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Specific heat (J/kg-K) Solids Aluminum. 900 Brass 402 Copper Glass Gold Ice Iron Lead Nickel 377 840 126 2095 461 130 502 Silver 239 Styrofoam 1131 Zinc 390 Liquids Bromine Ethyl Alcohol Gasoline Glycerin Mercury Water Substance Steam Specific heat (J/kg-K) 473 2400 2220 2430 140 4186 Latent Heat (J/kg) 2,260,000 water Icewater 333,000 A cube of ice is taken from the freezer at -9.2°C and placed in a 106 g glass cup filled with 289 g of water. Both the water & the cup are at 20.9°C. Eventually the system reaches thermal equilibrium at 5.1°C. Determine Qcup Qwater (for the water initially in the cup), Qicer & the mass of the ice. Qcup = 1,406.832 J Qwater 19,086.716 J Qice 20,520.94 J Mice = 54.92 g

Specific heat (J/kg-K) Solids Aluminum. 900 Brass 402 Copper Glass Gold Ice Iron Lead Nickel 377 840 126 2095 461 130 502 Silver 239 Styrofoam 1131 Zinc 390 Liquids Bromine Ethyl Alcohol Gasoline Glycerin Mercury Water Substance Steam Specific heat (J/kg-K) 473 2400 2220 2430 140 4186 Latent Heat (J/kg) 2,260,000 water Icewater 333,000 A cube of ice is taken from the freezer at -9.2°C and placed in a 106 g glass cup filled with 289 g of water. Both the water & the cup are at 20.9°C. Eventually the system reaches thermal equilibrium at 5.1°C. Determine Qcup Qwater (for the water initially in the cup), Qicer & the mass of the ice. Qcup = 1,406.832 J Qwater 19,086.716 J Qice 20,520.94 J Mice = 54.92 g

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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### Specific Heat Capacities of Various Substances #### Solids | Substance | Specific Heat (J/kg·K) | |------------|------------------------| | Aluminum | 900 | | Brass | 402 | | Copper | 385 | | Glass | 840 | | Gold | 126 | | Ice | 2095 | | Iron | 461 | | Lead | 130 | | Nickel | 502 | | Silver | 239 | | Styrofoam | 1131 | | Zinc | 390 | #### Liquids | Substance | Specific Heat (J/kg·K) | |----------------|------------------------| | Bromine | 473 | | Ethyl Alcohol | 2400 | | Gasoline | 2220 | | Glycerin | 2430 | | Mercury | 140 | | Water | 4186 | #### Latent Heat of Fusion/Vaporization | Substance | Latent Heat (J/kg) | |------------------|---------------------| | Steam ⇔ water | 2,260,000 | | Ice ⇔ water | 333,000 | ### Example Problem: Ice Melting in Water A cube of ice is taken from the freezer at -9.2°C and is placed in a 106 g glass cup filled with 289 g of water. Both the water and the cup are at 20.9°C. Eventually, the system reaches thermal equilibrium at 5.1°C. Determine the heat exchange between the components and compute the mass of the ice. Given data: - \( Q_{cup} = -1,406.832 \, J \) (Incorrect) - \( Q_{water} = 19,086.716 \, J \) (Incorrect) - \( Q_{ice} = 20,520.94 \, J \) (Correct) - \( m_{ice} = 54.92 \, g \) (Correct) #### Explanation of Heat Computations 1. **Heat Transfer for the Ice ($Q_{ice}$):** The heat absorbed by the ice to melt it and bring the resultant water to thermal equilibrium is calculated correctly as 20,520.94 J. 2. **Heat
Transcribed Image Text:### Specific Heat Capacities of Various Substances #### Solids | Substance | Specific Heat (J/kg·K) | |------------|------------------------| | Aluminum | 900 | | Brass | 402 | | Copper | 385 | | Glass | 840 | | Gold | 126 | | Ice | 2095 | | Iron | 461 | | Lead | 130 | | Nickel | 502 | | Silver | 239 | | Styrofoam | 1131 | | Zinc | 390 | #### Liquids | Substance | Specific Heat (J/kg·K) | |----------------|------------------------| | Bromine | 473 | | Ethyl Alcohol | 2400 | | Gasoline | 2220 | | Glycerin | 2430 | | Mercury | 140 | | Water | 4186 | #### Latent Heat of Fusion/Vaporization | Substance | Latent Heat (J/kg) | |------------------|---------------------| | Steam ⇔ water | 2,260,000 | | Ice ⇔ water | 333,000 | ### Example Problem: Ice Melting in Water A cube of ice is taken from the freezer at -9.2°C and is placed in a 106 g glass cup filled with 289 g of water. Both the water and the cup are at 20.9°C. Eventually, the system reaches thermal equilibrium at 5.1°C. Determine the heat exchange between the components and compute the mass of the ice. Given data: - \( Q_{cup} = -1,406.832 \, J \) (Incorrect) - \( Q_{water} = 19,086.716 \, J \) (Incorrect) - \( Q_{ice} = 20,520.94 \, J \) (Correct) - \( m_{ice} = 54.92 \, g \) (Correct) #### Explanation of Heat Computations 1. **Heat Transfer for the Ice ($Q_{ice}$):** The heat absorbed by the ice to melt it and bring the resultant water to thermal equilibrium is calculated correctly as 20,520.94 J. 2. **Heat
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