D870 Physical Chemistry I is part of WGU's secondary chemistry route. WGU describes the intersection of physics and chemistry: the principles governing chemical reactions and matter, covering atomic and molecular structure, thermodynamics and kinetics, with attention to real-world applications and practical problem-solving.
It is the most mathematical of the chemistry content courses. The challenge is choosing the right relationship for a situation and then explaining what a numerical result means for the reaction, not just calculating it.
Course at a Glance
| Item | Details |
|---|---|
| University | Western Governors University (WGU) |
| Course code | D870 |
| Level | Undergraduate, chemistry content |
| Subject area | Physical chemistry |
| Prerequisites | Check your degree plan |
| Assessment | Set by WGU on your course page; check it before you plan |
What D870 Covers
An earlier edition of WGU's guidebook lists physical chemistry competencies that match these themes. Confirm current details on your course page.
| Theme | What it means in practice |
|---|---|
| Atomic and molecular structure | How structure underlies chemical behavior |
| First law of thermodynamics | Heat and work in chemical processes and changes of state |
| Second law and free energy | Spontaneity and equilibrium |
| Real gases | Equations of state beyond the ideal gas |
| Kinetics | Rates, rate laws and mechanisms |
| Electrochemistry | Interchange of chemical and electrical energy |
Key Concepts Explained
Free Energy and Spontaneity
A process is spontaneous at constant temperature and pressure when the change in Gibbs free energy is negative: delta G = delta H - T delta S. Enthalpy and entropy can work together or oppose each other, and temperature decides the winner.
Example: A reaction has delta H = +40 kJ/mol and delta S = +0.150 kJ/(mol K). At 298 K, delta G = 40 - 298 x 0.150 = 40 - 44.7 = -4.7 kJ/mol, so it is spontaneous. At 250 K, delta G = 40 - 37.5 = +2.5 kJ/mol, so it is not. Temperature flips the result.
Rate Laws
The rate law links rate to concentrations, with exponents found from experiment, not from the balanced equation. For a first-order reaction, the half-life is constant and equals 0.693 / k.
Example: A first-order reaction has k = 0.0231 per minute. Half-life = 0.693 / 0.0231 = 30 min. After 90 minutes (three half-lives), one eighth of the starting material remains.
Equilibrium and the Reaction Quotient
Compare Q with K. If Q is less than K, the reaction shifts towards products; if Q is greater, towards reactants.
Typical Assignments and How to Approach Them
WGU's guidebook does not list task prompts. The table describes kinds of work this content points to. Follow your own instructions.
| Work type | What it tests | How to approach it |
|---|---|---|
| Thermodynamic calculations | Applying the laws | State the law, substitute, check sign and units |
| Kinetics analysis | Rate laws and mechanisms | Use data to find order, then k |
| Explanation of results | Mechanism over outcome | Say why, in terms of energy and rates |
| Applied scenario | Real-world links | Tie numbers to a practical situation |
A Study Approach That Works
- Secure the energy ideas. First law, enthalpy, entropy, free energy.
- Practice sign conventions. Heat in versus heat out is the classic trap.
- Learn kinetics by data. Determine order from tables before using formulas.
- Explain every result. Finish each calculation with a sentence on meaning.
Where Students Get Stuck
- Outcome without mechanism. Describing that a reaction goes is not enough; explain it thermodynamically or kinetically.
- Thermodynamics versus kinetics. A spontaneous reaction can still be slow.
- Units for R and k. Match them to the equation.
- Sign errors. Define heat flow direction in your first line.
Planning Table
| Stage | Goal | Evidence to keep |
|---|---|---|
| Read the task | List requirements | Rubric checklist |
| Choose the law | Match to situation | Formula line |
| Calculate | Substitute with units | Worked steps |
| Check | Sign and size | Sense check |
| Explain | State the meaning | Sentence |
Self-Check Questions
Test yourself with these prompts before you submit working.
- When is delta G negative, and how does temperature change that?
- What does the half-life of a first-order reaction tell you?
- How do you decide the order of a reaction from data?
- Why can a reaction be spontaneous yet slow?
- If Q is less than K, in which direction does the system shift?
Study Tips for D870
- Write the sign convention at the top of each solution.
- Keep a formula sheet with variable meanings and units.
- Convert kJ and J consistently.
- Use Kelvin for all temperature work.
- Explain every result in plain words.
How We Help with D870
Send the task instructions, the rubric and your working. A tutor can explain thermodynamics and kinetics with new numbers, check your steps, edit your explanations for clarity, or prepare a custom solution for you to study.
GradeEssays is independent of Western Governors University. Our work is a study and reference aid: use it to understand the method, then complete and submit your own work under WGU's academic integrity policy.
Orders are written from scratch, include free revisions within the scope of your original request, and are refunded in full if late. We cannot promise that any assessment will be passed.
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Frequently Asked Questions
WGU describes the intersection of physics and chemistry: atomic and molecular structure, thermodynamics and kinetics, with real-world applications.
WGU's description does not say. Be ready for algebra and logarithms at least; check your course materials.
Spontaneity is about free energy; speed depends on activation energy and the reaction mechanism.
Compare how the rate changes when a concentration changes, using the experimental data.
No. We provide tutoring, custom solutions and editing. You complete and submit your own work.
On your D870 course page and with your instructor. WGU sets the assessment.