Stephanie L

Saint Mary's College of California
Freelance general chemistry instructor

Biography

- Provide one-on-one sessions with clients (teens to adults), with up to 21 concurrent students per month
- Prepare curriculum and lesson plans for individual students
- Evaluate student needs and adapt teaching method to ensure maximum learning and growth
- Deliver high quality, efficient and productive sessions with a 5.0/5.0 rating from 653 ratings
- Total hours of tutoring: 1,620 hrs

Prior to this, I was teaching general chemistry at Penn State University

Education

BS Chemistry
Saint Mary's College of California
MS Analytical Chemistry
University of Michigan - Ann Arbor
Phd Chemistry
University of Michigan - Ann Arbor

Educator Statistics

Numerade tutor for 6 years
41 Students Helped

Topics Covered

Mastering Chemical Reactions and Stoichiometry for Optimal Results
Understanding Chemical Equilibrium: A Comprehensive Guide
Unlocking the Power of Composition: Tips and Techniques
Effective Solutions for Your Business Needs
Aqueous Equilibria: Understanding the Balance of Solutions
Understanding Electronic Structure: A Comprehensive Guide
Exploring the Fascinating World of Quantum Physics

Stephanie's Textbook Answer Videos

01:49
World of Chemistry

Elemental boron is produced in one industrial process by heating diboron trioxide with magnesium metal, also producing magnesium oxide. Write the unbalanced chemical equation for this process.

Chapter 7: Chemical Reactions: An Introduction
Section 2: Chemical Equations
Stephanie L
02:31
Introductory Chemistry

The _____ of a substance is the mass (in grams) of 1 mole of the substance.

Chapter 8: Chemical Composition
Section 5: Molar Mass
Stephanie L
01:25
Introductory Chemistry

In your own words, describe what Le Châtelier's principle tells us about how we can change the position
of a reaction system at equilibrium.

Chapter 17: Equilibrium
Section 7: Le Chatelier’s Principle
Stephanie L
02:03
Introductory Chemistry

Consider the reaction
$$2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{CO}_{2}(g)$$
Suppose the system is already at equilibrium, and then an additional mole of $\mathrm{CO}(g)$ is injected into the system at constant temperature. Does the amount of $\mathrm{CO}_{2}(g)$ in the system increase or decrease? Does the value of $K$ for the reaction change?

Chapter 17: Equilibrium
Section 7: Le Chatelier’s Principle
Stephanie L
01:59
Introductory Chemistry

For an equilibrium involving gaseous substances, what effect, in general terms, is realized when the volume of the system is decreased?

Chapter 17: Equilibrium
Section 7: Le Chatelier’s Principle
Stephanie L
02:58
Introductory Chemistry

What is the effect on the equilibrium position if an endothermic reaction is carried out at a higher temperature? Does the net amount of product increase or decrease? Does the value of the equilibrium constant change if the temperature is increased?

Chapter 17: Equilibrium
Section 7: Le Chatelier’s Principle
Stephanie L
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