Practice: A sample of copper absorbs 3.53 kJ of heat, which increases the temperature by 25 ºC, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J / g ºC.

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Enthalpy |

**Heat Capacity** is the amount of heat required to change the temperature of a substance.

Example #1: If the temperature of a water bath goes from 25 K to 50 K, what can be said about the amount of heat?

Example #2: If 15.7 g of silver raises its temperature by 17.2 ºC when it absorbs 6845.5 J, what is its molar heat capacity?

Example #3: How much heat (in kJ) is released when 120.0 g H_{2}O goes from 90 ºC to 45 ºC? The specific heat capacity of H_{2}O is 4.184 J / g ºC.

Practice: A sample of copper absorbs 3.53 kJ of heat, which increases the temperature by 25 ºC, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J / g ºC.

Practice: Based on their given specific heat capacities which compound would show the greatest temperature change upon absorbing 25.0 J of heat?

Practice: 50.00 g of heated metal ore is placed into an insulated beaker containing 822.5 g of water. Once the metal heats up the final temperature of the water is 32.08 ºC. If the metal gains 14.55 kJ of energy, what is the initial temperature of the water? The specific heat capacity of copper is 4.184 J / g ºC.

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Concept #1: Heat Capacity

Example #1: Heat Capacity Example 1

Concept #2: Heat Capacity

Example #2: Heat Capacity Example 2

Concept #3: Heat Capacity

Example #3: Heat Capacity Example 3

Practice #1: Heat Capacity Practice 1

Practice #2: Heat Capacity Practice 2

Practice #3: Heat Capacity Practice 3

If three samples of silver, one with a mass of 10.0 grams, another with a mass of 50.0 grams and a third with a mass of 100.0 grams each absorb 36.3 kJ of heat which sample will experience the greatest increase in temperature?
The 10.0 gram sample
The 50.0 gram sample
The 100.0 gram sample
Each will have the same increase in temperature
Depends on the starting temperature of each

The specific heat of copper metal is 0.385 J/g K. How many joules of heat are necessary to raise the temperature of a 1.42-kg block of copper from 25.0 °C to 88.5 °C?
A) 3.47 x 104 J
B) 34.7 J
C) 2.34 x 105 J
D) 8.46 J

Which substance (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?
a. 50.0 g Al, CAl = 0.903 J/g°C
b. 50.0 g Cu, CCu = 0.385 J/g°C
c. 25.0 g granite, Cgranite = 0.79 J/g°C
d. 25.0 g Au, CAu = 0.128 J/g°C
e. 25.0 g Ag, CAg – 0.235 J/g°C

The molar heat capacity of silver is 25.35 J/mol × oC . Calculate how much energy (in kJ) it would take to raise the temperature of 15.7 g of the silver metal by 17.2 oC.

Which of the following substances (with specific heat capacity provided) would show the greatest temperature change upon absorbing 100.0 J of heat?
a) 10.0 g Ag, CAg = 0.235 J/g°C
b) 10.0 g H2O, CH2O = 4.18 J/g°C
c) 10.0 g ethanol, Cethanol = 2.42 J/g°C
d) 10.0 g Fe, CFe = 0.449 J/g°C
e) 10.0 g Au, CAu = 0.128 J/g°C

How much energy must be transferred to raise the temperature of a cup of coffee that is 250 mL from 20.5 °C to 368.8 K? Assume that water and coffee have the same density 1.00 g/mL and specific heat capacity (4.184 J/g•K).

Which substance (with specific heat capacity provided) would show the smallest temperature change upon gaining 200.0 J of heat?
a) 50.0 g Al, CAl = 0.903 J/g°C
b) 50.0 g Cu, CCu = 0.385 J/g°C
c) 25.0 g granite, Cgranite = 0.79 J/g°C
d) 25.0 g Au, CAu = 0.128 J/g°C
e) 25.0 g Ag, CAg = 0.235 J/g°C

If it takes 0.216 kJ of heat to raise the temperature of a 12.0 g piece of Al from 15.5 to 35.5 oC, what is the specific heat (J/g K) of Al?

How much energy is required to change the temperature of 21.5 g Cu from 27 to 88.1 °C? The specific heat capacity of copper is 0.385 J/gK.
223 J
506 J
641 J
729 J
3.41 x 103

When 68.00 J of energy are added to a sample of Gallium that is initially at 25°C, the temperature rises to 38.0° C. What is the volume of the sample?
The specific heat of Gallium is 0.372 J•g -1•°C-1.
Density of Gallium is 5.904 g•cm–3.
a) 2.38 cm3
b) 4.28 cm3
c) 14.1 cm3
d) 31.0 cm3

Three separate 3.5g blocks of Al, Cu, and Fe at 25 °C each absorb 0.505 kJ of heat. Which block reaches the highest temperature? The specific heats of Al, Cu, and Fe are 0.900 J/g•°C, 0.385J/g•°C, and 0.444 J/g•°C, respectively.
a) Fe
b) Fe and Cu
c) Al and Cu
d) Al
e) Cu

The molar heat capacity of silver is 25.35 J/mol•°C. Calculate how much energy (in kJ) it would take to raise the temperature of 15.7 g of the silver metal by 17.2 °C.

In an exothermic chemical reaction:
A + 2 B → C
When the amount of A and B reacting is doubled, what is expected to the amount of heat released?
A. No change in the amount of heat released
B. The amount of heat released is two times the original
C. The amount of heat released is four times the original
D. The amount of heat released is eight times the original

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.
A) 3.95 J/g°C
B) 1.87 J/g°C
C) 2.29 J/g°C
D) 2.53 J/g°C
E) 4.38 J/g°C

When 75.4 J of energy is absorbed by 0.25 mol of CCl 4, what is the temperature change of CCl4? The specific heat capacity of CCl 4 is 0.861 J/g·°C. Molar mass of CCl 4 is 153.81 g/mol.
A) 17.8°C
B) 21.9°C
C) 2.3°C
D) 9.1°C
E) 44.6°C

Which of the following statements are correct?
A. specific heat capacity is defined as the amount of heat energy required to raise the temperature of an object 1K
B. under conditions of constant pressure, no work is done on or by the system
C. molar heat capacity is defined as the amount of heat energy required to raise the temperature of 1 mole of a substance 1K
D. heat is always transferred from an object with a lower temperature to an object with a higher temperature

It takes 75.0 J to raise the temperature of an 19.3 g piece of unknown metal from 21.0oC to 46.7oC. What is the specific heat of the metal?

Which will release more heat as it cools from 50°C to 25°C, 1 kg of water or 1 kg of aluminum? How do you know?

Two solid objects, A and B, are placed in boiling water and allowed to come to the temperature of the water. Each is then lifted out and placed in separate beakers containing 1000 g water at 10.0°C. Object A increases the water temperature by 3.50°C; B increases the water temperature by 2.60°C. (a) Which object has the larger heat capacity?

The specific heat of iron metal is 0.450 J/g-K. How many J of heat are necessary to raise the temperature of a 1.05-kg block of iron from 25.0°C to 88.5°C?

A house is designed to have passive solar energy features. Brickwork incorporated into the interior of the house acts as a heat absorber. Each brick weighs approximately 1.8 kg. The specific heat of the brick is 0.85 J/g-K. How many bricks must be incorporated into the interior of the house to provide the same total heat capacity as 1.7 x 103 gal of water?

A sample of calcium carbonate [CaCO3 (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1oC to 28.5oC. If the specific heat of calcium carbonate is 0.82 J/goC, what is the mass (in grams) of the sample?
A. 0.20
B. 5.0
C. 7.5
D. 410
e. 5.0 x 103

A sample of copper absorbs 43.6 kJ of heat, resulting in a temperature rise of 75°C, determine the mass (in kg) of the copper sample if the specific heat capacity of copper is 0.385 J/g°C.
A) 6.62 kg
B) 1.51 kg
C) 3.64 kg
D) 7.94 kg
E) 1.26 kg

Determine the specific heat capacity of an alloy that requires 59.3 kJ to raise the temperature of 150.0 g alloy from 298 K to 398 K.
A) 4.38 J/g°C
B) 3.95 J/g°C
C) 2.29 J/g°C
D) 1.87 J/g°C
E) 2.53 J/g°C

Calculate the amount of heat (in kJ) necessary to raise the temperature of 47.8 g benzene by 57 K. The specific heat capacity of benzene is 1.05 J/g°C
A) 2.59 kJ
B) 2.86 kJ
C) 3.85 kJ
D) 1.61 kJ
E) 16.6 kJ

Calculate the amount of heat (in kJ) required to raise the temperature of a 79.0 g sample of ethanol from 298 K to 385 K. The specific heat capacity of ethanol is 2.42 J/g°C.
A) 12.9 kJ
B) 57.0 kJ
C) 73.6 kJ
D) 28.4 kJ
E) 16.6 kJ

How much heat, in kJ, is required to raise the temperature of 125 g H 2O from 24.3°C to 64.9°C? The specific heat of water is 4.18 J g-1 °C-1.
A) 21.2 kJ
B) 42.4 kJ
C) 12.7 kJ
D) 33.9 kJ
E) 523 kJ

Calculate the amount of heat necessary to raise the temperature of 12.0 g of water from 15.4°C to 93.0°C.
A) 0.027 J
B) 324 J
C) 389 J
D) 931 J
E) 3,890 J

To raise 232 g of an unknown liquid from 15°C to 60°C, 17.9 kJ of energy are required. What is the specific heat capacity, Cs, of the liquid?
A) 5.41 J/(g ∙ °C)
B) 1.71 J/(g ∙ °C)
C) 3.48 J/(g ∙ °C)
D) 1.10 J/(g ∙ °C)

How much heat is absorbed by a pan made of iron, with a mass of 150 g whose temperature rises from 25.0°C to 100.0°C?

A chemistry student weighs a rock and finds its mass to be 4.7 g. She then finds that upon absorption of 57.2 J of heat, the temperature of the rock rises from 25 °C to 57 °C. Find the specific heat capacity of the substance composing the rock.

Calculate q (in kJ) when 2.00 g of water is heated from 37 °C to 47 °C. The specific heat capacity of water is 4.184 J/g•°C.

Which one of the following statements is correct?A) The SI unit of specific heat capacity is calories per gram (cal/g)B) Specific heat capacity is a positive value for liquids and a negative value for solidsC) When heat is transferred from the surrounding to the system q is negativeD) The larger the heat capacity of an object the more thermal energy it can storeE) Heat is transformed from the systems to the surroundings in an endothermic process

Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb 3.10 MJ of energy (in the form of heat) if the temperature of the sodium is not to increase by more than 10.0. Use Cm = 30.8 J/(K·mol) for Na(l).

What is the molar heat capacity of liquid water? Express your answer using four significant figures.

The specific heat of a certain type of cooking oil is 1.75 J/(g • °C). How much heat energy is needed to raise the temperature of 2.02 kg of this oil from 23 °C to 191 °C?

What is the heat capacity of 155 g of liquid water?

Suppose that 26 g of each of the following substances is initially at 28.0 ºC. What is the final temperature of each substance upon absorbing 2.40 kJ of heat?a) aluminum

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/g • °C. A. 3 °C B. 14 °C C. 22 °C D. 47 °C E. None of these choices is correct.

The specific heat of aluminum is 0.900 J/g • °C. How many joules of heat are absorbed by 15.0 g of Al if it is heated from 20.0°C to 60.0°C?a. 270 Jb. 2.40 Jc. 540 Jd. 812 Je. 0.000117 J

If 125 cal of heat is applied to a 60.0-g piece of copper at 22.0°C, what will the final temperature be? The specific heat of copper is 0.0920 cal/(g • °C). Express your answer with the appropriate units.

An 80.0-gram sample of a gas was heated from 25°C to 225°C. During this process, 346 J of work was done by the system and its internal energy increased by 6565 J. What is the specific heat of the gas?

Typically, water runs through the baseboard copper tubing and, therefore, fresh hot water is constantly running through the piping. However, consider a pipe where water was allowed to sit in the pipe. The hot water cools as it sits in the pipe. What is the temperature change (ΔT) of the water if 202.0 g of water sat in the copper pipe releasing 1760. J of energy to the pipe? The specific heat of water is 4.184 J/(g •°C). Express your answer to four significant figures.

Some homes that use baseboard heating use copper tubing. Hot water runs through and heats the copper tubing, which in turn heats aluminum fins. It is actually the aluminum fins that heat the air rising through the fins. How much energy (J) would it take to heat a section of the copper tubing that weighs about 505.0 g, from 13.33°C to 22.38°C? Copper has a specific heat of 0.3850 J/g • °C). Express your answer to four significant figures.

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