Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Concept explainers
Question
![### Thermodynamics Problem
**Problem Statement:**
If a system has \(4.50 \times 10^2\) kcal of work done to it, and releases \(5.00 \times 10^2\) kJ of heat into its surroundings, what is the change in internal energy (\(\Delta E\) or \(\Delta U\)) of the system?
**Solution:**
To solve this problem, we can use the First Law of Thermodynamics, which is expressed as:
\[
\Delta E = Q - W
\]
Where:
- \(\Delta E\) is the change in internal energy.
- \(Q\) is the heat absorbed by the system.
- \(W\) is the work done on the system.
**Given:**
- Work done on the system, \(W = 4.50 \times 10^2\) kcal.
- Heat released by the system, \(Q = -5.00 \times 10^2\) kJ.
**Conversion:**
1 kcal = 4.184 kJ
Convert the work done to kJ:
\[ W = 4.50 \times 10^2 \, \text{kcal} \times 4.184 \, \text{kJ/kcal} = 1882.8 \, \text{kJ} \]
**Calculation:**
Substitute the values into the equation:
\[
\Delta E = (-5.00 \times 10^2 \, \text{kJ}) - 1882.8 \, \text{kJ}
\]
Calculate \(\Delta E\):
\[
\Delta E = -500 - 1882.8 = -2382.8 \, \text{kJ}
\]
**Conclusion:**
The change in internal energy of the system is \(-2382.8\) kJ.](https://content.bartleby.com/qna-images/question/76884ef0-0050-4a4d-a83f-5c6d84fc3fcd/d6265d82-a12c-4fbc-9044-a4b20423ea5e/dtiq8x7_processed.jpeg)
Transcribed Image Text:### Thermodynamics Problem
**Problem Statement:**
If a system has \(4.50 \times 10^2\) kcal of work done to it, and releases \(5.00 \times 10^2\) kJ of heat into its surroundings, what is the change in internal energy (\(\Delta E\) or \(\Delta U\)) of the system?
**Solution:**
To solve this problem, we can use the First Law of Thermodynamics, which is expressed as:
\[
\Delta E = Q - W
\]
Where:
- \(\Delta E\) is the change in internal energy.
- \(Q\) is the heat absorbed by the system.
- \(W\) is the work done on the system.
**Given:**
- Work done on the system, \(W = 4.50 \times 10^2\) kcal.
- Heat released by the system, \(Q = -5.00 \times 10^2\) kJ.
**Conversion:**
1 kcal = 4.184 kJ
Convert the work done to kJ:
\[ W = 4.50 \times 10^2 \, \text{kcal} \times 4.184 \, \text{kJ/kcal} = 1882.8 \, \text{kJ} \]
**Calculation:**
Substitute the values into the equation:
\[
\Delta E = (-5.00 \times 10^2 \, \text{kJ}) - 1882.8 \, \text{kJ}
\]
Calculate \(\Delta E\):
\[
\Delta E = -500 - 1882.8 = -2382.8 \, \text{kJ}
\]
**Conclusion:**
The change in internal energy of the system is \(-2382.8\) kJ.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Calculate the energy required to heat 1.80kg of ammonia from 21.5°C to 41.0°C . Assume the specific heat capacity of ammonia under these conditions is ·4.70J·g−1K−1 Round your answer to 3 significant digits.arrow_forwardA chemist carefully measures the amount of heat needed to raise the temperature of a 0.88 kg sample of C,H0, from 35.8 °C to 51.4 °C. The experiment shows that 2.34 × 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H00,? Round your answer to 2 significant digits. |J-mol 1 - 1 •K х10arrow_forwardThe combustion of 1.880 g of sucrose, C,H,,O, (s), in a bomb calorimeter with a heat capacity of 4.30 kJ/°C results in an increase in the temperature of the calorimeter and its contents from 22.31 °C to 29.52 °C. What is the internal energy change, AU, for the combustion of 1.880 g of sucrose? AU = kJ Calculate the enthalpy of combustion, AHe, of sucrose in kilojoules per mole. kJ/mol AH. = A étv w MacBook Air DI DD 80 888 F12 F11 F9 F10 F7 FB 3 F4 F5 F6arrow_forward
- The enthalpy change for the oxidation of butane, C4H₁0, is measured by calorimetry. C4H10 (g) + 13/2 O2(g) → 4 CO2 (g) +5 H₂O(l) A₂H = -2877.6 kJ/mol-rxn Use this value, along with the standard enthalpies of formation of CO2(g) and H₂O(l) (-393.509 kJ/mol and -285.83 kJ/mol respectively), to calculate the enthalpy of formation of butane, C4H10, in kJ/mol. Enthalpy of formation = Submit Answer OCT 30 Try Another Version tv kJ/mol S4 I all 9 item attempts remaining Cengage Learning | Cengage Technical Support A MacBook Pro 7 ( O 04arrow_forwardThe combustion of 1.925 g of propanol (C₂H,OH) increases the temperature of a bomb calorimeter from 298.00 K to 302.14 K. The heat capacity of the bomb calorimeter is 15.61 kJ/K. Determine AH for the combustion of propanol to carbon dioxide gas and liquid water. kJ/mol ΔΗ = TOOLS x10arrow_forwardThe combustion of toluene has a AErxn of -3.91 x 10³ kJ/mol. When 1.30 g of toluene (C7H8) undergoes combustion in a bomb calorimeter, the temperature rises from 22.80 °C to 36.11 °C. Find the heat capacity of the bomb calorimeter. Express your answer using three significant figures. Ccal = 17| ΑΣΦ ? kJ/°Carrow_forward
- Answer the questions that are attachedarrow_forwardA system does 501 kJ of work and loses 216 kJ of heat to the surroundings. What is the change in internal energy, AE, of the system? Note that internal energy is symbolized as AU in some sources. AE = kJarrow_forwardA chemist carefully measures the amount of heat needed to ralse the temperature of a 1.48 kg sample of C,H,0, from 32.9 °C to 50.0 °C. The experlment 4-8 2 shows that 4.02 x 10* J of heat are needed. What can the chemist report for the molar heat capacity of C,H,0,? Be sure your answer has the correct number of significant digits.arrow_forward
- Part A A silver block, initially at 55.8 °C, is submerged into 100.0 g of water at 24.1°C in an insulated container. The final temperature of the mixture upon reaching thermal equilibrium is 26.3 °C. The specific heat capacities for water and silver are = 4.18 J/(g ·°C) and 0.235 J/(g·°C). What is the mass of the silver block? Express your answer to two significant figures and include the appropriate units. Cs, water • View Available Hint(s) Cs, silver = HA ? Value Units m =arrow_forwardIf a system has 225 kcal of work done to it, and releases 5.00 x 102 kJ of heat into its surroundings, what is the change in internal energy (AE or AU) of the system? ΔΕ- kJarrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY