The specific heat of a certain type of cooking oil is 1.75 J/(g-°C). How much heat energy is needed to raise the temperature of 2.93 kg of this oil from 23 °C to 191 °C? 9 = 2.261 Incorrect
The specific heat of a certain type of cooking oil is 1.75 J/(g-°C). How much heat energy is needed to raise the temperature of 2.93 kg of this oil from 23 °C to 191 °C? 9 = 2.261 Incorrect
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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![**Problem Statement:**
The specific heat of a certain type of cooking oil is 1.75 J/(g°C). How much heat energy is needed to raise the temperature of 2.93 kg of this oil from 23°C to 191°C?
**Equation:**
q =
**Answer:**
2.261 J (Note: This answer is marked incorrect.)
**Explanation:**
To solve this problem, you need to use the formula for heat energy:
\[ q = mc\Delta T \]
Where:
- \( q \) is the heat energy (in joules)
- \( m \) is the mass (in grams)
- \( c \) is the specific heat capacity (in J/g°C)
- \( \Delta T \) is the change in temperature (in °C)
First, convert the mass from kilograms to grams:
\[ 2.93 \, \text{kg} = 2930 \, \text{g} \]
Calculate the change in temperature:
\[ \Delta T = 191°C - 23°C = 168°C \]
Now, substitute the values into the formula:
\[ q = (2930 \, \text{g})(1.75 \, \text{J/g°C})(168°C) \]
Finally, calculate \( q \) to find the correct heat energy required.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffdc195bb-9009-47db-866e-65b6514806e8%2Ffb22df7a-64d1-4494-98d7-039122e6722f%2Fpfo7te_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
The specific heat of a certain type of cooking oil is 1.75 J/(g°C). How much heat energy is needed to raise the temperature of 2.93 kg of this oil from 23°C to 191°C?
**Equation:**
q =
**Answer:**
2.261 J (Note: This answer is marked incorrect.)
**Explanation:**
To solve this problem, you need to use the formula for heat energy:
\[ q = mc\Delta T \]
Where:
- \( q \) is the heat energy (in joules)
- \( m \) is the mass (in grams)
- \( c \) is the specific heat capacity (in J/g°C)
- \( \Delta T \) is the change in temperature (in °C)
First, convert the mass from kilograms to grams:
\[ 2.93 \, \text{kg} = 2930 \, \text{g} \]
Calculate the change in temperature:
\[ \Delta T = 191°C - 23°C = 168°C \]
Now, substitute the values into the formula:
\[ q = (2930 \, \text{g})(1.75 \, \text{J/g°C})(168°C) \]
Finally, calculate \( q \) to find the correct heat energy required.
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