2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C. Is this dissolution reaction exothermic? a. Why? b. Calculate 9H,0, using Equation 1. joules с. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). ΔΗ- joules
2. When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C. Is this dissolution reaction exothermic? a. Why? b. Calculate 9H,0, using Equation 1. joules с. Find AH for the reaction as it occurred in the calorimeter (Eq. 5). ΔΗ- joules
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 64PS: The enthalpy change for the oxidation of styrene. C8H8, is measured by calorimetry. C8H8() + 10...
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Heat Effects and Calorimetry
Transcribed Image Text:**Question 2**
When 4.98 g of NaOH was dissolved in 49.72 g of water in a calorimeter at 23.7°C, the temperature of the solution went up to 50.1°C.
a. Is this dissolution reaction exothermic? ______________ Why?
b. Calculate \( q_{\text{H}_2\text{O}} \) using Equation 1.
______________ joules
c. Find \( \Delta H \) for the reaction as it occurred in the calorimeter (Eq. 5).
\(\Delta H =\) ______________ joules
![### Educational Task
**Problem Statement:**
d. Find \(\Delta H\) for the dissolution of 1.00 g NaOH in water.
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/g}
\]
e. Find \(\Delta H\) for the dissolution of 1 mole NaOH in water.
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/mol}
\]
f. Given that NaOH exists as \( \text{Na}^+ \) and \( \text{OH}^- \) ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water.
g. Given the following heats of formation, \(\Delta H_f\), in kJ per mole, as obtained from a table of \(\Delta H_f\) data, calculate \(\Delta H\) for the reaction in Part (f). Compare your answer with the result you obtained in Part (e).
- NaOH(s), \(-425.6\)
- \( \text{Na}^+ (aq), \)
- \(-240.1\)
- \( \text{OH}^- (aq), \)
- \(-230.0\)
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/mol}
\]
### Explanation of Tasks:
1. **Calculation of \(\Delta H\) (d and e):** Determine the enthalpy change for both 1 gram and 1 mole of NaOH when dissolved in water.
2. **Ionization Equation (f):** Write the chemical equation representing the dissolution of NaOH into its constituent ions in an aqueous solution.
3. **Thermodynamic Calculation (g):** Utilize given standard heats of formation to calculate the enthalpy change for the solution process, and compare this calculated value with the result from part (e).
This exercise involves concepts related to thermodynamics, chemical reactions, and stoichiometry, essential for understanding chemical energetics.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd62a91b5-60c5-4a97-9022-e43a55d1b398%2Fa369f7e7-cfef-4b73-bd0c-0455ca0f64ec%2F2gj1f8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Educational Task
**Problem Statement:**
d. Find \(\Delta H\) for the dissolution of 1.00 g NaOH in water.
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/g}
\]
e. Find \(\Delta H\) for the dissolution of 1 mole NaOH in water.
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/mol}
\]
f. Given that NaOH exists as \( \text{Na}^+ \) and \( \text{OH}^- \) ions in solution, write the equation for the reaction that occurs when NaOH is dissolved in water.
g. Given the following heats of formation, \(\Delta H_f\), in kJ per mole, as obtained from a table of \(\Delta H_f\) data, calculate \(\Delta H\) for the reaction in Part (f). Compare your answer with the result you obtained in Part (e).
- NaOH(s), \(-425.6\)
- \( \text{Na}^+ (aq), \)
- \(-240.1\)
- \( \text{OH}^- (aq), \)
- \(-230.0\)
\[
\Delta H = \_\_\_\_\_\_\_\_\_\_ \text{ kJ/mol}
\]
### Explanation of Tasks:
1. **Calculation of \(\Delta H\) (d and e):** Determine the enthalpy change for both 1 gram and 1 mole of NaOH when dissolved in water.
2. **Ionization Equation (f):** Write the chemical equation representing the dissolution of NaOH into its constituent ions in an aqueous solution.
3. **Thermodynamic Calculation (g):** Utilize given standard heats of formation to calculate the enthalpy change for the solution process, and compare this calculated value with the result from part (e).
This exercise involves concepts related to thermodynamics, chemical reactions, and stoichiometry, essential for understanding chemical energetics.
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