Portland Community College | Portland, Oregon

Upon successful completion of the course, students should be able to:

1. Apply stoichiometry to a variety of problems involving reactions, gases, liquids, solutions, thermochemistry, kinetics, and equilibrium expressions.
2. Apply kinetic molecular theory and gas laws to predict the behavior of gases at various conditions.
3. Identify types of intermolecular forces and apply them to physical properties of solids, liquids, and solutions.
4. Describe solution concepts and factors affecting solution properties.
5. Determine the effects of different factors on chemical reaction rates and examine the role of catalysis in modifying these rates.
6. Apply concepts of thermochemistry to explain thermal energy transfer and the energy changes that accompany chemical and physical changes.
7. Identify and apply appropriate equations related to gas laws, solutions, colligative properties, thermochemistry, kinetics, and equilibrium expressions.

Students will be able to..

1. Apply stoichiometry to a variety of problems involving reactions, gases, liquids, solutions, thermochemistry, kinetics and equilibrium expressions.

1a. Use solution stoichiometry to calculate the amounts of reactants and products for a given chemical equation (aqueous/solid, aqueous/aqueous, and aqueous/gas).

1b. Given a chemical equation in which one of the products is a gas, a mass of one of the reactants, the stipulation that the other reactants are in excess, and two of the following (P, T, or V) calculate the third.

2. Apply kinetic molecular theory and gas laws to predict the behavior of gasses at various conditions.

2a. Define pressure and state common units.

2b. Describe how gas pressure is measured.

2c. Rank gas particles in terms of urms or rate of effusion.

2d. Given the ideal gas constant and any three of the four following data (volume, pressure, temperature, and amount), calculate the fourth.

2e. Given the total pressure of a gas mixture and the mole fractions, determine the partial pressure of each gas in the mixture.

2f. Explain a macroscopic level observation about gases based on particle level behavior.

2h. Explain the difference between a real and ideal gas.

3. Identify types of intermolecular forces and apply them to physical properties of solids, liquids and solutions.

3a. Identify the intermolecular forces present in a pure sample of a given compound.

3b. Determine if a hydrogen bond can form between two given molecules and draw the resulting interaction.

3c. Predict the solubility of two molecular compounds based on their intermolecular forces. 

3d. Discuss the origin of the following intermolecular forces  in terms of electrostatics (dipole-dipole, ion-dipole, dispersion, H-bonding, and dipole-induced dipole).

3e. Define vapor pressure and describe the effects of changing temperature, volume of the container and the amount of liquid.

3f. Given the molecular structure of several compounds, put them in increasing order of physical properties such as boiling point, melting point and vapor pressure.

3g. Label the phases, triple point, and critical point on a blank pressure-temperature phase diagram for a pure substance.

3h. Identify the phase transitions associated with movement from one region of a blank temperature-pressure phase diagram to another.

4. Describe solution concepts and factors affecting solution properties.

4a. Rank solutions of given concentrations in order of increasing or decreasing osmotic pressure, boiling point, or vapor pressure.

4b. Given two aqueous solutions of ionic compounds, predict the solubility of the resulting products with a solubility table.

4c. Write a total and net ionic equation that describes the reaction between two aqueous compounds.

5. Determine the effects of different factors on chemical reaction rates and examine the role of catalysis in modifying these rates.

5a. Define the rate of reaction in terms of the rate of disappearance of reactants and appearance of products.

5b. Identify and compare and contrast: instantaneous rates, average rates and initial rates from a plot of concentration versus time.

5c. Given initial concentrations and initial rates for multiple trials of a reaction, write the rate law for the reaction.

5d. Given a first order reaction, the integrated rate law, and any three of the four following data (initial concentration, final concentration, time, and rate constant), solve for the fourth. 

5e. Discuss how a catalyst affects a chemical reaction.

5f. Given a multi-step mechanism for a reaction, identify any catalysts or intermediates. 

5g. Given a two-step mechanism for a reaction with one step identified as the slow step, determine the observed rate law for the overall reaction.

5h. Given a balanced chemical equation and the forward and reverse rate constants, construct an appropriate reaction coordinate diagram.

5i. Given a set of data of the rate constant for a reaction at different temperatures, generate an appropriate, correctly labeled Arrhenius plot of ln k vs. 1/T to determine the best fit line and compute the activation energy and frequency factor, A, with appropriate units.

5j. Given the necessary set of the following values (k, Ea T, R) for a given reaction, utilize a given Arrhenius equation (either exponential or linear form) to determine one of the variables if the remaining are given.

6. Apply concepts of thermochemistry to explain thermal energy transfer and the energy changes that accompany chemical and physical changes.

6a. For a thermodynamic process define the system and the surroundings.

6b. Define the internal energy as the sum of kinetic and potential energy.

6c. Given a system, apply the 1st Law of Thermodynamics to calculate the internal energy change based on the heat transferred and/or work done.

6d. Identify reactions in which the change in internal energy is equal to the change in enthalpy.

6e. Given any three of the four following data (specific heat capacity, mass, temperature change or heat), calculate the fourth.

6f. Given the melting point, boiling point, enthalpy changes associated with phase changes, and specific heats of the respective phases, calculate the heat needed to warm or cool a material from one temperature to another through a phase change.

6g. Given a balanced chemical equation and the enthalpy change associated with that equation, calculate the heat consumed or evolved when a certain mass of one of the reactants completely reacts.

6h. Write the balanced chemical equation associated with the standard enthalpy of formation for a given compound.

6i. Given a balanced chemical equation and a table of standard enthalpies of formation and bond dissociation energies, calculate the standard enthalpy change associated with the reaction.

6j. Give examples of properties that are state functions.

6k. Use Hess’s law to calculate the enthalpy change of a balanced chemical equation that can be derived from a given set of balanced chemical equations and their respective enthalpy changes.

6l. Identify if a physical or chemical change is endo- or exothermic and draw a corresponding energy diagram.

6m. Categorize bond breaking and bond formation as an endo- or exothermic process.

7. Identify and apply appropriate equations related to gas laws, solutions, colligative properties, thermochemistry, kinetics and equilibrium expressions.

7a. Calculate changes in boiling point, freezing point, and vapor pressure using colligative property equations.

7b. Apply knowledge of colligative properties to describe the phenomenon on a particle level.