Question
In: Physics
A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g...
- A 200 g aluminum calorimeter contains 500 g of water at 20 C. A 100 g piece of ice cooled to -20 C is placed in the calorimeter.
- Find the final temperature of the system, assuming no heat losses. (The specific heat of ice is 2.0 kJ/kg K)
- A second 200 g piece of ice at -20 C is added. How much ice remains in the system after it reaches equilibrium?
- Would your answer to part b be different if both pieces of ice were added at the same time?
(specific heat of aluminum is 0.9 kJ/kg K and water is 4.18 kJ/kg K)
Solutions
genius_generous answered 4 months agoRelated Solutions
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...
A 200 g aluminum calorimeter can contain 500 g of water at 20
C. A 100 g piece of ice cooled to -20 C is placed in the
calorimeter.
A) Find the final temperature of the system, assuming no heat
losses. (Assume that the specific heat of ice is 2.0 kJ/kg K)
B) A second 200 g piece of ice at -20 C is added. How much ice
remains in the system after it reaches equilibrium?
C) Would your answer...
A 200 g aluminum calorimeter can contain 500 g of water at 20 C. A 100...
A 200 g aluminum calorimeter can contain 500 g of water at 20
C. A 100 g piece of ice cooled to -20 C is placed in the
calorimeter.
Find the final temperature of the system, assuming no heat
losses. (Assume that the specific heat of ice is 2.0 kJ/kg K)
A second 200 g piece of ice at -20 C is added. How much ice
remains in the system after it reaches equilibrium?
Would your answer to part b...
If 200 g of water is contained in a 300g aluminum calorimeter at 20
If 200 g of water is contained in a 300g aluminum calorimeter at
20
A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0 °C. A 100.0 g...
A 200.0 g aluminum calorimeter contains 600.0 g of water at 20.0
°C. A 100.0 g piece of
ice is cooled to −20.0 °C and then placed in the calorimeter. Use
the following specific
heats: cAl = 900.0 J Kg-1 °C-1, cwater = 4186 J Kg-1 °C-1, cice =
2.10 x 103 J Kg-1 °C-1. The
latent heat of fusion for water is LF = 333.5 x 103 J/Kg.
(a) Find the final temperature of the system, assuming no heat...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter cup containing 260 g of...
Steam at 100°C is condensed into a 54.0 g aluminum calorimeter
cup containing 260 g of water at 25.0°C. Determine the amount of
steam (in g) needed for the system to reach a final temperature of
64.0°C. The specific heat of aluminum is 900 J/(kg · °C).
A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C . A 124.0-g block of...
A coffee-cup calorimeter contains 130.0 g of water at 25.3 ∘C .
A 124.0-g block of copper metal is heated to 100.4 ∘C by putting it
in a beaker of boiling water. The specific heat of Cu(s) is 0.385
J/g⋅K . The Cu is added to the calorimeter, and after a time the
contents of the cup reach a constant temperature of 30.3 ∘C .
Part A
Determine the amount of heat, in J , lost by the copper
block....
A coffee cup calorimeter contains 152.18 g of water at 20.90 °C. A 55.336 g piece...
A coffee cup calorimeter contains 152.18 g of water at 20.90 °C.
A 55.336 g piece of iron is heated to 98.37 °C. The piece of iron
is added to the coffee cup caloriemter and the contents reach
thermal equilibrium at 23.60 °C. The specific heat capacity of iron
is 0.449 J g⋅K and the specific heat capacity of water is 4.184 J
g⋅K . How much heat, q , is lost by the piece of iron?
How much heat,...
A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of water...
A 200 g insulated aluminum cup at 16 ∘C is filled with 255 g of
water at 100 ∘C
a) Determine the final temperature of the mixture.
b) Determine the total change in entropy as a result
of the mixing process (use
ΔS=∫dQ/T).
100 g of ice at -20°C are mixed with 250 g of water at 20°C in...
100 g of ice at -20°C are mixed with 250 g of water at 20°C in
an insulated calorimeter. What is the final temperature of the
system? How many grams of liquid water and how many grams of ice
will you find after the system equilibrates? find T in degrees C; m
of solid (in grams); m of liquid (in grams)
T=____
ms=____
mliq=____
A calorimeter contains 20.0 mL of water at 12.5 ∘C . When 1.40 g of X...
A calorimeter contains 20.0 mL of water at 12.5 ∘C . When 1.40 g
of X (a substance with a molar mass of 64.0 g/mol ) is added, it
dissolves via the reaction
X(s)+H2O(l)→X(aq)
and the temperature of the solution increases to 28.5 ∘C .
Calculate the enthalpy change, ΔH, for this reaction
per mole of X.
Assume that the specific heat of the resulting solution is equal
to that of water [4.18 J/(g⋅∘C)], that density of water is 1.00...
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