Question

A hot lump of 38.038.0 g of iron at an initial temperature of 79.7 °C79.7 °C is placed in 50.0 mL H2OH2O initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the iron and water, given that the specific heat of iron is 0.449 J/(g·°C)?0.449 J/(g·°C)? Assume no heat is lost to surroundings.

Answer #1

A hot lump of 47.6 g of iron at an initial temperature of 50.8
°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
iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings.

A hot lump of 37.8 g of iron at an initial temperature of 51.3
°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
iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings.

A hot lump of 44.5 g of iron at an initial temperature of 74.5
°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
iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings.

A hot lump of 46.0 g of iron at an initial temperature of 91.5
°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
iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings.

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 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 hot lump of 26.3 g of aluminum at an initial temperature of
67.2 °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 aluminum and water given that the specific heat of aluminum
is 0.903 J/(g·°C)? Assume no heat is lost to surroundings.

A hot lump of 42.6 g of aluminum at an initial temperature of
62.2 °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 aluminum and water given that the specific heat of aluminum
is 0.903 J/(g·°C)? Assume no heat is lost to surroundings. Please
show all work

1. A hot lump of 46.2 g of iron at an initial temperature of
77.9 °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 iron and water given that the specific heat of iron is 0.449
J/(g·°C)? Assume no heat is lost to surroundings. 2.When 1422 J of
heat energy is added to 40.8 g of hexane, C6H14, the temperature
increases by 15.4 °C....

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