Question
In: Physics
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 is
transferred to
or from the system.
(b) A second piece of ice at −20.0 °C with a mass of 100.0 g is
added. How
much solid ice remains in the system after the system reaches
equilibrium?
Solutions
genius_generous answered 2 years agoRelated Solutions
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...
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...
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 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,...
Part A A calorimeter contains 16.0 mL of water at 12.5 ∘C . When 1.70 g...
Part A
A calorimeter contains 16.0 mL of water at 12.5 ∘C . When 1.70 g
of X (a substance with a molar mass of 54.0 g/mol ) is added, it
dissolves via the reaction X(s)+H2O(l)→X(aq) and the temperature of
the solution increases to 30.0 ∘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...
PART A A calorimeter contains 27.0 mL of water at 14.5 ∘C . When 1.70 g...
PART A
A calorimeter contains 27.0 mL of water at 14.5 ∘C . When 1.70 g
of X (a substance with a molar mass of 75.0 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...
A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g of X...
A calorimeter contains 31.0 mL of water at 15.0 ∘C . When 2.50 g
of X (a substance with a molar mass of 62.0 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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