8. Thermochemistry

Thermal Equilibrium

Thermal Equilibrium, Temperature and Temperature Scales | A-level Physics | AQA, OCR, Edexcel

If 50.0 mL of ethanol (density = 0.789 g>mL) initially at 7.0 °C
is mixed with 50.0 mL of water (density = 1.0 g/mL) initially at
28.4 °C in an insulated beaker, and assuming that no heat is
lost, what is the final temperature of the mixture?

Two substances, A and B, initially at different temperatures,
come into contact and reach thermal equilibrium. The mass of
substance A is 6.15 g and its initial temperature is 20.5 °C. The
mass of substance B is 25.2 g and its initial temperature is 52.7
°C. The final temperature of both substances at thermal equilibrium
is 46.7 °C. If the specific heat capacity of substance B is
1.17 J>g # °C, what is the specific heat capacity of substance A?

Thermal Equlibrium

Dry ice is solid carbon dioxide. Instead of melting, solid carbon
dioxide sublimes according to the equation:
CO2(s)¡CO2( g)

◀ When carbon dioxide sublimes,
the gaseous cO2 is cold enough
to cause water vapor in the air to
condense, forming fog.

When dry ice is added to warm water, heat from the water
causes the dry ice to sublime more quickly. The evaporating carbon
dioxide produces a dense fog often used to create special effects.
In a simple dry ice fog machine, dry ice is added to warm
water in a Styrofoam cooler. The dry ice produces fog until it
evaporates away, or until the water gets too cold to sublime the
dry ice quickly enough. Suppose that a small Styrofoam cooler
holds 15.0 L of water heated to 85 °C. Use standard enthalpies of
formation to calculate the change in enthalpy for dry ice sublimation,
and calculate the mass of dry ice that should be added
to the water so that the dry ice completely sublimes away when
the water reaches 25 °C. Assume no heat loss to the surroundings.
(The ΔH °f for CO2(s) is -427.4 kJ/mol.)

Relationship between Temperature & Thermal Equilibrium | Skill-Lync

Heat Transfer and Thermal Equilibrium

A 2.85-g lead weight, initially at 10.3 °C, is submerged in 7.55 g
of water at 52.3 °C in an insulated container. What is the final
temperature of both substances at thermal equilibrium?

A 31.1-g wafer of pure gold, initially at 69.3 °C, is submerged into
64.2 g of water at 27.8 °C in an insulated container. What is the
final temperature of both substances at thermal equilibrium?

A 32.5-g iron rod, initially at 22.7 °C, is submerged into an unknown
mass of water at 63.2 °C, in an insulated container. The
final temperature of the mixture upon reaching thermal equilibrium
is 59.5 °C. What is the mass of the water?

A silver block, initially at 58.5 °C, is submerged into 100.0 g of
water at 24.8 °C, in an insulated container. The final temperature
of the mixture upon reaching thermal equilibrium is 26.2 °C.
What is the mass of the silver block?

A 25.5-g aluminum block is warmed to 65.4 °C and plunged into
an insulated beaker containing 55.2 g water initially at 22.2 °C.
The aluminum and the water are allowed to come to thermal
equilibrium. Assuming that no heat is lost, what is the final temperature of the water and aluminum?

We pack two identical coolers for a picnic, placing 24 12-ounce
soft drinks and five pounds of ice in each. However, the drinks
that we put into cooler A were refrigerated for several hours before
they were packed in the cooler, while the drinks that we put into
cooler B were at room temperature. When we open the two coolers
three hours later, most of the ice in cooler A is still present, while
nearly all of the ice in cooler B has melted. Explain this difference.

If 53.2 g Al at 120.0 ºC is placed in 110.0 g H2O at 90 ºC within an insulated container that absorbs a negligible amount of heat, what is the final temperature of the aluminum? The specific heat capacities of water and aluminum are 4.184 J/g ∙ ºC and 0.897 J/g ∙ ºC, respectively.

An ice cube with a mass of 20 g at -20 °C (typical freezer 
temperature) is dropped into a cup that holds 500 mL of 
hot water, initially at 83 °C. What is the final temperature 
in the cup? The density of liquid water is 1.00 g>mL; the 
specific heat capacity of ice is 2.03 J>g@C; the specific heat 
capacity of liquid water is 4.184 J>g@C; the enthalpy of 
fusion of water is 6.01 kJ>mol.

What is the Zeroth Law of Thermodynamics?

A 25.0 g piece of granite at 100.0°C was added to 100.0 g of water of 25.0°C, and the temperature rose to 28.4°C. What is the specific heat capacity of the granite? (The specific heat capacity for water is 4.18 J/(g•°C).) (LO 9.10)
(a) 0.563 J/(g•°C)
(b) 1.53 J/(g•°C)
(c) 0.992 J/(g•°C)
(d) 0.794 J/(g•°C)

The Zeroth Law of Thermodynamics: Thermal Equilibrium

Thermal Equilibrium Example 1

Under non-ideal conditions, calorimeter absorbs some of the heat from the object.

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Hess's Law

Hess's Law involves the use of partial reactions in the determination of the overall enthalpy of reaction.

Nature of Energy

Thermochemistry is the study of matter and energy associated with chemical reactions or physical changes.&nbsp;

Endothermic & Exothermic Reactions

Endothermic and Exothermic Reactions involve the absorbing and releasing of thermal energy respectively.&nbsp;&nbsp;

Heat Capacity

Heat Capacity is the amount of heat required to change the temperature of a substance.&nbsp;

Thermochemical Equations

Thermochemical Equations&nbsp;involve a balanced chemical equation with a given enthalpy value.

Internal Energy

The Internal Energy of a system is the total energy from all forms of kinetic and potential energy.&nbsp;

Kinetic & Potential Energy

Mechanical Energy is the energy associated with an object's velocity (Kinetic Energy) and its position (Potential Energy).&nbsp;

Formation Equations

Formation Equations involve the standard states of elements combining to form 1 mole of product.

Enthalpy of Formation

The Enthalpy of Formation for an element is a key component in determining the enthalpy of reaction.&nbsp;

Thermal Equilibrium involves two substances that are in physical contact reaching the same final temperature over time.&nbsp;

Constant-Pressure Calorimetry

Constant-Pressure Calorimetry uses a coffee cup calorimeter to determine the heat transfers occurring in a liquid solution.

Constant-Volume Calorimetry

Constant-Volume Calorimetry uses a bomb calorimeter and a combustion reaction to determine its enthalpy of reaction.&nbsp;

First Law of Thermodynamics

The First Law of Thermodynamics states that energy cannot be created nor destroyed, but instead is transferred.&nbsp;

First Law of Thermodynamics -

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