8. Thermochemistry

Formation Equations

5.1 Standard enthalpy changes of formation and combustion

How to Calculate Enthalpy of Reaction using Heat of Formation Examples, Practice Problems, Explained

CHEMISTRY 101:  Standard Enthalpy of reaction from Standard Enthalpies of Formation

What is meant by the standard state of a substance?

(a) Why does the standard enthalpy of formation of both the
very reactive fluorine 1F22 and the almost inert gas nitrogen
1N22 both read zero?

Write balanced equations that describe the formation of the
following compounds from elements in their standard states,
and then look up the standard enthalpy of formation for
each substance in Appendix C: (a) CH3OH(l)

Ibuprofen is used as an anti-inflammatory agent used to deal with pain and bring down fevers. If it has a molecular formula of C13H­18O2, determine the balanced chemical equation that would give you directly the enthalpy of formation for ibuprofen.&nbsp;

Write balanced equations for the formation of the following compounds from their elements. (b) Sodium sulfate

What is the phase of the standard states of the following ele- ments and compounds?
(a) NH3 (b) Fe (c) N2 (d) Br2

How is the standard state of an element defined? Why do
elements always have ∆H°f = 0?

Write an equation for the formation of each compound from 
its elements in their standard states, and find ΔH °rxn for each in 
Appendix IIB. 
d. CH3OH(l )

Write an equation for the formation of each compound from
its elements in their standard states, and find ΔH °rxn for each in
Appendix IIB.
b. MgCO3(s)

Write balanced equations for the formation of the following compounds from their elements.
(b) Sucrose (table sugar, C12H22O11)

For each of the following compounds, write a balanced thermochemical 
equation depicting the formation of one mole 
of the compound from its elements in their standard states 
and then look up H °f for each substance in Appendix C. 
(b) SO31g2

Elements can exist as solids, liquids or gases at 25ºC and 1 atm standard pressure.

Write balanced equations for the formation of the following compounds from their elements.
(c) Uranium hexafluoride (a solid at 25 °C)

What phase of matter is associated with the standard states of the following elements and compounds? (a) Cl2 (b) Hg (c) CO2 (d) Ga

Identify a substance that is not in its standard state.

Which of the following represents the formation equation for barium nitrate, Ba(NO3)2?

Formation Equations Example 1

Enthalpies of Formation - Chemsitry Tutorial

What is Enthalpy of Formation?

Write balanced equations for the formation of the following compounds from their elements. (c) Dichloromethane (a liquid, CH2Cl2)

Formation Equations Example 2

5.7 Standard Enthalpies of Formation

Write balanced equations for the formation of the following compounds from their elements. (a) Ethanol (C2H6O)

(c) What is meant by the term standard
enthalpy of formation?

Write balanced equations for the formation of the following compounds from their elements.
(a) Iron(III) oxide

Write an equation for the formation of each compound from
its elements in their standard states, and find ΔH °f for each in
Appendix IIB.
a. NH3( g)

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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 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

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 -