Question

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

Answer #1

mass of the nugget m_{n} = 25g

Initial temperature of nugget T_{1} =
60^{o}C

Final temperature of the nugget T

volume of water V = 100ml

density of water = 1g/cc = 1g/ml

mass of the water m_{w}= V*1 = 100g

Initial temperature of water T_{2} = 5^{o}C

Final temperature of water = T

since the thermal equilibrium is reached between the nugget and the water, the final temperatures of both are the same.

heat lost by the gold nugget = heat gained by the water

m_{n}c_{n}(T_{1} - T) =
m_{w}c_{w}(T - T_{2})

25*0.128*(60 - T) = 100*4.184*(T - 5)

=> 60 - T = 130.75(T - 5)

=> 60 - T = 130.75T - 653.75

=> 131.75T = 713.75

=> T = 5.4174 = 5.42^{o}C

Therefore the final temperature = 5.42^{o}C

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.

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

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 12.30-g block of solid gold at 63.62 °C is immersed in a
23.29-g pool of liquid ethanol with a temperature of 12.25 °C. When
thermal equilibrium is reached, what is the temperature of the gold
and ethanol?
Specific heat capacities: gold = 0.129 J/g °C; ethanol = 2.44
J/g °C
________°C

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 299 g silver figure of a polar bear is dropped into the 211 g
aluminum cup of a well‑insulated calorimeter containing 259 g of
liquid water at 21.5∘C. The bear's initial temperature is 96.5∘C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

A 281 g silver figure of a polar bear is dropped into the 219 g
aluminum cup of a well‑insulated calorimeter containing 269 g of
liquid water at 21.3∘C. The bear's initial temperature is 99.5∘C.
What is the final temperature of the water, cup, and bear when they
reach thermal equilibrium? The specific heats of silver, aluminum,
and liquid water are, respectively, 234 J/(kg·K), 910 J/(kg·K), and
4190 J/(kg·K).

Suppose that 23 g of each of the following substances is
initially at 26.0 ∘C. What is the final temperature of each
substance upon absorbing 2.25 kJ of heat?
For:
a) gold
b) silver
c) aluminum
d) water

Suppose that 27 g of each of the following substances is
initially at 28.0 ∘C. What is the final temperature of each
substance upon absorbing 2.40 kJ of heat?
a) Gold
b) silver
c) aluminum
d) water

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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