9-2. Consider this thermochem ical equation: 4 PCl() → Pa(s) + 6 Ch(g) AH° = +1278.8 kJ If the chlorine gas is collected at STP, then what volume of chlorine is produced when 68 joules are absorbed in the reaction?
9-2. Consider this thermochem ical equation: 4 PCl() → Pa(s) + 6 Ch(g) AH° = +1278.8 kJ If the chlorine gas is collected at STP, then what volume of chlorine is produced when 68 joules are absorbed in the reaction?
Chemistry
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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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![**Thermochemical Equation Analysis**
**Question 9-2:**
Consider the following thermochemical equation:
\[ 4 \, \text{PCl}_3(l) \rightarrow \text{P}_4(s) + 6 \, \text{Cl}_2(g) \]
\[ \Delta H^\circ = +1278.8 \, \text{kJ} \]
**Problem Statement:**
If the chlorine gas is collected at Standard Temperature and Pressure (STP), determine the volume of chlorine gas produced when 68 joules are absorbed in the reaction.
**Explanation:**
This is a thermochemical equation describing the reaction where liquid phosphorus trichloride (\(\text{PCl}_3\)) is converted into solid phosphorus (\(\text{P}_4\)) and gaseous chlorine (\(\text{Cl}_2\)). The enthalpy change (\(\Delta H^\circ\)) for this reaction is \(+1278.8 \, \text{kJ}\), indicating that the reaction absorbs energy.
**Objective:**
To find out how much chlorine gas (\(\text{Cl}_2\)) is generated when 68 joules of energy are absorbed at STP conditions.
**Approach:**
- Use the given enthalpy change to determine the proportion of chlorine gas produced with 68 joules of absorbed energy.
- Apply gas laws to calculate the volume of gas produced under STP conditions, knowing that one mole of gas occupies 22.4 liters at STP.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdf619e63-1a49-4777-acbc-e2486c509c25%2Fff5b1894-aea2-4dbc-81e9-7e1447fa6b03%2Fsbebp0w_processed.png&w=3840&q=75)
Transcribed Image Text:**Thermochemical Equation Analysis**
**Question 9-2:**
Consider the following thermochemical equation:
\[ 4 \, \text{PCl}_3(l) \rightarrow \text{P}_4(s) + 6 \, \text{Cl}_2(g) \]
\[ \Delta H^\circ = +1278.8 \, \text{kJ} \]
**Problem Statement:**
If the chlorine gas is collected at Standard Temperature and Pressure (STP), determine the volume of chlorine gas produced when 68 joules are absorbed in the reaction.
**Explanation:**
This is a thermochemical equation describing the reaction where liquid phosphorus trichloride (\(\text{PCl}_3\)) is converted into solid phosphorus (\(\text{P}_4\)) and gaseous chlorine (\(\text{Cl}_2\)). The enthalpy change (\(\Delta H^\circ\)) for this reaction is \(+1278.8 \, \text{kJ}\), indicating that the reaction absorbs energy.
**Objective:**
To find out how much chlorine gas (\(\text{Cl}_2\)) is generated when 68 joules of energy are absorbed at STP conditions.
**Approach:**
- Use the given enthalpy change to determine the proportion of chlorine gas produced with 68 joules of absorbed energy.
- Apply gas laws to calculate the volume of gas produced under STP conditions, knowing that one mole of gas occupies 22.4 liters at STP.
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