Chapter 5 - Learning Goals

Thermochemistry

5.1 Give examples of different forms of energy.

5.2 List the important units in which energy is expressed and convert from one to another.

5.3 Define the first law of thermodynamics both in writing and
by means of an equation.

5.4 Describe how the change in internal energy of a system is
related to the exchanges of heat and work between the system
and its surroundings.

5.5 Define the term state function and describe its importance
in thermochemistry.

5.6 Define enthalpy, and relate the enthalpy change in a process occurring at constant pressure to the heat added to or lost
by the system during the process.

5.7 Sketch an energy diagram such as that shown in Figure 5.11
of the text, given the enthalpy changes in the processes involved,
and associate the sign of delta H with whether the process is exothermic or endothermic.

5.8 Calculate the quantity of heat involved in a reaction at constant pressure given the quantity of reactants and the enthalpy change
for the reaction on a mole basis.

5.9 Define the terms heat capacity and specific heat.

5.10 Calculate any one of the following quantities given the other
three: heat, quantity of material, temperature change, and
specific heat [Q = SW (deltaT)].

5.11 Calculate the heat capacity of a calorimeter, given the
temperature change, its quantity of water, and the quantity
of heat involved; also calculate the heat evolved or absorbed
in the process from a knowledge of the heat capacity of the
system, its quantity of water, and its temperature change . . .
Q total = (SW(deltaT)) H2O + Ccal(deltaT)

5.12 State Hess's Law, and apply it to calculate the enthalpy change
in a process, given the enthalpy changes in other processes that
could be combined to yield the reaction of interest.

5.13 Define and illustrate what is meant by the term standard state,
and identify the standard states for the elements carbon,
hydrogen, and oxygen.

5.14 Define the term standard heat of formation, and identify the
type of chemical reaction with which it is associated.

5.15 Calculate the enthalpy change in a reaction occurring at
constant pressure, given the standard enthalpies of formation
of each reactant and product.

5.16 Define the term fuel value; calculate the fuel value of a substance given its heat of combustion or estimate the fuel value of a
material given its composition.

You are responsible for all material discussed in Lecture and all material
contained in the text (unless otherwise indicated) whether or not it appears here.

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	5.1	Give examples of different forms of energy.

	5.2	List the important units in which energy is expressed and convert from one to another.

	5.3	Define the first law of thermodynamics both in writing and by means of an equation.

	5.4	Describe how the change in internal energy of a system is related to the exchanges of heat and work between the system and its surroundings.

	5.5	Define the term state function and describe its importance in thermochemistry.

	5.6	Define enthalpy, and relate the enthalpy change in a process occurring at constant pressure to the heat added to or lost by the system during the process.

	5.7	Sketch an energy diagram such as that shown in Figure 5.11 of the text, given the enthalpy changes in the processes involved, and associate the sign of delta H with whether the process is exothermic or endothermic.

	5.8	Calculate the quantity of heat involved in a reaction at constant pressure given the quantity of reactants and the enthalpy change for the reaction on a mole basis.

	5.9	Define the terms heat capacity and specific heat.

	5.10	Calculate any one of the following quantities given the other three: heat, quantity of material, temperature change, and specific heat [Q = SW (deltaT)].

	5.11	Calculate the heat capacity of a calorimeter, given the temperature change, its quantity of water, and the quantity of heat involved; also calculate the heat evolved or absorbed in the process from a knowledge of the heat capacity of the system, its quantity of water, and its temperature change . . . Q total = (SW(deltaT)) H2O + Ccal(deltaT)

	5.12	State Hess's Law, and apply it to calculate the enthalpy change in a process, given the enthalpy changes in other processes that could be combined to yield the reaction of interest.

	5.13	Define and illustrate what is meant by the term standard state, and identify the standard states for the elements carbon, hydrogen, and oxygen.

	5.14	Define the term standard heat of formation, and identify the type of chemical reaction with which it is associated.

	5.15	Calculate the enthalpy change in a reaction occurring at constant pressure, given the standard enthalpies of formation of each reactant and product.

	5.16	Define the term fuel value; calculate the fuel value of a substance given its heat of combustion or estimate the fuel value of a material given its composition.