ENTHALPY CHANGE FOR THE DECOMPOSITION OF AMMONIUM CHLORIDE SHOW WORK PLEASE!!!!!

Question

ENTHALPY CHANGE FOR THE DECOMPOSITION OF AMMONIUM CHLORIDE

SHOW WORK PLEASE!!!!!!!!!!

Experiment 1: Find the Calorimeter Constant

Take a constant temperature bath from the Instruments shelf and place it on the workbench.

Run the bath at 60 °C.

Take an Erlenmeyer flask from the Containers shelf and place it on the workbench.

Take water from the Materials shelf and add 50.0 mL to the flask.

Place the flask into the constant temperature bath.

Take a thermometer from the Instruments shelf and attach it to the flask.

Take a calorimeter from the Containers shelf and place it on the workbench.

Take water from the Materials shelf and add 50.0 mL to the calorimeter.

Take a thermometer from the Instruments and attach it to the calorimeter. Record the temperature in your Lab Notes. Remember to press Save Notes.

When the temperature of the water in the Erlenmeyer flask reaches 60 °C, remove the thermometer from the flask and drag and drop the flask onto the calorimeter. Select Pour All to empty the flask into the calorimeter.

Record the temperature of the combined liquid in the calorimeter in your Lab Notes.

Clear your station by dragging all containers and instruments to the recycling bin beneath the workbench.

Experiment 2: Determine the Enthalpy of Neutralization of HCl by NH3

Take a new calorimeter from the Containers shelf and place it on the workbench.

Take 2 M hydrochloric acid (HCl) solution from the Materials shelf and add 25.0 mL to the calorimeter.

Take a thermometer from the Instruments shelf and attach it to the calorimeter. Record the temperature inside the calorimeter in your Lab Notes.

Take 2 M ammonia (NH3) solution from the Materials shelf and add 25.0 mL to the calorimeter. Observe the temperature change in the calorimeter and record it in your Lab Notes. Make sure to record the highest temperature before the calorimeter begins to lose heat to the surroundings.

Clear your station by dragging all containers and instruments to the recycling bin. Remember to press Save Notes.

Experiment 3: Determine the Enthalpy of Dissolution of NH4Cl in Water

Take a new calorimeter from the Containers shelf and place it on the workbench.

Take water from the Materials shelf and add 25.0 mL to the calorimeter.

Take a thermometer from the Instruments shelf and attach it to the calorimeter. Record the temperature inside the calorimeter in your Lab Notes.

Take ammonium chloride (NH4Cl) from the Materials shelf and add 5.000 g to the calorimeter.

Observe the temperature change in the calorimeter as the reaction proceeds. Record the new temperature your Lab Notes.

Clear your station by dragging all containers and instruments to the recycling bin. Remember to press Save Notes.

NOTES:

Experiment 1:

1. temp in caloriometer is 21.5 degrees celsius

2. temp in caloriometer after poured was 39.9 degrees celsius

Experiment 2:

1. Initial temp of the 2 M hydrochloric acid is 21.5 degrees celsius

2. Temp rose to 33.2 celsius when 2 M ammonia was added

Experiment 3:

1. Initial temp is 21.5 degrees celsius

2. Temp dropped to 9.1 degrees celsius

Questions:

1. What was the mass of the cold water used?

A. 50 g

B. 18 g

C. 25 g

D. 10 g

2. How much heat was lost by the hot water? Choose the closest answer.

A. -3890 J

B. 3890 J

C. -4160 J

D. 4160 J

3. How much heat was absorbed by the cold water? Choose the closest answer.

A. -4160 J

B. -3890 J

C. 3890 J

D. 4160 J

4. How much heat was absorbed by the calorimeter? Choose the closest answer.

A. -4160 J

B. 390 J

C, 270 J

D. -270 J

5. What was the deltaT for the cold water? Choose the closest answer.

A. - 18.6 degrees celsius

B. 19.9 C

C. - 19.9 C

D. 18.6 C

6. What was the deltaT for the hot water? Choose the closest answer.

A. - 18.6 degrees celsius

B. 19.9 C

C. - 19.9 C

D. 18.6 C

7. The value of the calorimeter constant is between?

A. 75 and 80 J/C

B. 10 and 15 J/C

C. 20 and 30 J/C

D. 5 and 10 J/C

8. In Experiment 2, what was the initial temperature of the calorimeter with the HCl?

A. 50.3 C

B. 21.5 C

C. 79.6 C

D. 15.2 C

9. What was the total mass of solution in the calorimeter after NH3 neutralizes the HCl?

A. 25g

B. 50g

C. 75g

D. 100 g

10. What was the change in temperature (deltaT) when ammonia was added to the hydrochloric acid solution?

A. 21.5 C

B. 13.5 C

C. 33.2 C

D. 11.7 C

11. What is the heat of solution (qsoln) for the neutralization reaction between NH3 and HCl?

A. -1220 J

B. 1220 J

C. - 2450 J

D. 2450 J

12. What is the heat of reaction for the neutralization reaction between NH3 and HCl?

A. 2450 J

B. - 2450 J

C. 2620 J

D. -2620 J

13. In Experiment 3, what happened to the temperature of the solution in the calorimeter after the addition of NH4Cl?

B. The temp decreased

14. How many moles of NH4Cl did you add to the calorimeter? The molar mass of NH4Cl is 53.49 g/mol.

A. 0.0250 moles

B. 0.09348 moles

C. 5 moles

D. 53.49 moles

15. What was the heat of solution (qsoln) for the dissolution of ammonium chloride in water? Choose the closest answer.

A. 1740

B. 1560 J

C. -1740 J

D. -1560 J

16. What was the value of qcal for the dissolution of ammonium chloride in water? Choose the closest answer.

A. -1740 J

B. 14.6 J

C. 181 J

D. -181 J

17. What was the change of temperature (deltaT) for the dissolution of ammonium chloride in water? Choose the closest answer.

A. 12.4

B. 9.1

C. -12.4

18.

Based on the molar enthalpies calculated for experiment 2 and 3, use Hess's Law to write a series of reactions that will sum up to the reaction of the decomposition of ammonium chloride. In addition to the molar enthalpies from experiment 2 and 3, you will also need to include the following reactions which account for the enthalpy change when HCl and NH3change state.

NH3(g) -> NH3(aq) (deltaH = -34,640 J/mol)

HCl(g) -> HCl(aq) (deltaH = -75,140 J/mol)

Choose the equation that shows the correct direction and sign for the enthalpy value for the reaction between NH3 and HCl in your series of reactions.

19.

Given the data in the table below, what is the enthalpy of reaction for the following sulphur dioxide synthesis reaction?

S(s) + O2(g) -> SO2(g)

A. 593.6 K/J

B. -593.6 K/J

C. 296.8 K/J

D. -296.8 K/J

Explanation / Answer

1. What was the mass of the cold water used?

A. 50 g

B. 18 g

C. 25 g

D. 10 g

Volume of water is 50ml and density is 1.0 g/ ml

Thus mass = volume * density

= 50 ml* 1.0 g/ ml

= 50 g

Thus the correct answer is A. 50 g

2. How much heat was lost by the hot water? Choose the closest answer.

A. -3890 J

B. 3890 J

C. -4160 J

D. 4160 J

Q = mcdT

= 50*4.184* (33.2-21.5

= 4204.92 J

C. -4160 J

3. How much heat was absorbed by the cold water? Choose the closest answer.

A. -4160 J

B. -3890 J

C. 3890 J

D. 4160 J

Q = mcdT

= 50*4.184* (39.9-60.0

= 3849.28 J

C. 3890 J

4. How much heat was absorbed by the calorimeter? Choose the closest answer.

A. -4160 J

B. 390 J

C, 270 J

D. -270 J

heat was absorbed by the calorimeter =4160 J -3890 J

= 270 J

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