Concept explainers
Steam at 100°C is added to ice at 0°C. (a) Find the amount of ice melted and the final temperature when the mass of steam is 10.0 g and the mass of ice is 50.0 g. (b) What If? Repeat when the mass of steam is 1.00 g and the mass of ice is 50.0 g.
(a)
The amount of ice melted and final temperature when the mass of steam is
Answer to Problem 20.21P
The amount of ice melted is
Explanation of Solution
Given info: Steam at
The expression for the energy needed to melt
Here,
Substitute
Thus, the energy needed to melt
The expression for the energy needed to warm
Here,
Substitute
Thus, the energy needed to warm
The expression for the energy released by
Here,
Substitute
Thus, the energy released by
The expression for the total amount of heat required to convert
Substitute
Thus, the total amount of heat required to convert
From the above result it is clear that the amount of energy released by the steam to condense is more than the amount of energy needed to melt
So, the all the ice will melt to water.
For the final common temperature of ice-steam system:
Here,
Substitute
Conclusion:
Therefore, the amount of ice melted is
(b)
The amount of ice melted and final temperature when the mass of steam is
Answer to Problem 20.21P
The amount of ice melted is
Explanation of Solution
The expression of the energy released by
Substitute
As the energy released by the steam is much less than the amount of heat required melting the ice to water. So, the final temperature of the ice steam system will be
For the final common temperature of ice-steam system:
Here,
Substitute
Conclusion:
Therefore, the amount of ice melted is
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Chapter 20 Solutions
Physics for Scientists and Engineers, Technology Update (No access codes included)
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