Exam 2 Study Guide: Learning Objectives for Chapters 4, 5, and 6

Comprehensive practice flashcards formatted as questions and answers covering study strategies, chemical reaction types, gas laws, and thermochemistry from the Exam 2 Study Guide.

According to the study guide, what action should students take for any learning objective they rate as a 1 or a 2?

Focus on studying those learning objectives and practice more problems found in the end-of-chapter problems in the textbook.

How is a rating of 4 defined on the learning objective self-assessment scale?

"I can explain it and solve problems independently, even when the wording changes."

How are ratings of 1, 2, and 3 defined on the learning objective self-assessment scale?

1 = "I do not yet understand this learning objective."; 2 = "I recognize the concept but cannot reliably solve problems on my own."; 3 = "I can solve most problems but occasionally need help."

What are the two primary components that make up a solution in Chapter 4?

Solute(s) and solvent.

What three electrolyte categories must students be able to distinguish and identify from a list of compounds?

Strong electrolytes, weak electrolytes, and non-electrolytes (nonelectrolytes).

What concentration unit and associated calculation type are highlighted in Chapter 4 Learning Objective 3?

Molarity and calculations related to dilution.

What tool must students memorize to predict whether a precipitate will form in a reaction?

The solubility rules.

What two types of ionic equations must students be able to write for precipitation and acid/base reactions?

Total ionic equation (TIE) and net ionic equation (NIE).

What are the three broad categories of reactions covered in Chapter 4?

Precipitation, Acid-Base, and Redox (which has subcategories).

What four key terms must students be able to define and identify in a redox reaction?

Oxidation, reduction, oxidizing agent, and reducing agent.

What are students required to know regarding complete combustion reactions?

The reactants and products of a complete combustion reaction, and how to complete and balance this type of reaction.

What four properties are used to describe any sample of gas in Chapter 5?

Pressure, volume, amount, and temperature.

What two measuring devices are mentioned in Chapter 5 for measuring pressure?

Barometers and manometers.

What two values can be calculated using rearrangements of the ideal gas law?

Density and molar mass.

What does the abbreviation STP stand for in Chapter 5?

Standard temperature and pressure.

Which law governs partial pressures, and what two specific examples of its application are cited in the study guide?

Dalton's Law of partial pressure; examples include the scuba example and the collection over water example.

Which law describes the relationship between the rate of diffusion or effusion of gases and their molecular mass?

Graham's law.

What equation is used to describe a gas system when the ideal gas law fails?

The van der Waals equation.

How is enthalpy related to heat transfer according to Chapter 6 Learning Objective 2?

Enthalpy is a state function that relates to heat at constant pressure.

From what perspective must heat transfer be related when defining a system and surroundings?

From the system-centered perspective.

What is the difference between endothermic and exothermic changes?

An endothermic change absorbs heat into the system, whereas an exothermic change releases heat from the system.

What are the three general methods used to calculate the change in enthalpy of a reaction ($\Delta H$)?

1. Calorimetry, 2. Standard heats of formation ($\Delta H_f$), and 3. Hess' Law.

What property indicates how much heat a substance absorbs per temperature change and is utilized in calorimetry calculations?

Specific heat capacity.

What thermodynamic condition must students know the defining criteria for according to Chapter 6 Learning Objective 9?

Standard State.