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In an experiment to determine the relationship between the temperature change of water and the amount of heat absorbed by the water, an electrical heater was used to increase the temperature of 1.000 g of H2O by 1.000 °C. The energy required was 4.184 J. 6. How much heat was required to increase the temperature of 1.000 g of H;0 by 1.000 °C? 7. How much heat would be required to increase the temperature of 100.0 g of H;O by 1.000 °C? 8. How much heat would be required to increase the temperature of 1.000 g of H;O by 50.00 °C? 9. The specific heat capacity of a substance is defined as the amount of energy needed to increase the temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include units of J/g°C. 10. What is the equation that relates the amount of heat absorbed or released by any substance to the change in temperature of that substance? Write this equation using the following notation: q = heat, m = mass, AT = change in temperature, and Cs = specific heat capacity. 11. In preparing dinner, you need a cup of very hot water, which you prepare on your electric stove. You use 80 kJ of electrical energy to heat 250 g of H;O starting at 20 °C. What is the final temperature of the water? 12. An unknown piece of metal weighing 100.0 g is heated to 90.0 °C. It is dropped into 250.0 g of H;0 at 20.0 °C. The final temperature of the system was found to be 29.0 °C. Determine the specific heat of the metal using the fact that the heat lost by the metal must equal the heat absorbed by the water.

In an experiment to determine the relationship between the temperature change of water and the amount of heat absorbed by the water, an electrical heater was used to increase the temperature of 1.000 g of H2O by 1.000 °C. The energy required was 4.184 J. 6. How much heat was required to increase the temperature of 1.000 g of H;0 by 1.000 °C? 7. How much heat would be required to increase the temperature of 100.0 g of H;O by 1.000 °C? 8. How much heat would be required to increase the temperature of 1.000 g of H;O by 50.00 °C? 9. The specific heat capacity of a substance is defined as the amount of energy needed to increase the temperature of 1.000 g of the substance by 1.000 °C. What is the specific heat of water? Be sure to include units of J/g°C. 10. What is the equation that relates the amount of heat absorbed or released by any substance to the change in temperature of that substance? Write this equation using the following notation: q = heat, m = mass, AT = change in temperature, and Cs = specific heat capacity. 11. In preparing dinner, you need a cup of very hot water, which you prepare on your electric stove. You use 80 kJ of electrical energy to heat 250 g of H;O starting at 20 °C. What is the final temperature of the water? 12. An unknown piece of metal weighing 100.0 g is heated to 90.0 °C. It is dropped into 250.0 g of H;0 at 20.0 °C. The final temperature of the system was found to be 29.0 °C. Determine the specific heat of the metal using the fact that the heat lost by the metal must equal the heat absorbed by the water.

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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### Experiment: Understanding Heat Transfer In an experiment to determine the relationship between temperature change in water and the amount of heat absorbed, an electrical heater was used to increase the temperature of 1.000 g of H₂O by 1.000°C. The energy required was 4.184 J. --- **Key Questions and Calculations** **6. How much heat was required to increase the temperature of 1.000 g of H₂O by 1.000°C?** - The heat required is 4.184 J, based on the experimental setup. **7. How much heat would be required to increase the temperature of 100.0 g of H₂O by 1.000°C?** - Calculation involves scaling up the heat required for 1.000 g. Therefore, \( 100.0 \, \text{g} \times 4.184 \, \text{J/g} = 418.4 \, \text{J} \). **8. How much heat would be required to increase the temperature of 1.000 g of H₂O by 50.0°C?** - Calculation involves scaling up the temperature change. Therefore, \( 50.0 \, \text{°C} \times 4.184 \, \text{J} = 209.2 \, \text{J} \). --- **9. Specific Heat Capacity** - Defined as the energy needed to increase 1.000 g of a substance by 1.000°C. Specific heat of water is 4.184 J/g°C. **10. Heat Transfer Equation** - The formula relating heat absorbed/released to temperature change is: \( q = m \cdot \Delta T \cdot C_s \), where \( q \) is heat, \( m \) is mass, \( \Delta T \) is temperature change, \( C_s \) is specific heat capacity. --- **Energy Use in Everyday Life** **11. Heating Water for Dinner** - To heat 250 g of H₂O from 20°C using 80 kJ of electrical energy, find the final temperature. The formula \( q = m \cdot \Delta T \cdot C_s \) can solve for \( \Delta T \). --- **12. Determining Specific Heat of Metal** - An unknown metal weighing 100.0 g is heated to
Transcribed Image Text:### Experiment: Understanding Heat Transfer In an experiment to determine the relationship between temperature change in water and the amount of heat absorbed, an electrical heater was used to increase the temperature of 1.000 g of H₂O by 1.000°C. The energy required was 4.184 J. --- **Key Questions and Calculations** **6. How much heat was required to increase the temperature of 1.000 g of H₂O by 1.000°C?** - The heat required is 4.184 J, based on the experimental setup. **7. How much heat would be required to increase the temperature of 100.0 g of H₂O by 1.000°C?** - Calculation involves scaling up the heat required for 1.000 g. Therefore, \( 100.0 \, \text{g} \times 4.184 \, \text{J/g} = 418.4 \, \text{J} \). **8. How much heat would be required to increase the temperature of 1.000 g of H₂O by 50.0°C?** - Calculation involves scaling up the temperature change. Therefore, \( 50.0 \, \text{°C} \times 4.184 \, \text{J} = 209.2 \, \text{J} \). --- **9. Specific Heat Capacity** - Defined as the energy needed to increase 1.000 g of a substance by 1.000°C. Specific heat of water is 4.184 J/g°C. **10. Heat Transfer Equation** - The formula relating heat absorbed/released to temperature change is: \( q = m \cdot \Delta T \cdot C_s \), where \( q \) is heat, \( m \) is mass, \( \Delta T \) is temperature change, \( C_s \) is specific heat capacity. --- **Energy Use in Everyday Life** **11. Heating Water for Dinner** - To heat 250 g of H₂O from 20°C using 80 kJ of electrical energy, find the final temperature. The formula \( q = m \cdot \Delta T \cdot C_s \) can solve for \( \Delta T \). --- **12. Determining Specific Heat of Metal** - An unknown metal weighing 100.0 g is heated to
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