AH and Calorimetry: 8. Suppose 33mL of 1.20M HCI is added to 42mL of a solution containing excess sodium hydroxide in a coffee-cup calorimeter. 31.8°C. COMPARE ANSWER WITH PROBLEM #9. a. Provide a thermochemical equation, including AH in kJ. (include sign) b. What is the energy (AH) evolved in kJ per mole of HCI? (include sign) For simplicity, assume the heat capacity and the density of the final solution are those of H20. (Note: in more accurate work, these values are not the same and must be calculated). Also assume that the total volume of the solution equals the sum of the volumes of HCI(aq) and NaOH(aq). work space Provide a thermochemical equation. The solution temperature, originally at 25.0°C, rises to a) b. Show your work/calculations
AH and Calorimetry: 8. Suppose 33mL of 1.20M HCI is added to 42mL of a solution containing excess sodium hydroxide in a coffee-cup calorimeter. 31.8°C. COMPARE ANSWER WITH PROBLEM #9. a. Provide a thermochemical equation, including AH in kJ. (include sign) b. What is the energy (AH) evolved in kJ per mole of HCI? (include sign) For simplicity, assume the heat capacity and the density of the final solution are those of H20. (Note: in more accurate work, these values are not the same and must be calculated). Also assume that the total volume of the solution equals the sum of the volumes of HCI(aq) and NaOH(aq). work space Provide a thermochemical equation. The solution temperature, originally at 25.0°C, rises to a) b. Show your work/calculations
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...
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Can someone please explain how to do this in detail and show me how to do the work. I have 2 more problems like this and I need to learn how to set it up and complete it and why.
Thank you in advance!
![**ΔH and Calorimetry:**
8. Suppose 33 mL of 1.20 M HCl is added to 42 mL of a solution containing excess sodium hydroxide in a coffee-cup calorimeter. The solution temperature, originally at 25.0°C, rises to 31.8°C. COMPARE ANSWER WITH PROBLEM #9.
a. Provide a thermochemical equation, **including ΔH in kJ**. (Include sign)
b. What is the **energy (ΔH) evolved in kJ per mole of HCl**? (Include sign)
- For simplicity, assume the heat capacity and the density of the final solution are those of H₂O. (Note: in more accurate work, these values are not the same and must be calculated). Also assume that the total volume of the solution equals the sum of the volumes of HCl(aq) and NaOH(aq).
**Work space** Provide a thermochemical equation.
a) [Workspace for providing equation]
b. Show your work/calculations
**Must include a sign**
9. (Basically the same reaction as #8 above, **without some of the assumptions**)
In one experiment, a student placed 50.0 mL of 1.00 M HCl at 25.5°C in a coffee-cup calorimeter. To this was added 50.0 mL of 1.00 M NaOH solution also at 25.5°C. The mixture was stirred, and the temperature quickly increased to a maximum of 32.2°C.
a. Provide a thermochemical reaction, **including ΔH in kJ**. (Include sign)
b. What is the **energy (ΔH) evolved in kJ per mole of HCl**? (Include sign)
- Because the solutions are relatively dilute, we can assume their specific heats are close to that of H₂O, 4.184 J/g°C. However, **do not assume** the density of the solutions is that of water.
- The density of 1.00 M HCl is 1.20 g/mL and 1.00 M NaOH is 1.40 g/mL.
**Work space** Provide a thermochemical equation.
a) [Workspace for providing equation]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c1acf50-412f-4982-8252-15b8622c1b87%2F1c6b0c9c-10c0-48ed-8618-311076e7e024%2Frn2bvk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**ΔH and Calorimetry:**
8. Suppose 33 mL of 1.20 M HCl is added to 42 mL of a solution containing excess sodium hydroxide in a coffee-cup calorimeter. The solution temperature, originally at 25.0°C, rises to 31.8°C. COMPARE ANSWER WITH PROBLEM #9.
a. Provide a thermochemical equation, **including ΔH in kJ**. (Include sign)
b. What is the **energy (ΔH) evolved in kJ per mole of HCl**? (Include sign)
- For simplicity, assume the heat capacity and the density of the final solution are those of H₂O. (Note: in more accurate work, these values are not the same and must be calculated). Also assume that the total volume of the solution equals the sum of the volumes of HCl(aq) and NaOH(aq).
**Work space** Provide a thermochemical equation.
a) [Workspace for providing equation]
b. Show your work/calculations
**Must include a sign**
9. (Basically the same reaction as #8 above, **without some of the assumptions**)
In one experiment, a student placed 50.0 mL of 1.00 M HCl at 25.5°C in a coffee-cup calorimeter. To this was added 50.0 mL of 1.00 M NaOH solution also at 25.5°C. The mixture was stirred, and the temperature quickly increased to a maximum of 32.2°C.
a. Provide a thermochemical reaction, **including ΔH in kJ**. (Include sign)
b. What is the **energy (ΔH) evolved in kJ per mole of HCl**? (Include sign)
- Because the solutions are relatively dilute, we can assume their specific heats are close to that of H₂O, 4.184 J/g°C. However, **do not assume** the density of the solutions is that of water.
- The density of 1.00 M HCl is 1.20 g/mL and 1.00 M NaOH is 1.40 g/mL.
**Work space** Provide a thermochemical equation.
a) [Workspace for providing equation]
![10. A reaction known to release 1.78 kJ of heat takes place in a calorimeter containing 0.100 L of solution and the temperature rose by 3.65°C. *The calorimeter was then rinsed out and emptied.* To the empty calorimeter was placed a small piece of calcium carbonate and 0.100 L of dilute HCl was poured over it (in the same calorimeter). The temperature of the calorimeter then rose by 3.57°C. What is the **heat, q**, in kJ released by the reaction? *Remember to include the correct sign in your answer.*
**Show your work/calculations:**
[ *Must include a sign* ]
[ ]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6c1acf50-412f-4982-8252-15b8622c1b87%2F1c6b0c9c-10c0-48ed-8618-311076e7e024%2Fx92ngf8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:10. A reaction known to release 1.78 kJ of heat takes place in a calorimeter containing 0.100 L of solution and the temperature rose by 3.65°C. *The calorimeter was then rinsed out and emptied.* To the empty calorimeter was placed a small piece of calcium carbonate and 0.100 L of dilute HCl was poured over it (in the same calorimeter). The temperature of the calorimeter then rose by 3.57°C. What is the **heat, q**, in kJ released by the reaction? *Remember to include the correct sign in your answer.*
**Show your work/calculations:**
[ *Must include a sign* ]
[ ]
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