Question

In an experiment, 100 g of aluminum (with a specific heat of 900
J/kg·K) at 79.0°C is mixed with 80.0 g of water (with a specific
heat of 4186 J/kg·K) at 43.0°C, with the mixture thermally
isolated. **(a)** What is the equilibrium temperature?
What are the entropy changes of **(b)** the aluminum,
**(c)** the water, and **(d)** the
aluminum-water system?

Answer #1

The value of specific heat for copper is 390 J/kg⋅C∘, for
aluminun is 900 J/kg⋅C∘, and for water is 4186 J/kg⋅C∘.
What will be the equilibrium temperature when a 215 g block of
copper at 245 ∘C is placed in a 155 g aluminum calorimeter cup
containing 815 g of water at 16.0 ∘C?

The value of specific heat for copper is 390 J/kg⋅C∘, for
aluminun is 900 J/kg⋅C∘, and for water is 4186 J/kg⋅C∘ What will be
the equilibrium temperature when a 215 g block of copper at 245 ∘C
is placed in a 155 g aluminum calorimeter cup containing 875 g of
water at 12.0 ∘C?

The value of specific heat for copper is 390 J/kg⋅C∘, for
aluminun is 900 J/kg⋅C∘,and for water is 4186 J/kg⋅C∘.
What will be the equilibrium temperature when a 275 g block of
copper at 255 ∘C is placed in a 155 g aluminum calorimeter cup
containing 815 g of water at 16.0 ∘C?

The value of specific heat for copper is 390 J/kg?C?, for
aluminun is 900 J/kg?C?, and for water is 4186 J/kg?C?. What will
be the equilibrium temperature when a 215 g block of copper at 255
?C is placed in a 155 g aluminum calorimeter cup containing 875 g
of water at 16.0 ?C?

An 100-g aluminum calorimeter contains 280 g of water at an
equilibrium temperature of 20°C. A 170-g piece of metal, initially
at 277°C, is added to the calorimeter. The final temperature at
equilibrium is 32°C. Assume there is no external heat exchange. The
specific heats of aluminum and water are 910 J/kg·K and 4190
J/kg·K, respectively. The specific heat of the metal is closest
to:
a) 270 J/kg·K.
b) 240 J/kg·K.
c) 330 J/kg·K.
d) 390 J/kg·K.
e) 360 J/kg·K.

Assuming the specific heat of water is 4200 J/kg/K and the
specific heat of aluminum is 900 J/Kg/K, what is the increase of
the system's entropy by the time it will reach equilibrium in
temperature if it is 160 grams of aluminum at 370 deg. K in a cup
of 1.3 kg of water at 281 deg. K

What mass of steam at 100°C must be mixed with 216 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 65.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

What mass of steam at 100°C must be mixed with 162 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 71.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg.

What mass of steam at 100°C must be mixed with 260 g of ice at
its melting point, in a thermally insulated container, to produce
liquid water at 73.0°C? The specific heat of water is 4186 J/kg·K.
The latent heat of fusion is 333 kJ/kg, and the latent heat of
vaporization is 2256 kJ/kg

Chapter 18, Problem 041
(a) Two 58 g ice cubes are dropped into 410 g
of water in a thermally insulated container. If the water is
initially at 20°C, and the ice comes directly from a freezer at
-11°C, what is the final temperature at thermal equilibrium?
(b) What is the final temperature if only one ice
cube is used? The specific heat of water is 4186 J/kg·K. The
specific heat of ice is 2220 J/kg·K. The latent heat of...

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