6. Calculate the heat released by each reaction (gained by the thermometer/surroundings), qthermometers by using the following formula (use the mass 0 of the total solution) (3 pts): 9thermometer = msolution CPwater Atwater (Cp = 4.18 J/g°C) 7. Find the heat lost by the reaction (qrxn = -qthermometer). Record answers in Table 2. Explain why this is true. (2 pts) 8. Calculate moles of NaOH used in each reaction. [HINT: In Reactions 1 and 2, this can be found from the mass of the NaOH. In Reaction 3, it can be found using the molarity, M, of the NaOH and its volume, in L] (4 pts) 9. Calculate enthalpy (AH): AH=qxn/mol NaOH in each of the three reactions. (1 pt) 10. Mathematically and experimentally verify Hess's Law and explain how you came to this conclusion. Be sure to show how reaction 1 and 2 sum up to rxn 3. Compare the experimental AH of reaction 3 to the mathematical AH of rxn 3. Table 1: Raw (measured) Data 1. Mass of solid NaOH 2. Mass (total) of solution 3. Final Reaction 1 Reaction 2 2.2 2.05 g Reaction 3 (no solid NaOH mass) 101.47100.84, 99.98 g temperature, t₂ 28.9 °C 28.9 °C 30.7 °C 4. Initial temperature, t₁ 24.7 °C 24.5 °C 24.4 °C 5. Change in temperature, At 4.2 °C 4.4 °C 6.3 °C (Work on the analysis questions and fill in this table as you go through the questions) Table 2: Calculated Data 6. Heat, thermometer 7.9rxn Reaction 1 J J Reaction 2 J J Reaction 3 J J 8. Moles of NaOH mol mol mol J/mol J/mol J/mol 9. AH
6. Calculate the heat released by each reaction (gained by the thermometer/surroundings), qthermometers by using the following formula (use the mass 0 of the total solution) (3 pts): 9thermometer = msolution CPwater Atwater (Cp = 4.18 J/g°C) 7. Find the heat lost by the reaction (qrxn = -qthermometer). Record answers in Table 2. Explain why this is true. (2 pts) 8. Calculate moles of NaOH used in each reaction. [HINT: In Reactions 1 and 2, this can be found from the mass of the NaOH. In Reaction 3, it can be found using the molarity, M, of the NaOH and its volume, in L] (4 pts) 9. Calculate enthalpy (AH): AH=qxn/mol NaOH in each of the three reactions. (1 pt) 10. Mathematically and experimentally verify Hess's Law and explain how you came to this conclusion. Be sure to show how reaction 1 and 2 sum up to rxn 3. Compare the experimental AH of reaction 3 to the mathematical AH of rxn 3. Table 1: Raw (measured) Data 1. Mass of solid NaOH 2. Mass (total) of solution 3. Final Reaction 1 Reaction 2 2.2 2.05 g Reaction 3 (no solid NaOH mass) 101.47100.84, 99.98 g temperature, t₂ 28.9 °C 28.9 °C 30.7 °C 4. Initial temperature, t₁ 24.7 °C 24.5 °C 24.4 °C 5. Change in temperature, At 4.2 °C 4.4 °C 6.3 °C (Work on the analysis questions and fill in this table as you go through the questions) Table 2: Calculated Data 6. Heat, thermometer 7.9rxn Reaction 1 J J Reaction 2 J J Reaction 3 J J 8. Moles of NaOH mol mol mol J/mol J/mol J/mol 9. AH
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter13: Solutions And Their Behavior
Section: Chapter Questions
Problem 107SCQ
Related questions
Question
Use the data table to answer those questions
![6. Calculate the heat released by each reaction (gained by the
thermometer/surroundings), qthermometers by using the following formula (use the mass
0
of the total solution) (3 pts): 9thermometer = msolution CPwater Atwater (Cp = 4.18 J/g°C)
7. Find the heat lost by the reaction (qrxn = -qthermometer). Record answers in Table 2.
Explain why this is true. (2 pts)
8. Calculate moles of NaOH used in each reaction. [HINT: In Reactions 1 and 2, this
can be found from the mass of the NaOH. In Reaction 3, it can be found using the
molarity, M, of the NaOH and its volume, in L] (4 pts)
9. Calculate enthalpy (AH): AH=qxn/mol NaOH in each of the three reactions. (1 pt)
10. Mathematically and experimentally verify Hess's Law and explain how you came
to this conclusion. Be sure to show how reaction 1 and 2 sum up to rxn 3. Compare
the experimental AH of reaction 3 to the mathematical AH of rxn 3.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca7975f0-7bad-4799-a454-dce488604bae%2Fa2293733-15cf-4eed-8e37-485962a182db%2Fxfvmrn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:6. Calculate the heat released by each reaction (gained by the
thermometer/surroundings), qthermometers by using the following formula (use the mass
0
of the total solution) (3 pts): 9thermometer = msolution CPwater Atwater (Cp = 4.18 J/g°C)
7. Find the heat lost by the reaction (qrxn = -qthermometer). Record answers in Table 2.
Explain why this is true. (2 pts)
8. Calculate moles of NaOH used in each reaction. [HINT: In Reactions 1 and 2, this
can be found from the mass of the NaOH. In Reaction 3, it can be found using the
molarity, M, of the NaOH and its volume, in L] (4 pts)
9. Calculate enthalpy (AH): AH=qxn/mol NaOH in each of the three reactions. (1 pt)
10. Mathematically and experimentally verify Hess's Law and explain how you came
to this conclusion. Be sure to show how reaction 1 and 2 sum up to rxn 3. Compare
the experimental AH of reaction 3 to the mathematical AH of rxn 3.
Transcribed Image Text:Table 1: Raw (measured) Data
1. Mass of solid
NaOH
2. Mass (total)
of solution
3. Final
Reaction 1
Reaction 2
2.2 2.05
g
Reaction 3
(no solid NaOH mass)
101.47100.84, 99.98
g
temperature, t₂
28.9
°C
28.9
°C
30.7
°C
4. Initial
temperature, t₁
24.7
°C
24.5
°C
24.4
°C
5. Change in
temperature, At
4.2
°C
4.4
°C
6.3
°C
(Work on the analysis questions and fill in this table as you go through the questions)
Table 2: Calculated Data
6. Heat, thermometer
7.9rxn
Reaction 1
J
J
Reaction 2
J
J
Reaction 3
J
J
8. Moles of NaOH
mol
mol
mol
J/mol
J/mol
J/mol
9. AH
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