heat of Reaction for a Redox Reaction

Trial 1 – Calorimeter #1 Trial 2 – Calorimeter #2

Mass of entire solution, (g) (density = 1.0 g/mL)

Initial temperature of HCl prior to mixing, Ti (ºC)

Tf after mixing (highest or lowest T over 3 minutes) (ºC)

ΔT (ºC)

qsoln (kJ)

qcal (kJ)

qrxn (kJ)

ΔHrxn (kJ)

Average ΔHrxn (kJ)

Exothermic or Endothermic?