Question
In: Physics
In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is...
In an experiment, 300 g of aluminum (specific heat of 900 J/kg*K) at 120 Celsius is mixed with 60 g of water at 20 Celsius, with the mixture thermally isolated. You will need to look up the specific heat of water. (a) What is the equilibrium temperature? (b) What is the entropy change for the aluminum block? (c) What is the entropy change for the water? (d) What is the entropy change for the aluminum-water system?
Solutions
genius_generous answered 1 year agoRelated Solutions
The value of specific heat for copper is 390 J/kg⋅C∘, for aluminun is 900 J/kg⋅C∘, and...
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 225 g block of copper at 245
∘C is placed in a 155 g aluminum calorimeter cup containing 835 g
of water at 14.0 ∘C ? Express your answer using three significant
figures.
The value of specific heat for copper is 390 J/kg⋅C∘, for aluminun is 900 J/kg⋅C∘, and...
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∘.
Part A
What will be the equilibrium temperature when a 275 g block of
copper at 245 ∘C is placed in a 135 g aluminum calorimeter cup
containing 855 g of water at 15.0 ∘C?
Express your answer using three significant figures.'
T= ∘C
A chunk of brass with mass 0.6 kg, with specific heat 380 J/(kg· K), and with...
A chunk of brass with mass 0.6 kg, with specific heat 380 J/(kg·
K), and with temperature 400 K is placed in 0.6 kg of water, with
specific heat 4186 J/(kg· K), and with temperature 280 K. The water
and the brass are in an insulated container and come to thermal
equilibrium. Find the final temperature in kelvins (closest
answer).
AND
The asteroid Oumuamua observed this year in November traveled
around the sun at a speed of 87,500 m/s. Its...
A 5.00 g sample of aluminum (specific heat capacity = 0.89 J °C-1 g-1) and a...
A 5.00 g sample of aluminum (specific heat capacity = 0.89 J
°C-1 g-1) and a
10.00 g sample of iron (specific heat capacity = 0.45 J °C-1 g-1)
are heated to
100.0 °C. The mixture of hot iron and aluminum is then dropped into
91.9 g of
water at 23.7 °C.
i) State the conditions for phase equilibrium of this system.
NOTE: For an isolated system, the equilibrium state corresponds
to the state with maximum entropy.
Specific heat of ice: 2.09 J/(g⋅∘C Specific heat of liquid water: 4.18 J/(g⋅∘C) Enthalpy of fusion:...
Specific heat of ice: 2.09 J/(g⋅∘C
Specific heat of liquid water: 4.18 J/(g⋅∘C)
Enthalpy of fusion: ΔHfus=334J
Enthalpy of vaporization: ΔHvap=2250 J/g
How much heat energy, in kilojoules, is required to convert
47.0 g of ice at −−18.0 ∘C∘C to water at 25.0 ∘C?
1. A 5.88 kg piece of granite with a specific heat of 0.803 J g-1 °C-1...
1. A 5.88 kg piece of granite with a specific heat of 0.803 J
g-1 °C-1 and a temperature of 85.1 °C is
placed into 2.00 L of water at 19.0 °C. When the granite and water
come to the same temperature, what will the temperature be?
2. The combustion of methane (the chief component of natural
gas) follows the equation:
CH4(g) + 2O2(g) →
CO2(g) + 2H2O(g)
∆H° for this reaction is -802.3 kJ. How many grams of methane...
I just need to find the specific heat of copper, steel and aluminum. Experiment 12 Specific...
I just need to find the specific heat of copper, steel and
aluminum.
Experiment 12 Specific Heat Capacity [Calorimetry)
See the Introduction section onpage L2-2.
A metal sample of 'mass ms is heated in boiling water to a high
temperature of Tl, - 101.3 oC. It is then quickly placed in a
calorimeter cup of mass mc = 5T .9 grams containing liquid water of
mass m*, both at an initial cool temperature T.. The specific heat
capacity of liquid...
120 g + 18˚ water is in a calorimeter, whose heat capacity is 50 J /...
120
g + 18˚ water is in a calorimeter, whose heat capacity is 50 J /
˚C. Clarification is done by calculating what happens when 36 g of
ice of 0 ˚C is added in the calorimeter.
(Answer T = 0 ˚C, remaining approximately 6 g of ice)
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
Given that the specific heat capacities of ice and steam are
2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and
vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol,
respectively, and the specific heat capacity of water is 4.18
J/g°C, calculate the total quantity of heat evolved when 20.4 g of
steam at 162°C is condensed, cooled, and frozen to ice at
-50.°C.
Given that the specific heat capacities of ice and steam are 2.06 J/g°C and 2.03 J/g°C,...
Given that the specific heat capacities of ice and steam are
2.06 J/g°C and 2.03 J/g°C, the molar heats of fusion and
vaporization for water are 6.02 kJ/mol and 40.6 kJ/mol,
respectively, and the specific heat capacity of water is 4.18
J/g°C, calculate the total quantity of heat evolved when 13.2 g of
steam at 192°C is condensed, cooled, and frozen to ice at
-50.°C.
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