Exam 1 Review
Chapter 5 (5.6-5.7)
- What is Hess's Law? How can Hess's Law be used to determine enthalpies
for reactions which may be difficult or dangerous to perform?
- What are 'standard' conditions as far as reaction enthalpies go? What are the standard states
of the elements at 298K and 1 atm? (For example, hydrogen is H2(g), etc.)
- What is meant by a formation reaction for a compound?
- How are tabulated standard
heats of formation used to calculate standard enthalpies for reactions?
- Suggested problems: 5.60, 5.61, 5.63, 5.67, 5.69, 5.71
Chapter 10
- What are the characteristics of gases?
- How is pressure defined?
- How do we measure atmospheric pressure? What are the common units
used in measuring pressure? How do we convert between these units?
- How do we measure gas pressures in the lab?
- How is pressure related to volume at constant temperature and moles?
- How are moles and volume related at constant temperature and pressure?
- Be able to make and interpret sketches of P vs V and V vs T
- What is an ideal gas?
- What is the ideal gas law?
- What is the value of R, the gas constant (in liter-atm/mol-K)?
- What conditions are referred to as standard temperature and pressure?
- What is the combined gas law? For what types of transformations is it
useful?
- How do we rearrange the ideal gas law to find the density of an ideal gas?
- What is Dalton's law of partial pressures?
- How do we calculate partial pressures in terms of mole fractions?
- Given a balanced chemical equation, how do we calculate gas volumes of
products or reactants in a chemical reaction?
- What are the postulates of the kinetic-molecular theory of gases?
- How does the kinetic-molecular theory explain pressure?
- What is the absolute temperature of a gas a measure of?
- Do all of the gas molecules in a sample move at the same exact speed?
- How are kinetic energy and velocity related?
- Do two different gases at the same temperature have the same kinetic
energy?
- How does the rms speed of gas molecules depend on temperature? On mass?
- Under what conditions of temperature and pressure does the ideal gas law
break down?
- What is the van der Waals equation of state?
- What does the "b" constant in van der Waals equation correct for? What does
the van der Waals "a" constant correct?
- Given a, b, V and T, know how to calculate the pressure of a gas using both
the ideal gas law and van der Waals equation, and know how to explain the difference
between the results.
- Suggested problems: 10.9, 10.27, 10.31, 10.37, 10.41, 10.45, 10.47, 10.61, 10.67, 10.73,
10.77
Chapter 14
- What four factors affect the rate of a chemical reaction?
- How is the average rate of a chemical reaction defined?
- What are the typical units of a reaction rate?
- What is the difference between an average rate and an instantaneous rate?
- How is reaction rate related to stoichiometry?
- Be able to relate the rate of appearance/disappearance of any species in a
balanced chemical equation to the rate of appearance/disappearance of any other species.
- What is a kinetic rate law?
- In general, can we determine rate laws for stoichiometric reactions by looking at the balanced chemical equation?
- What is the difference between a rate law and a rate constant?
- How do we determine rate laws from experimental (i.e., intial rate) data?
- How do we calculate rate constants?
- What is meant by reaction order?
- What are the units of a first-order rate constant? A second or third order rate constant?
- What is the rate law for a first order reaction (e.g., A --> products?)
- What is the integrated first order rate law? What is it used for?
- A plot of _____ vs _____ is linear for a first order reaction, and the slope = ____
- How is the half-life for a first order reaction calculated?
- What is a second order reaction?
- What is the rate law for a second order reaction of the form 2A--> product?
- What is the integrated second order rate law?
- For a second order reaction, a plot of ____ vs _____ is linear with slope = ______
- What is the collision model of chemical reactions?
- What is the activation energy?
- What is an activated complex?
- Can you get a bottle of activated complex at the stockroom?
- Know how to draw and interpret energy profile diagrams
- What is meant by the mechanism of a reaction?
- What is an elementary step?
- What is meant by the molecularity of an elementary step?
- Be able to tell if an elementary step is unimolecular, bimolecular,
or termolecular
- What do the elementary steps in a multistep reaction mechanism have to add up to?
- How do we write rate laws for elementary processes?
- How do we determine rate laws for multistep mechanisms?
- Which step in a multistep mechanism is the rate-determining step?
- How do we deduce the rate law for a multistep mechanism for which the first
step is slow?
- When will intermediate appear in a rate law for an elementary step in a multistep mechanism?
- How and why do we assume equilibrium in a slow first step?
- How do we eliminate intermediates from rate laws using the assumption of equilibrium?
- Suggested problems: 14.1, 9, 11, 13, 17, 19, 23, 25, 27, 28, 31, 39, 43, 45,
53, 55, 57, 59, 87
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