10. A reaction at 45 °C has the following enthalpy and entropy: AH° = -86.6 kJ and AS = 382J/K. a. Calculate AG gros fess b. Is the reaction spontaneous at this temperature? 11. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put into 100.0 g of water at 23.7 °C. The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. 12. A 237 g sample of molybdenum metal is heated to 100.1 °C and then dropped into an insulated cup containing 244 g of water at 10.0 °C. If the final temperature of the water and metal in the cup is 15.3 °C, then what is the specific heat of molybdenum?
10. A reaction at 45 °C has the following enthalpy and entropy: AH° = -86.6 kJ and AS = 382J/K. a. Calculate AG gros fess b. Is the reaction spontaneous at this temperature? 11. A piece of metal weighing 59.047 g was heated to 100.0 °C and then put into 100.0 g of water at 23.7 °C. The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat of the metal. 12. A 237 g sample of molybdenum metal is heated to 100.1 °C and then dropped into an insulated cup containing 244 g of water at 10.0 °C. If the final temperature of the water and metal in the cup is 15.3 °C, then what is the specific heat of molybdenum?
Chemistry: An Atoms First Approach
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ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
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Chapter7: Chemical Energy
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Problem 55E: A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of...
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Hi sorry to bother I know that you guys can only answer 3 questions per the ask questions so I was wondering if you could solve the following 3 for me please thank you
![### Thermodynamics and Calorimetry Problems
#### 10. A reaction at 45°C has the following enthalpy and entropy:
- ΔH° = -86.6 kJ
- ΔS° = 392 J/K
**a. Calculate ΔG°**
**b. Is the reaction spontaneous at this temperature?**
#### 11. Specific Heat Calculation
A piece of metal weighing 50.947 g was heated to 100.0°C and then put into 100.0 g of water at 23.7°C. The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat is lost to the environment, calculate the specific heat of the metal.
#### 12. Specific Heat of Molybdenum
A 23.7g sample of molybdenum metal is heated to 100.1°C and then dropped into an insulated cup containing 244 g of water at 10.0°C. If the final temperature of the water and metal in the cup is 15.3°C, then what is the specific heat of molybdenum?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c430cc2-4097-4d45-9871-f052d1dcc428%2F4be8e67f-bf80-43e8-8dd1-6ab1103835cd%2Fmnoqwqb_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Thermodynamics and Calorimetry Problems
#### 10. A reaction at 45°C has the following enthalpy and entropy:
- ΔH° = -86.6 kJ
- ΔS° = 392 J/K
**a. Calculate ΔG°**
**b. Is the reaction spontaneous at this temperature?**
#### 11. Specific Heat Calculation
A piece of metal weighing 50.947 g was heated to 100.0°C and then put into 100.0 g of water at 23.7°C. The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8°C. Assuming no heat is lost to the environment, calculate the specific heat of the metal.
#### 12. Specific Heat of Molybdenum
A 23.7g sample of molybdenum metal is heated to 100.1°C and then dropped into an insulated cup containing 244 g of water at 10.0°C. If the final temperature of the water and metal in the cup is 15.3°C, then what is the specific heat of molybdenum?
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