If a piece of aluminum with a mass of 2.39g and a temperature of 100.0°C is dropped into 10.0cm³ of water at 14.1°C, what will be the final temperature of the system? (Use 1.00g/cm³as the density of water.) Cp Al = 0.900J/g °C
If a piece of aluminum with a mass of 2.39g and a temperature of 100.0°C is dropped into 10.0cm³ of water at 14.1°C, what will be the final temperature of the system? (Use 1.00g/cm³as the density of water.) Cp Al = 0.900J/g °C
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...
Related questions
Question
![**Problem Statement:**
If a piece of aluminum with a mass of 2.39g and a temperature of 100.0°C is dropped into 10.0cm³ of water at 14.1°C, what will be the final temperature of the system?
*(Use 1.00g/cm³ as the density of water, Cₚ Al = 0.900 J/g°C)*
---
**Explanation of the Problem:**
- We are tasked with finding the final temperature when a hot piece of aluminum is placed in cooler water.
- The aluminum has a known specific heat capacity, mass, and initial temperature.
- The water has a known volume, which will be converted to mass using the given density.
- A heat exchange will occur, aiming for thermal equilibrium, meaning the same final temperature for both substances.
**Note:** The problem requires the use of the principle of conservation of energy, where the heat lost by aluminum will equal the heat gained by the water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fda32a2fc-08e4-44f0-a5cc-b9514bad5aff%2F4b2daa36-fe9c-4d86-909a-c6628ee5b138%2Ffatyo7g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
If a piece of aluminum with a mass of 2.39g and a temperature of 100.0°C is dropped into 10.0cm³ of water at 14.1°C, what will be the final temperature of the system?
*(Use 1.00g/cm³ as the density of water, Cₚ Al = 0.900 J/g°C)*
---
**Explanation of the Problem:**
- We are tasked with finding the final temperature when a hot piece of aluminum is placed in cooler water.
- The aluminum has a known specific heat capacity, mass, and initial temperature.
- The water has a known volume, which will be converted to mass using the given density.
- A heat exchange will occur, aiming for thermal equilibrium, meaning the same final temperature for both substances.
**Note:** The problem requires the use of the principle of conservation of energy, where the heat lost by aluminum will equal the heat gained by the water.
![If a piece of cadmium (Cd) with a mass of 75.2 g and a temperature of 100.0°C is dropped into 25.0 g of water at 23.0°C, what will be the final temperature of the system?
Cₚ Cd = 0.230 J/g°C](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fda32a2fc-08e4-44f0-a5cc-b9514bad5aff%2F4b2daa36-fe9c-4d86-909a-c6628ee5b138%2Fuol947o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:If a piece of cadmium (Cd) with a mass of 75.2 g and a temperature of 100.0°C is dropped into 25.0 g of water at 23.0°C, what will be the final temperature of the system?
Cₚ Cd = 0.230 J/g°C
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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.Recommended textbooks for you
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY