QUESTIONS If 20.0 Cal make an ounce, how many ounces of formula should a baby drink per day if the energy need per day is 1.50 x 10³ Cal? Express answer to the correct number of significant figures. 75.0 x 10E3 QUESTION 3 A 9.86 g sample of iron metal was heated in water to 85°C. Then, it was dropped into a beaker containing 240.0 g of H₂O at 28.5°C. Assuming that the water gained all the heat lost by the iron, what is the final temperature of the H₂O and Fe? QUESTION 4 If 756 cal of heat were added to 64.8 g of Al at 32.5 °C, what is the final temperature of the aluminum?

Chemistry
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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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**Educational Website Content: Thermodynamics Problems**

**QUESTION 1**

*Context: Energy Conversion Problem*

If 20.0 Cal make an ounce, how many ounces of formula should a baby drink per day if the energy need per day is 1.50 x 10³ Cal? Express the answer to the correct number of significant figures.

**Answer Box**: [75.0 x 10²]

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**QUESTION 3**

*Context: Heat Transfer and Equilibrium Temperature Problem*

A 9.86 g sample of iron metal was heated in water to 85°C. Then, it was dropped into a beaker containing 240.0 g of H₂O at 28.5°C. Assuming that the water gained all the heat lost by the iron, what is the final temperature of the H₂O and Fe?

**Answer Box**: [                       ]

---

**QUESTION 4**

*Context: Heat Addition and Temperature Change Problem*

If 756 cal of heat were added to 64.8 g of Al at 32.5°C, what is the final temperature of the aluminum?

**Answer Box**: [                       ]

---

*Note: For these problems, apply the principles of thermodynamics, specifically the concepts of heat transfer, to solve for unknown variables such as final temperature or mass. Consider using equations like \( q = mc\Delta T \) where \( q \) is the heat added or removed, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.*
Transcribed Image Text:**Educational Website Content: Thermodynamics Problems** **QUESTION 1** *Context: Energy Conversion Problem* If 20.0 Cal make an ounce, how many ounces of formula should a baby drink per day if the energy need per day is 1.50 x 10³ Cal? Express the answer to the correct number of significant figures. **Answer Box**: [75.0 x 10²] --- **QUESTION 3** *Context: Heat Transfer and Equilibrium Temperature Problem* A 9.86 g sample of iron metal was heated in water to 85°C. Then, it was dropped into a beaker containing 240.0 g of H₂O at 28.5°C. Assuming that the water gained all the heat lost by the iron, what is the final temperature of the H₂O and Fe? **Answer Box**: [ ] --- **QUESTION 4** *Context: Heat Addition and Temperature Change Problem* If 756 cal of heat were added to 64.8 g of Al at 32.5°C, what is the final temperature of the aluminum? **Answer Box**: [ ] --- *Note: For these problems, apply the principles of thermodynamics, specifically the concepts of heat transfer, to solve for unknown variables such as final temperature or mass. Consider using equations like \( q = mc\Delta T \) where \( q \) is the heat added or removed, \( m \) is the mass, \( c \) is the specific heat capacity, and \( \Delta T \) is the change in temperature.*
Expert Solution
Step 1: Relation between heat and mass

The heat gained or lost by matter is given by,q=mcTwhere,m=mass of the substancec=specific heat capacityT=change in temperature

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