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A cube of ice is taken from the freezer at -8.8°C and placed in a 104 g iron cup filled with 279 g of water. Both the water & the cup are at 23.9°C. Eventually the system reaches thermal equilibrium at 12.4°C. Determine Qcup, Qwater (for the water initially in the cup), Qice, & the mass of the ice. Qcup =

A cube of ice is taken from the freezer at -8.8°C and placed in a 104 g iron cup filled with 279 g of water. Both the water & the cup are at 23.9°C. Eventually the system reaches thermal equilibrium at 12.4°C. Determine Qcup, Qwater (for the water initially in the cup), Qice, & the mass of the ice. Qcup =

College Physics
College Physics
11th Edition
ISBN:9781305952300
Author:Raymond A. Serway, Chris Vuille
Publisher:Raymond A. Serway, Chris Vuille
Chapter1: Units, Trigonometry. And Vectors
Section: Chapter Questions
Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...
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A cube of ice is taken from the freezer at -8.8°C and placed in a 104 g iron cup filled with 279 g of water. Both the water & the cup are at 23.9°C. Eventually the system reaches thermal equilibrium at 12.4°C. Determine Qcup, Qwater (for the water initially in the cup), Qice, & the mass of the ice.
Qcup = 
Qwater = 
Qice = 
mice = 
### Educational Resource: Understanding Specific Heat and Latent Heat **Tables of Specific Heat (J/kg·K)** - **Solids:** - Aluminum: 900 - Brass: 402 - Copper: 377 - Glass: 840 - Gold: 126 - Ice: 2095 - Iron: 461 - Lead: 130 - Nickel: 502 - Silver: 239 - Styrofoam: 1131 - Zinc: 390 - **Liquids:** - Bromine: 473 - Ethyl Alcohol: 2400 - Gasoline: 2220 - Glycerin: 2430 - Mercury: 140 - Water: 4186 **Latent Heat (J/kg)** - **Substances:** - Steam ↔ Water: 2,260,000 - Ice ↔ Water: 333,000 **Problem Description** A cube of ice is taken from the freezer at **-8.8°C** and placed in a **104 g iron cup** filled with **279 g of water**. Both the water and the cup are initially at **23.9°C**. Eventually, the system reaches thermal equilibrium at **12.4°C**. **Questions to Solve:** Determine the following: - \( Q_{\text{cup}} = \) - \( Q_{\text{water}} = \) (for the water initially in the cup) - \( Q_{\text{ice}} = \) - \( m_{\text{ice}} = \) (mass of the ice) ### Explanation of Concepts: - **Specific Heat** is the amount of heat per unit mass required to raise the temperature by one degree Celsius (or Kelvin). It is crucial for calculating heat transfer in substances with known initial and final temperatures. - **Latent Heat** refers to the heat required to transform a substance from one phase to another without changing its temperature. For melting ice, the latent heat is a key factor in calculating energy transfer during phase transition. ### Solving the Problem: To solve the problem, you need to use the concepts of specific heat and latent heat to calculate the heat exchanges in the system and the mass of the ice using formulas from thermodynamics.
Transcribed Image Text:### Educational Resource: Understanding Specific Heat and Latent Heat **Tables of Specific Heat (J/kg·K)** - **Solids:** - Aluminum: 900 - Brass: 402 - Copper: 377 - Glass: 840 - Gold: 126 - Ice: 2095 - Iron: 461 - Lead: 130 - Nickel: 502 - Silver: 239 - Styrofoam: 1131 - Zinc: 390 - **Liquids:** - Bromine: 473 - Ethyl Alcohol: 2400 - Gasoline: 2220 - Glycerin: 2430 - Mercury: 140 - Water: 4186 **Latent Heat (J/kg)** - **Substances:** - Steam ↔ Water: 2,260,000 - Ice ↔ Water: 333,000 **Problem Description** A cube of ice is taken from the freezer at **-8.8°C** and placed in a **104 g iron cup** filled with **279 g of water**. Both the water and the cup are initially at **23.9°C**. Eventually, the system reaches thermal equilibrium at **12.4°C**. **Questions to Solve:** Determine the following: - \( Q_{\text{cup}} = \) - \( Q_{\text{water}} = \) (for the water initially in the cup) - \( Q_{\text{ice}} = \) - \( m_{\text{ice}} = \) (mass of the ice) ### Explanation of Concepts: - **Specific Heat** is the amount of heat per unit mass required to raise the temperature by one degree Celsius (or Kelvin). It is crucial for calculating heat transfer in substances with known initial and final temperatures. - **Latent Heat** refers to the heat required to transform a substance from one phase to another without changing its temperature. For melting ice, the latent heat is a key factor in calculating energy transfer during phase transition. ### Solving the Problem: To solve the problem, you need to use the concepts of specific heat and latent heat to calculate the heat exchanges in the system and the mass of the ice using formulas from thermodynamics.
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