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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro
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An ice cube at 0.00 °C with a mass of 23.5 g is placed into 550.0 g of water, initially

Chapter 12, Problem 103P

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QUESTION:

An ice cube at \(0.00^{\circ} \mathrm{C}\) with a mass of 23.5 g is placed into 550.0 g of water, initially at \(28.0^{\circ} \mathrm{C}\), in an insulated container. Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all of the ice has melted?

Equation Transcription:

Text Transcription:

0.00 degrees C

28.0 degrees C

Questions & Answers

QUESTION:

An ice cube at \(0.00^{\circ} \mathrm{C}\) with a mass of 23.5 g is placed into 550.0 g of water, initially at \(28.0^{\circ} \mathrm{C}\), in an insulated container. Assuming that no heat is lost to the surroundings, what is the temperature of the entire water sample after all of the ice has melted?

Equation Transcription:

Text Transcription:

0.00 degrees C

28.0 degrees C

ANSWER:

Solution 103P

Given:

Mass of ice = 23.5g

Mass of water = 550  g

Initial temperature = 28oC

We will have to find the temperature of the entire water sample after all of the ice has melted?

Explanation: 

The specific enthalpy of fusion of water is 333.55 kJ/kg at 0 °C. = 333.55 J g-1

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