Question

Which of the following will have the largest temperature increase in response to 250 J of heat? ethanol, 2.42 J/g°C aluminum, 0.903 J/g°C copper, 0.385 J/g°C gold, 0.128 J/g°C

Answer #1

Assume that the mass is constant. m = 1 g

Heat required is constant Q = 250 J

For Ethanol

Q = m x Cp x temperature rise

Temperature rise = 250 J / (1 g x 2.42 J/gC) = 103.31 °C

For aluminum

Temperature rise = 250 J / (1 g x 0.903 J/gC) = 276.85 °C

For copper

Temperature rise = 250 J / (1 g x 0.385 J/gC) = 649.35°C

For gold

Temperature rise = 250 J / (1 g x 0.128 J/gC) = 1953.13°C

For the same mass and same heat required, lower the value of heat capacity of metal, higher the temperature increase.

Gold has the lowest heat capacity,

Gold will have the largest temperature increase in response to 250 J of heat.

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

The following table lists the specific heat capacities of select
substances: Substance Specific heat capacity [J/(g⋅∘C)] silver
0.235, copper 0.385, iron 0.449, aluminum 0.903, ethanol 2.42,
water 4.184, Water (2430 g ), is heated until it just begins to
boil.
If the water absorbs 5.07×105 J of heat in the process, what was
the initial temperature of the water? Express your answer with the
appropriate units.

You have three metal pans (Cu, Fe, Al) that you want to pre-heat
on the stovetop to cook. If the metal pans were all the same mass,
which would you heat up the quickest? Explain your reasoning.
Metal
Specific Heat Capacity (J/ g * C)
Copper
0.385
Iron
0.449
Aluminum
0.903

6) How much heat energy in J) is required to rise the
temperature of 250 g plate of pure aluminum "Al” from 25 °C to 55
°C. (Cp,m of Al = 24.35 JK' mol'']

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

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 4
g good block at 250 °C and a 1 g aluminum block at 120 °C are
placed on a 45 g sheet of copper at 20 °C. If the three objects are
well-insulted from their surroundings, what equilibrium temperature
do they eventually reach? The heat capacities of good, aluminum are
129, 900 and 385 J/(kgK), respectively.

The value of specific heat for copper is 390 J/kg⋅C∘, for
aluminun is 900 J/kg⋅C∘, and for water is 4186 J/kg⋅C∘.
What will be the equilibrium temperature when a 215 g block of
copper at 245 ∘C is placed in a 155 g aluminum calorimeter cup
containing 815 g of water at 16.0 ∘C?

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