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Burning 1.09 g of a fuel causes the water in a calorimeter to increase by 14.7°C.If the calorimeter has a heat capacity of

Burning 1.09 g of a fuel causes the water in a calorimeter to increase by 14.7°C.If the calorimeter has a heat capacity of

Chemistry
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:** Burning 1.09 g of a fuel causes the water in a calorimeter to increase by 14.7°C. If the calorimeter has a heat capacity of 3.09 kJ/°C, what is the energy density of the fuel (in kJ/g)? **Input Section:** Type answer: [Text Box] **Submit Button:** CHECK **Explanation:** This text is part of an exercise where students need to calculate the energy density of a fuel based on the heat energy transferred to a calorimeter. Students have to use the formula for energy transfer: \[ \text{Energy} = \text{Heat Capacity} \times \Delta T \] \[ \text{Energy Density} = \frac{\text{Energy}}{\text{Mass of Fuel}} \] Given: - Mass of fuel = 1.09 g - Temperature increase (\(\Delta T\)) = 14.7°C - Heat capacity = 3.09 kJ/°C Students need to find the energy density in kJ/g by first calculating the total energy absorbed by the calorimeter and then dividing it by the mass of the fuel burned.
Transcribed Image Text:**Problem Statement:** Burning 1.09 g of a fuel causes the water in a calorimeter to increase by 14.7°C. If the calorimeter has a heat capacity of 3.09 kJ/°C, what is the energy density of the fuel (in kJ/g)? **Input Section:** Type answer: [Text Box] **Submit Button:** CHECK **Explanation:** This text is part of an exercise where students need to calculate the energy density of a fuel based on the heat energy transferred to a calorimeter. Students have to use the formula for energy transfer: \[ \text{Energy} = \text{Heat Capacity} \times \Delta T \] \[ \text{Energy Density} = \frac{\text{Energy}}{\text{Mass of Fuel}} \] Given: - Mass of fuel = 1.09 g - Temperature increase (\(\Delta T\)) = 14.7°C - Heat capacity = 3.09 kJ/°C Students need to find the energy density in kJ/g by first calculating the total energy absorbed by the calorimeter and then dividing it by the mass of the fuel burned.
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