Question

What is the final temperature (in C) of 1.50 g of water with an initial temperature of 24.0 C after 6.969 J of heat is added to it?

Answer #1

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....

A calorimeter contains 75.0 g of water at an initial temperature
of 25.2 °C. 151.28 g of copper metal at a temperature of 95.5 °C
was placed in the calorimeter. The equilibrium temperature was 36.2
°C. The molar heat capacity of water is 75.4 J / mol °C. Determine
the molar heat capacity of the copper.

A 25 g gold nugget with an initial temperature of 60 °C is
dropped into an insulated cup containing 100 ml of water initially
at a temperature of 5°C. What is the final temperature after
thermal equilibrium is established?
Table 3.4 Specific Heat Capacities of Some Common Substances
Substance Specific Heat Capacity (J/g °C) Lead 0.128 Gold 0.128
Silver 0.235 Copper 0.385 Iron 0.449 Aluminum 0.903 Ethanol 2.42
Water 4.184

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.

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 46.2 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.

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