Question
In: Physics
0.7 kg of ice at 0 ◦C and 3 kg of water at Ti are brought...
0.7 kg of ice at 0 ◦C and 3 kg of water at Ti are brought into thermal contact in an iso- lated container. All the ice melts, and the mixture reaches an equilibrium temperature of 10 ◦C.
(a) (5 points) Determine the initial temperature Ti of the liquid water.
(b) (1 point) Determine the entropy change ∆S_melt associated with this amount of ice melting.
(c) (3 points) Determine the entropy change ∆S_coolwater associated with the decreasing temperature of the water. (Hint: find an expression for dQ in terms of dT.)
(d) (2 points) Determine the entropy change ∆S_warmwater associated with the increasing temperature of the melted ice.
(e) (2 points) Determine the net entropy change associated with this thermal process. Explain whether your result obeys the Second Law of Thermodynamics.
Solutions
genius_generous answered 1 year agoRelated Solutions
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A piece of ice at 0 0C is put in 2.00 Kg of water at 20...
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TK=TC+273.15)
a) Find the mass of ice?
Kg
b) Find the entropy change of ice?
J/K
c) Find the entropy change of water?
J/K
d) Find the total entropy change of sysem?
J/K
It is well known that water freezes at 0°C at atmospheric pressure. The mixture of liquid water and ice at 0°C is said to be
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1.45 kg of ice at -5 ∘C is dropped into 31 kg of water at temperature 15.3 ∘C . Part...
1.45 kg of ice at -5
∘C is dropped into 31
kg of water at temperature 15.3
∘C .
Part A - Final Temperature
What is the final temperature of the system? (If I've set the
problem up right, you should be given numbers such that all of the
ice has melted.)
Tf =
∘C
Part B - Entropy of Warming Ice
What is the change in entropy of the ice, as it warms up before
melting?
S =
J/K
Part C - Entropy...
Table 1. Steel Bolt Specific Heat Data Bolt Ti (°C) Water Ti (°C) Water and Bolt...
Table 1. Steel Bolt Specific Heat Data
Bolt Ti (°C)
Water Ti (°C)
Water and Bolt Tf (°C)
Water ΔT =
Tf - Ti
Bolt ΔT
(°C)
Bolt Mass (kg)
Water Mass (kg)
Steel Bolt
72
20
26
52
-72
.021
.15
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the water in the calorimeter. Use the equations provided above and
what you know about heat to solve for the specific heat (C) of...
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ice (which is initially at −15.0°C), what is the final temperature
(in °C)? You may assume that the water cools so rapidly that
effects of the surroundings are negligible.
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