Question

2.50 kg of water at 90 (degrees of C) is contained in a thermally-isolated container. A 1.50 kg chunk of ice at - 10 degrees C is added to the water, in the same thermally isolated container. a.) Describe the final state of the system when it has reached thermal equilibrium, give the final temperature and the amount of ice let (if any). b.) Find the net change in entropy of the system during this process.

Answer #1

A 0.66300.6630 kg ice cube at −12.40−12.40 °C is placed inside a
rigid, thermally isolated chamber containing steam at 365.0365.0
°C. Later, you notice that the ice cube has completely melted into
a puddle of water. The specific heats of ice, water, and steam are
?ice=2093 J/(kg·∘C),cice=2093 J/(kg·∘C), ?water=4186
J/(kg·∘C),cwater=4186 J/(kg·∘C), and ?steam=2009
J/(kg·∘C),csteam=2009 J/(kg·∘C), respectively.
If the chamber initially contained 6.1906.190 moles of steam
(water) molecules before the ice was added, calculate the final
temperature ?fTf of the puddle...

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(a) Two 64 g ice cubes are dropped into 278 g of water in a
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Finding the equilibrium temperature of a mixture: An isolated
thermal system consists of a copper container ﬁlled with a quantity
of liquid water and a quantity of ice. What is the fully
thermalized state of the system (the ﬁnal temperature, how much
water, and how much ice) provided that initially there is 1.0kg of
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An insulated container has 2.00kg of water at 25◦C to which an
unknown
amount of ice at 0◦C is added. The system comes to an
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fusion for ice is kg·K
kJ LF =334kg.
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(c) What is the change in...

A perfectly insulated thermos contains 0.300 kg of water
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In a thermally isolated environment, you add ice at 0°C and
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