Question

A 60.0 g aluminum block, initially at 55.00 °C, is submerged
into an unknown mass of water at 293.15 K in an insulated
container. The final temperature of the mixture upon reaching
thermal equilibrium is 25.00 °C. What is the approximate
**mass** of the **water**? The specific
heat of water is 4.18 J/g ** ^{.}** °C. The
specific heat of aluminum is 0.897 J/g

Answer #1

A silver block, initially at 59.3 ∘C, is submerged into 100.0 g
of water at 25.3 ∘C, in an insulated container. The final
temperature of the mixture upon reaching thermal equilibrium is
26.5 ∘C.
What is the mass of the silver block?

A silver block, initially at 55.0 ∘C, is submerged into 100.0 g
of water at 25.2 ∘C, in an insulated container. The final
temperature of the mixture upon reaching thermal equilibrium is
27.8 ∘C. What is the mass of the silver block?

A silver block, initially at 55.6 ∘C, is submerged into 100.0 g
of water at 25.2 ∘C, in an insulated container. The final
temperature of the mixture upon reaching thermal equilibrium is
27.3 ∘C. Part A What is the mass of the silver block?

A 32.5 g iron rod, initially at 22.6 ∘C, is submerged into an
unknown mass of water at 63.1 ∘C, in an insulated container. The
final temperature of the mixture upon reaching thermal equilibrium
is 59.2 ∘C.
What is the mass of the water?
Express your answer to two significant figures and include the
appropriate units.

A 32.9 g iron rod, initially at 22.4 ∘C, is submerged into an
unknown mass of water at 62.6 ∘C, in an insulated container. The
final temperature of the mixture upon reaching thermal equilibrium
is 58.4 ∘C.
What is the mass of the water?
Express your answer to two significant figures and include the
appropriate units.

1. A silver block, initially at 55.1 ∘C, is submerged into 100.0
g of water at 24.9 ∘C, in an insulated container. The final
temperature of the mixture upon reaching thermal equilibrium is
27.2 ∘C.
What is the mass of the silver block? (Express answer to two
significant figures and appropriate units)

A 500-g aluminum container holds 300 g of water. The water and
aluminum are initially at 40∘C. A 200-g iron block at 0∘C is added
to the water. Assume the specific heat of iron is 450 J/kg⋅∘C, the
specific heat of water 4180 J/kg⋅∘C and the specific heat of
aluminum is 900 J/kg⋅∘C
.
1Determine the final equilibrium temperature.
2.Determine the change in thermal energy of the aluminum
3.Determine the change in thermal energy of the water. 4.
Determine...

A 26.5-g aluminum block is warmed to 65.2 ∘Cand plunged into an
insulated beaker containing 55.2 g of water initially at 22.2 ∘C.
The aluminum and the water are allowed to come to thermal
equilibrium. (Cs,H2O=4.18 J/g⋅∘C,
Cs,Al=0.903J/g⋅∘C)
Assuming that no heat is lost, what is the final temperature of
the water and aluminum?

An insulated aluminum calorimeter vessel of 150 g mass contains
300 g of liquid nitrogen boiling at 77 K. A metal block at an
initial temperature of 303 K is dropped into the liquid nitrogen.
It boils away 15.8 g of nitrogen in reaching thermal equilibrium.
The block is then withdrawn from the nitrogen and quickly
transferred to a second insulated copper calorimeter vessel of 200
g mass containing 500 g of water at 30.1 degrees celsius. The block
coolds...

1a) A 25.5-g piece of lead initially at 98.6 °C is submerged
into 122.3 g of water at 20.9 °C. What is the final temperature of
the metal once the metal and water reaches thermal equilibrium? The
specific heats of lead and water are 0.128 J/g·°C and 4.18 J/g·°C,
respectively.

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