REPOST please help with reaction 2 and 3 under calculations (for reaction 2 help had been provide till part 3Note: Since you have posted a question with multiple sub-parts, we will provide the solution only to the first three sub-parts as per our Q&A guidelines. Please repost the remaining sub-parts separately.Given that:Initial temperature, T1 = 24.0oCFinal temperature, T2 = 32.1oCVolume of HCl = 100 mLDensity of HCl = 1 g/mLConcentration of HCl = 1.0 mol/L = 1.0 Marrow_forwardStep 21.) The change in temperature is calculated using the following expression:∆T=Final temprature-Initial temperature=T2-T1Substitute 32.1oC for T2, and 24.0oC for T1 in the above expression to calculate the change in temperature for reaction 2.∆T=32.1°C-24.0°C=8.1°Carrow_forwardStep 32.) The formula to calculate the mass of a substance is written as follows:Mass=Volume×DensitySubstitute 100 mL for the volume and 1 g/mL for the density in the above formula to calculate the mass of HCl.Mass of HCl=100 mL×1 g/mL=100 gStep 4 The specific heat capacity of 1M solution of HCl is 4.04 J g-1 oC-1.The formula to calculate the amount of heat released in reaction 2 is given as follows:Q=mC∆THere, m = mass of HClC = specific heat capacity of HCl∆T = Change in temperatureStep 5: Substitute 100 g for m, 4.04 J g-1 oC-1 for C, and 8.1 oC for ∆T in the above expression to calculate the amount of heat released in reaction 2.Q=100 g×4.04 J g-1 °C-1×8.1 °C=3272.4 J Step 63.) Unit conversion:1 kJ = 1000 Jor 1 J = 10-3 kJTherefore,Q=3272.4 J=3272.4×10-3 kJ=3.2724 kJ Although you will not be working with actual chemicals during this laboratory, since you will bedoing it virtually, the procedure is given in order for you to be aware of the process that would befollowed in a laboratory setting.IntroductionIn this experiment, you will use Hess's Law to determine the heat for a reaction that is difficult tomeasure directly. Magnesium metal burns rapidly, releasing light and heat, as observed in photoflashbulbs or by burning magnesium ribbon. The reaction is presented by the equation:Mg(s) + 1/2O2(g)MgO(s)This equation can be obtained by combining equations (2), (3) and (4):MgO(s) + 2HCl(aq) →→→→ MgCl₂(aq) + H₂OMg(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂(g)H₂(g) + 1/2O2(0)H₂O)Material(1)Safety(2)(3)By combining these three equations, you can obtain equation (1). The heats of reaction forequations (2) and (3) can easily be determined by experiments. The heat of reaction forequation (4) can be obtained from a table of values for previously measured reactions.(4)Chemicalsmagnesium, magnesium oxide, hydrochloric acidApparatus:Polystyrene calorimeter, graduated cylinder, electronic balance, filter paper, spatula,thermometer, glass stirring rod, stop watch,Safety goggles and a lab apron should always be worn when working with chemicals.This lab will be performed using small quantities of chemicals (micro-scale chemistry).ProcedureREACTION 2:1. Pour 100 mL of 1.0 mol/L hydrochloric acid into your polystyrene calorimeter.2. Weigh out 1.00 g of magnesium oxide on a filter paper.3. Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁(precise to 0.1°C). It may take several seconds for the temperature to stabilize.4. Add the magnesium oxide powder to the solution.5. Use a glass stirring rod to stir the cup contents until maximum temperature has beenreached and the temperature starts to drop.6. Record the maximum temperature, T₂REACTION 3:1. Pour 100 mL of 1.0 M hydrochloric acid into your polystyrene calorimeter.2. Weigh out 0.50 g of magnesium ribbon (this is about 46 cm). Roll it up loosely around apencil so that you end up with a coil. Make sure it is not too tightly coiled.3.Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁(precise to 0.1°C). It may take several seconds for the temperature to stabilize.4. Add the magnesium ribbon to the solution.5. Use a glass stirring rod to stir the cup contents until maximum temperature has beenreached and the temperature starts to drop.6. Record the maximum temperature, T₂. This video shows a similar procedure. Watch the video and answer the questions belowa) What were 3 pieces of lab equipment you saw in the video?b) What were some of the safety precautions they mentioned?c) Were the reactions shown the same as the ones in this lab? How can you tell?ResultsUse the table of standard enthalpies of formation to calculate the theoretical value.Sample results are provided below.Table #1: Volume, Temperature and Mass Values for Reactions 2 and 3Volume of HCIFinal temperature (T₂)Initial temperature (T₁)Change in temperature (AT)Mass of solidCalculations:3. Convert your answer into kJ.4. How many moles of MgO were used?5. Convert your answer into kJ/mol MgO.Reaction 31. Combine equations (2), (3) and (4) to obtain equation (1).Reaction 2Reaction 2(MgO)32.1°C% error-24.0°CConclusion0.96 g#experimental - # actual# actual1. Calculate the change in temperature for reaction (2).2. Calculate the energy released (AH) in (2) (in J), using Q=mcAT. The mass to be used isthe mass of HCI. Assume the density of hydrochloric acid to be 1 g/mL.x 100Reaction 3(Mg)48.2°C1. Calculate the change in temperature for reaction (3).2. Calculate the energy released (AH) in (3) (in J), using Q=mcAT. The mass to be used isthe mass of HCI.24.0°C3. Convert your answer into kJ.4. How many moles of Mg were used?5. Convert your answer into kJ/mol Mg.6. Calculate the heat of reaction (1) in kJ/mol of MgO by combining (2), (3) and (4) andtheir AH values that you obtained, in order to get equation (1) and its AH for thecombustion of Mg.0.55 g7. Determine the theoretical value for the combustion of magnesium, from the table ofstandard enthalpies of formation.8. Calculate the percentage error.Briefly state the results for the laboratory, in general. This should be no more than twosentences.

Given that: Initial temperature, T1 = 24.0oC Final temperature, T2 = 48.2oC Volume of HCl = 100 mL…

Answered: 1. Calculate the change in temperature…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Question

REPOST please help with reaction 2 and 3 under calculations (for reaction 2 help had been provide till part 3

Note: Since you have posted a question with multiple sub-parts, we will provide the solution only to the first three sub-parts as per our Q&A guidelines. Please repost the remaining sub-parts separately.

Given that:

Initial temperature, T₁= 24.0^oC

Final temperature, T₂= 32.1^oC

Volume of HCl = 100 mL

Density of HCl = 1 g/mL

Concentration of HCl = 1.0 mol/L = 1.0 M

arrow_forward

Step 2

1.) The change in temperature is calculated using the following expression:

∆T=Final temprature-Initial temperature=T2-T1

Substitute 32.1^oC for T₂, and 24.0^oC for T₁ in the above expression to calculate the change in temperature for reaction 2.

∆T=32.1°C-24.0°C=8.1°C

arrow_forward

Step 3

2.) The formula to calculate the mass of a substance is written as follows:

Mass=Volume×Density

Substitute 100 mL for the volume and 1 g/mL for the density in the above formula to calculate the mass of HCl.

Mass of HCl=100 mL×1 g/mL=100 g

Step 4 The specific heat capacity of 1M solution of HCl is 4.04 J g^-1^oC^-1.

The formula to calculate the amount of heat released in reaction 2 is given as follows:

Q=mC∆T

Here, m = mass of HCl

C = specific heat capacity of HCl

∆T = Change in temperature

Step 5: Substitute 100 g for m, 4.04 J g^-1^oC^-1for C, and 8.1 ^oC for ∆T in the above expression to calculate the amount of heat released in reaction 2.

Q=100 g×4.04 J g-1 °C-1×8.1 °C=3272.4 J

Step 6

3.) Unit conversion:

1 kJ = 1000 J

or 1 J = 10^-3 kJ

Therefore,

Q=3272.4 J=3272.4×10-3 kJ=3.2724 kJ

Although you will not be working with actual chemicals during this laboratory, since you will be
doing it virtually, the procedure is given in order for you to be aware of the process that would be
followed in a laboratory setting.
Introduction
In this experiment, you will use Hess's Law to determine the heat for a reaction that is difficult to
measure directly. Magnesium metal burns rapidly, releasing light and heat, as observed in photo
flashbulbs or by burning magnesium ribbon. The reaction is presented by the equation:
Mg(s) + 1/2O2(g)
MgO(s)
This equation can be obtained by combining equations (2), (3) and (4):
MgO(s) + 2HCl(aq) →→→→ MgCl₂(aq) + H₂O
Mg(s) + 2HCl(aq) →→→ MgCl₂(aq) + H₂(g)
H₂(g) + 1/2O2(0)
H₂O)
Material
(1)
Safety
(2)
(3)
By combining these three equations, you can obtain equation (1). The heats of reaction for
equations (2) and (3) can easily be determined by experiments. The heat of reaction for
equation (4) can be obtained from a table of values for previously measured reactions.
(4)
Chemicals
magnesium, magnesium oxide, hydrochloric acid
Apparatus:
Polystyrene calorimeter, graduated cylinder, electronic balance, filter paper, spatula,
thermometer, glass stirring rod, stop watch,
Safety goggles and a lab apron should always be worn when working with chemicals.
This lab will be performed using small quantities of chemicals (micro-scale chemistry).
Procedure
REACTION 2:
1. Pour 100 mL of 1.0 mol/L hydrochloric acid into your polystyrene calorimeter.
2. Weigh out 1.00 g of magnesium oxide on a filter paper.
3. Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁
(precise to 0.1°C). It may take several seconds for the temperature to stabilize.
4. Add the magnesium oxide powder to the solution.
5. Use a glass stirring rod to stir the cup contents until maximum temperature has been
reached and the temperature starts to drop.
6. Record the maximum temperature, T₂
REACTION 3:
1. Pour 100 mL of 1.0 M hydrochloric acid into your polystyrene calorimeter.
2. Weigh out 0.50 g of magnesium ribbon (this is about 46 cm). Roll it up loosely around a
pencil so that you end up with a coil. Make sure it is not too tightly coiled.
3.
Place the thermometer in the hydrochloric acid to obtain the initial temperature, T₁
(precise to 0.1°C). It may take several seconds for the temperature to stabilize.
4. Add the magnesium ribbon to the solution.
5. Use a glass stirring rod to stir the cup contents until maximum temperature has been
reached and the temperature starts to drop.
6. Record the maximum temperature, T₂.

This video shows a similar procedure. Watch the video and answer the questions below
a) What were 3 pieces of lab equipment you saw in the video?
b) What were some of the safety precautions they mentioned?
c) Were the reactions shown the same as the ones in this lab? How can you tell?
Results
Use the table of standard enthalpies of formation to calculate the theoretical value.
Sample results are provided below.
Table #1: Volume, Temperature and Mass Values for Reactions 2 and 3
Volume of HCI
Final temperature (T₂)
Initial temperature (T₁)
Change in temperature (AT)
Mass of solid
Calculations:
3. Convert your answer into kJ.
4. How many moles of MgO were used?
5. Convert your answer into kJ/mol MgO.
Reaction 3
1. Combine equations (2), (3) and (4) to obtain equation (1).
Reaction 2
Reaction 2
(MgO)
32.1°C
% error-
24.0°C
Conclusion
0.96 g
#experimental - # actual
# actual
1. Calculate the change in temperature for reaction (2).
2. Calculate the energy released (AH) in (2) (in J), using Q=mcAT. The mass to be used is
the mass of HCI. Assume the density of hydrochloric acid to be 1 g/mL.
x 100
Reaction 3
(Mg)
48.2°C
1. Calculate the change in temperature for reaction (3).
2. Calculate the energy released (AH) in (3) (in J), using Q=mcAT. The mass to be used is
the mass of HCI.
24.0°C
3. Convert your answer into kJ.
4. How many moles of Mg were used?
5. Convert your answer into kJ/mol Mg.
6. Calculate the heat of reaction (1) in kJ/mol of MgO by combining (2), (3) and (4) and
their AH values that you obtained, in order to get equation (1) and its AH for the
combustion of Mg.
0.55 g
7. Determine the theoretical value for the combustion of magnesium, from the table of
standard enthalpies of formation.
8. Calculate the percentage error.
Briefly state the results for the laboratory, in general. This should be no more than two
sentences.

Expert Solution

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

1. Calculate the change in temperature for reaction (3). 2. Calculate the energy released (AH) in (3) (in J), using Q=mcAT. The mass to be used is the mass of HCI. 3. Convert your answer into kJ. 4. How many moles of Mg were used? 5. Convert your answer into kJ/mol Mg.