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How much heat in kilojoules is evolved in converting 1.00 mol of steam at 145 °C to ice

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 95P Chapter 12

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 95P

How much heat in kilojoules is evolved in converting 1.00 mol of steam at \(145^{\circ} \mathrm{C}\) to ice at \(-50.0^{\circ} \mathrm{C}\)? The heat capacity of steam is \(1.84 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\) and that of ice is \(2.09 \mathrm{~J} / \mathrm{g}^{\circ} \mathrm{C}\).

Equation Transcription:

Text Transcription:

145 degrees C

-50.0 degrees C

1.84 J/g degrees C

2.09 J/g degrees C

Step-by-Step Solution:

Solution 95P

Step 1:

Converting 1.00 mol of steam at 145 °C to ice at -50.0 °C involves the loss of

57.71 kJ of energy.

There are five heats to consider:

q1 = heat lost on cooling steam from 145 °C to 100 °C.

q2 = heat lost on condensing steam to water at 100 °C.

q3 = heat lost on cooling water from 100 °C to 0°C.

q4 = heat lost on freezing water to ice at 0 °C.

q5 = heat lost on cooling ice from 0 °C to -50.0 °.

The total heat evolved is

q=q1+q2+q3+q4+q5

Step 2 of 2

Chapter 12, Problem 95P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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