CHEM 113 completes UMGC's two-course general chemistry sequence for science majors, shifting from what reacts to how fast and how far.
UMGC describes it as an exploration and application of chemical reactions, with topics including chemical kinetics; homogeneous, heterogeneous and ionic equilibria; oxidation-reduction reactions; electrochemistry; and chemistry of the elements. It carries 4 credits, fulfills the laboratory science requirement and requires CHEM 103 or CHEM 105.
Equilibrium is where many students stall. The maths is algebra, but setting up the problem correctly takes practice.
Course at a Glance
| Item | Details |
|---|---|
| University | University of Maryland Global Campus (UMGC) |
| Course code | CHEM 113 |
| Credits | 4; fulfills the laboratory science requirement |
| Prerequisite | CHEM 103 or CHEM 105 |
| Credit overlap | Credit for only one of CHEM 113 or CHEM 115 |
| Typical work | Problem sets, lab reports, quizzes and exams |
What CHEM 113 Covers
| Topic (UMGC) | Key question |
|---|---|
| Chemical kinetics | How fast does a reaction go, and what controls the rate? |
| Homogeneous and heterogeneous equilibria | How far does a reaction go before it balances? |
| Ionic equilibria | Acids, bases, buffers and solubility |
| Oxidation-reduction reactions | Which species gains or loses electrons? |
| Electrochemistry | How redox reactions produce or use electricity |
| Chemistry of the elements | Patterns in the properties and reactions of elements |
Key Concepts Explained
Rate Laws
A rate law links rate to concentrations: rate = k[A]m[B]n. The orders m and n come from experiment, not from the balanced equation.
Example: Doubling [A] while holding [B] constant doubles the rate, so the reaction is first order in A. Doubling [B] with [A] constant quadruples the rate, so it is second order in B. Rate = k[A][B]2, third order overall.
Equilibrium and ICE Tables
An equilibrium constant K expresses product and reactant concentrations at balance. ICE tables (initial, change, equilibrium) organize the algebra.
Example: For A gives 2B with K = 4.0 and [A] starting at 1.0 M: at equilibrium [A] = 1.0 - x and [B] = 2x, so 4x2 / (1.0 - x) = 4.0. Solving x2 + x - 1 = 0 gives x about 0.62, so [A] is about 0.38 M and [B] about 1.24 M.
Le Chatelier's Principle
When a system at equilibrium is disturbed, it shifts to partly offset the change. Adding reactant pushes it towards products; raising temperature favors the endothermic direction.
Galvanic Cells
In a galvanic cell, oxidation happens at the anode and reduction at the cathode. The cell potential is E(cathode) minus E(anode), using standard reduction potentials; a positive value means the reaction is spontaneous.
Typical Assignments and How to Approach Them
| Assignment type | What it tests | How to approach it |
|---|---|---|
| Kinetics problems | Rate laws and orders from data | Compare experiments where only one concentration changes |
| Equilibrium problems | K expressions and ICE tables | Write K first, then fill the table |
| Redox and electrochemistry | Balancing half-reactions, cell potentials | Balance electrons before combining half-reactions |
| Lab reports | Data analysis and interpretation | Show graphs or calculations that support conclusions |
How the Topics Connect
CHEM 113's topics look separate but share one theme: predicting the behavior of reactions. Kinetics tells you how fast; equilibrium tells you how far; redox and electrochemistry apply both to electron-transfer reactions. Ionic equilibria apply equilibrium ideas to acids, bases and solubility.
Seeing these links helps on exams, where a single question may combine them, such as a redox reaction's equilibrium constant or how a buffer resists pH change.
Balancing Redox Reactions
Redox questions are a large part of CHEM 113. The half-reaction method keeps them manageable: split the reaction into oxidation and reduction, balance atoms other than O and H, balance O with water and H with H+ (in acid), then balance charge with electrons. Multiply so electrons cancel and add the halves.
Example: Zinc metal in copper(II) solution: Zn gives Zn2+ + 2e- (oxidation) and Cu2+ + 2e- gives Cu (reduction). Electrons already match, so the overall reaction is Zn + Cu2+ gives Zn2+ + Cu.
Where Students Get Stuck
- Taking orders from coefficients. Orders come from data.
- Including solids in K. Pure solids and liquids are left out.
- Unbalanced electrons in redox. Electrons lost must equal electrons gained.
- Anode and cathode mix-ups. Remember: oxidation at the anode, reduction at the cathode.
Study Tips for CHEM 113
- Practice ICE tables until the setup is automatic.
- Keep a one-page sheet of rate law and equilibrium rules.
- Draw every galvanic cell, labeling electron flow.
- Review CHEM 103 stoichiometry if calculations feel shaky.
How We Help with CHEM 113
Send the problems, lab instructions and data, rubric and feedback. A chemistry tutor can prepare worked solutions, explain concepts or review your lab report. Our lab report writing guide covers structure.
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Frequently Asked Questions
CHEM 103 or CHEM 105.
4 credits, and it fulfills the laboratory science requirement.
UMGC allows credit for only one of CHEM 113 or CHEM 115.
Many students find equilibrium setups and redox balancing hardest. Structured practice helps.
Yes. UMGC describes the CHEM 103 and CHEM 113 sequence as for students majoring in a science.
Yes. We set out the K expression and ICE table and explain each step.