What quantity of heat (in kJ) is absorbed in the process of making 0.779 mol of CF4 from the following reaction? C (s) + 2 F₂ (g) → CF₂ (g) AH° = 141.3 kJ/mol
What quantity of heat (in kJ) is absorbed in the process of making 0.779 mol of CF4 from the following reaction? C (s) + 2 F₂ (g) → CF₂ (g) AH° = 141.3 kJ/mol
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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![**Question 12 of 25**
*Objective: Calculate Heat Absorption in a Chemical Reaction*
**Question:**
What quantity of heat (in kJ) is absorbed in the process of making 0.779 mol of CF₄ from the following reaction?
\[ \text{C (s) + 2 F}_2 \text{ (g)} \rightarrow \text{CF}_4 \text{ (g)} \quad \Delta H^\circ = 141.3 \, \text{kJ/mol} \]
**Explanation:**
This question involves calculating the heat absorbed during the formation of carbon tetrafluoride (CF₄) from carbon (C) and fluorine gas (F₂) given the enthalpy change of the reaction (\( \Delta H^\circ \)). The provided standard enthalpy change of the reaction is 141.3 kJ per mole of CF₄ produced.
**Calculation:**
To find the total heat absorbed for 0.779 mol of CF₄, use the formula:
\[ \text{Heat absorbed (kJ)} = \Delta H^\circ \times \text{moles of CF}_4 \]
Substitute the values:
\[ \text{Heat absorbed} = 141.3 \, \text{kJ/mol} \times 0.779 \, \text{mol} \]
\[ \text{Heat absorbed} = 110.0447 \, \text{kJ} \]
The heat absorbed during the formation of 0.779 mol of CF₄ is approximately 110.04 kJ.
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Transcribed Image Text:**Question 12 of 25**
*Objective: Calculate Heat Absorption in a Chemical Reaction*
**Question:**
What quantity of heat (in kJ) is absorbed in the process of making 0.779 mol of CF₄ from the following reaction?
\[ \text{C (s) + 2 F}_2 \text{ (g)} \rightarrow \text{CF}_4 \text{ (g)} \quad \Delta H^\circ = 141.3 \, \text{kJ/mol} \]
**Explanation:**
This question involves calculating the heat absorbed during the formation of carbon tetrafluoride (CF₄) from carbon (C) and fluorine gas (F₂) given the enthalpy change of the reaction (\( \Delta H^\circ \)). The provided standard enthalpy change of the reaction is 141.3 kJ per mole of CF₄ produced.
**Calculation:**
To find the total heat absorbed for 0.779 mol of CF₄, use the formula:
\[ \text{Heat absorbed (kJ)} = \Delta H^\circ \times \text{moles of CF}_4 \]
Substitute the values:
\[ \text{Heat absorbed} = 141.3 \, \text{kJ/mol} \times 0.779 \, \text{mol} \]
\[ \text{Heat absorbed} = 110.0447 \, \text{kJ} \]
The heat absorbed during the formation of 0.779 mol of CF₄ is approximately 110.04 kJ.
**Interactive Component:**
There's a keypad displayed for entering numerical answers, featuring numbers (0-9), a decimal point, and other input functions.
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