Question

A copper block of mass 17.5 kg initially at 481 K is immersed in 31.5 kg of water initially at 298 K.

CP,m(H2O,l)=75.3J⋅K−1⋅mol−1

CP,m(Cu,s)=24.4J⋅K−1⋅mol−1

Assume that the heat capacity of Cu remains constant at its 298.15 K value over the temperature interval of interest.

1) Calculate ΔS for the water.

2) Calculate ΔS for the Cu block.

Answer #1

Calculate the minimum work needed to reduce the temperature of a
1.0-g block of copper form 1.10 K to 0.10 K, the surroundings being
at 1.20 K. Proceed by supposing that the heat capacity remains
constant at 39 m J K-1 mol-1 and that the
coefficient of performance can be evaluated at the mean temperature
of the block. Then go on to do a more realistic calculation in
which Cp,m = AT3 + BT, with A = 48.2 m J...

A cooper block having a mass of 10 kg and at a temperature of
800 K is placed in a well-insulated vessel containing 100 kg of
water initially at 290 K. Calculate:
a) Calculate the entropy change for the block, the water, and
the total process.
b) What is the maximum amount of work that could have been
obtained from the copper block and water in a Carnot engine? The
heat capacities are 4.185 kJ/kg/K for water and 0.398 kJ/kg/K...

A 50 kg copper block initially at 350 oC is quenched in a
closed, rigid insulated tank containing 120 L of liquid water at 25
oC. Specific heat of copper, Cc = 385 J/(kgK), specific heat of
liquid water, Cw = 4180J/(kgK). (i) Calculate the entropy change
(kJ/K) of copper block. (ii) Determine the entropy change (kJ/K) of
liquid water.

Consider an isolated system containing two blocks of copper with
equal mass. One block is initially at 0oC while the other is at
100oC.They are brought into contact with each other and allowed to
thermally equilibrate. What is the entropy change for the system
during this process? The heat capacity for copper is Cp =
24.5 [J/mol k]

Please Show all work, thank you!
A copper block with a mass of 400 grams is cooled to 77 K by
being immersed in liquid nitrogen. The block is then placed in a
Styrofoam cup containing some water that is initially at +50.0°C.
Assume no heat is transferred to the cup or the surroundings. The
specific heat of liquid water is 4186 J/(kg °C), of solid water is
2060 J/(kg °C), and of copper is 385 J/(kg °C). The latent...

A block of copper has a mass of 100 kg and an initial
temperature of 900 K. Copper can be modeled as an incompressible
substance with a specific heat capacity of 0.4 kJ/kg-K.
a.) The copper block is dropped into a large lake at 300 K and
allowed to come to thermal equilibrium. How much entropy is
generated (kJ/K)?
b.) If a reversible heat engine were connected between the lake
and the copper block and operated until the temperature of...

A 1.05 kg block of copper at 100°C is placed in an insulated
calorimeter of negligible heat capacity containing 3.50 L of liquid
water at 0.0°C. (a) Find the entropy change of the copper block.
J/K (b) Find the entropy change of the water. J/K (c) Find the
entropy change of the universe. J/K

A 4.2-kg block of ice originally at 263 K is placed in thermal
contact with a 13.4-kg block of silver (cAg = 233
J/kg-K) which is initially at 1075 K. The H2O - silver
system is insulated so no heat flows into or out of it.
1) At what
temperature will the system achieve equilibrium?
2)
What will be the
phase of the H2O at equilibrium?
Solid (ice)
Liquid (water)
Gas (vapor)

A copper block is removed from a 320 ∘C oven and dropped into
1.20 kg of water at 22.0 ∘C. The water quickly reaches 27.5 ∘C∘and
then remains at that temperature.
What is the mass of the copper block? The specific heats of
copper and water are 385 J/(kg⋅K) and 4190 J/(kg⋅K) respectively.
Express your answer with the appropriate units.

Calculate ΔH and ΔS when a 10.0 kg block of Fe at 500 K is
placed in contact with a 5.0 kg block of Fe at 273 K. The specific
heat capacity of Fe is 0.449 J K-1 g-1. Ignore the effect of the
container.

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