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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 12 - Problem 95p
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 12 - Problem 95p

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# How much heat in kilojoules is evolved in converting 1.00 mol of steam at 145 °C to ice ISBN: 9780321910295 34

## Solution for problem 95P Chapter 12

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

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