Question

A 100-gram metal block is initially heated to 100 degrees Celsius. The copper block is then placed in 200-grams of water at 20 degrees Celsius. The block and the water are allowed to come to thermal equilibrium and reach a temperature of 23.52 degrees Celsius. a.) What is the change in temperature of the block and the water? b.) If the specific heat of water is 4.184 J/g C, what is the heat gained by the water? c.) What is the heat lost by the metal, and what is the specific heat of the metal?

Answer #1

A
47.5 block of an unknown metal is heated in a hot water bath to 100
degrees Celsius. When the block is placed in an insulated vessel
containing 130.0 g of water at 25.0 degrees Celsius, the final
temperature is 28.0 degrees Celsius. Determine the specific heat of
the unknown metal. The Cs for water is 4.18 J/g degrees
Celsius.

A hot lump of 45.0 g of iron at an initial temperature of 68.2
degrees celsius is placed in 50.0 mL of H2O initially at 25.0
degrees celsius and allowed to reach thermal equillibrium. What is
the final temperature of the iron and water given that the specific
heat of iron is 0.449 J/(G x degrees celsius)? Assume no heat is
lost to surroundings.

A 100g block of copper initially at 100°C is dropped into 1000g
of water initially at 0℃. The specific heat of copper is 0.0923 ???
?℃ ,. What is the final temperature of the water and copper when
they reach thermal equilibrium?

A metal is heated to 100 degrees Celsius and is cooled in room
temperature water at 20 degrees Celsius. If the mass of the water
is 100g, the metal's mass is 45g, and the final temperature of the
water/metal system is 31 degrees Celsius, what is the specific
heart of the metal.
Please leave final answer in kg.

A small ice cube (initially at -5.00 degrees Celsius) is placed
in a calorimeter along with 750.0 grams of water (at 45.00 degrees
Celsius) and a 250.0 gram piece of copper (at 100.00 degrees
Celsius). The system comes to thermal equilibrium at 43.34 degrees
Celsius. What is the mass of the ice cube?

A 35.7 gram sample of iron (heat capacity 0.45 g/J°C) was heated
to 99.10 °C and placed into a coffee cup calorimeter containing
42.92 grams of water initially at 15.15 °C. What will the final
temperature of the system be? (Specific heat of water is 4.184
J/g°C).
Please show work.

A hot lump of 46.2 g of copper at an initial temperature of 93.9
°C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to
reach thermal equilibrium. What is the final temperature of the
copper and water given that the specific heat of copper is 0.385
J/(g·°C)? Assume no heat is lost to surroundings.

A hot lump of 27.5 g of copper at an initial temperature of 54.7
°C is placed in 50.0 mL of H2O initially at 25.0 °C and allowed to
reach thermal equilibrium. What is the final temperature of the
copper and water given that the specific heat of copper is 0.385
J/(g·°C)? Assume no heat is lost to surroundings.

A sample of copper weighing 12.0g is heated to 100.0 degrees
celsius and then placed 50.0 mL of water at 26.5 degrees celsius.
What will the final temperature of the water be?

a 25.0g piece of aluminum (molar heat capacity of 24.03 J/g
degrees Celsius) is heated to 82.4 degrees Celsius and dropped into
a calorimeter containing water (specific heat capacity of water is
4.18 J/g degrees Celsius) initially at 22.3 degrees Celsius. The
final temperature of the water is 24.98 degrees Celsius. Calculate
the mass of water in the calorimeter.

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