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A gold ball with a mass of 138 g has been heated to a temperature of 92.4°C and is then dropped into 974 g o water at an initial temperature of 19.2°C. What will the equilibrium (i.e., final) temperature of the ball and the water be? The specific heat of gold is 0.129 J/g.°C and that of water is 4.184 J/g.°C. (A) (B) (C) (D) (E) 92.1°C 55.8°C 13.1°C 18.9°C 19.5°C

A gold ball with a mass of 138 g has been heated to a temperature of 92.4°C and is then dropped into 974 g o water at an initial temperature of 19.2°C. What will the equilibrium (i.e., final) temperature of the ball and the water be? The specific heat of gold is 0.129 J/g.°C and that of water is 4.184 J/g.°C. (A) (B) (C) (D) (E) 92.1°C 55.8°C 13.1°C 18.9°C 19.5°C

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter15: Energy And Chemical Change
Section: Chapter Questions
Problem 78A: Alloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the...
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A gold ball with a mass of 138 g has been heated to a temperature of 92.4°C and is then dropped into 974 g of water at an initial temperature of 19.2°C. What will the equilibrium (i.e., final) temperature of the ball and the water be? The specific heat of gold is 0.129 J/g.°C and that of water is 4.184 J/g.°C. (A) (B) (C) (D) (E) 92.1°C 55.8°C 13.1°C 18.9°C 19.5°C
Transcribed Image Text:A gold ball with a mass of 138 g has been heated to a temperature of 92.4°C and is then dropped into 974 g of water at an initial temperature of 19.2°C. What will the equilibrium (i.e., final) temperature of the ball and the water be? The specific heat of gold is 0.129 J/g.°C and that of water is 4.184 J/g.°C. (A) (B) (C) (D) (E) 92.1°C 55.8°C 13.1°C 18.9°C 19.5°C
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