1. The metabolism of one mole of glycerol trioleate, C5 H93O6, a common fat, produces 3.022 x 10*kJ of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°C?
1. The metabolism of one mole of glycerol trioleate, C5 H93O6, a common fat, produces 3.022 x 10*kJ of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°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: Metabolism of Glycerol Trioleate**
The metabolism of one mole of glycerol trioleate, \( \text{C}_{51}\text{H}_{93}\text{O}_{6} \), a common fat, produces \( 3.022 \times 10^4 \, \text{kJ} \) of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°C?
---
This problem involves calculating the amount of fatty substance required to provide enough energy to raise a specific amount of water by 5°C. This involves using the heat capacity formula to determine the energy needed for the temperature change and then use the metabolic energy of the fat to find out the mass required.
**The Key Concepts:**
1. **Heat Capacity of Water:**
- For water, the specific heat capacity (\( c \)) is \( 4.18 \, \text{J/g}^\circ\text{C} \).
2. **Energy Calculation:**
- The amount of energy (\( Q \)) required to raise the temperature can be calculated with:
\[ Q = mc\Delta T \]
where \( m \) is the mass of the water, \( c \) is its specific heat capacity, and \( \Delta T \) is the temperature change.
3. **Metabolic Energy of Glycerol Trioleate:**
- The metabolism of one mole of this fat releases \( 3.022 \times 10^4 \, \text{kJ} \), which can be converted to Joules if necessary (1 kJ = 1000 J).
**Solution Steps:**
1. Calculate \( Q \) using the formula for the 50 g water temperature increase.
2. Determine how much fat is required using the energy released per mole of glycerol trioleate.
This analysis can help understand thermodynamics and energy transfer in biological systems.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7da24128-1448-42e8-87d5-1a5f72065541%2F5cfbae4d-5a48-4dfa-80e9-1b79f8cdbf86%2Fozexiy_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem: Metabolism of Glycerol Trioleate**
The metabolism of one mole of glycerol trioleate, \( \text{C}_{51}\text{H}_{93}\text{O}_{6} \), a common fat, produces \( 3.022 \times 10^4 \, \text{kJ} \) of heat. How many grams of the fat must be burned to raise the temperature of 50 g of water from 25.0°C to 30.0°C?
---
This problem involves calculating the amount of fatty substance required to provide enough energy to raise a specific amount of water by 5°C. This involves using the heat capacity formula to determine the energy needed for the temperature change and then use the metabolic energy of the fat to find out the mass required.
**The Key Concepts:**
1. **Heat Capacity of Water:**
- For water, the specific heat capacity (\( c \)) is \( 4.18 \, \text{J/g}^\circ\text{C} \).
2. **Energy Calculation:**
- The amount of energy (\( Q \)) required to raise the temperature can be calculated with:
\[ Q = mc\Delta T \]
where \( m \) is the mass of the water, \( c \) is its specific heat capacity, and \( \Delta T \) is the temperature change.
3. **Metabolic Energy of Glycerol Trioleate:**
- The metabolism of one mole of this fat releases \( 3.022 \times 10^4 \, \text{kJ} \), which can be converted to Joules if necessary (1 kJ = 1000 J).
**Solution Steps:**
1. Calculate \( Q \) using the formula for the 50 g water temperature increase.
2. Determine how much fat is required using the energy released per mole of glycerol trioleate.
This analysis can help understand thermodynamics and energy transfer in biological systems.
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 now
This is a popular solution!
Step by step
Solved 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.Recommended textbooks for you
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
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