Christopher Nilsen

Columbia University in the City of New York
Teacher of Chemistry

Biography

Why did that test tube get hot? How did two clear solutions produce a blue solid? What’s happening at the molecular level? These types of questions inspired me to earn my B.S. and M.S. degrees in Chemical Engineering and Applied Chemistry at Columbia University.

After spending a decade in the pharmaceutical industry, I wanted to find ways to get more people interested in science and engineering. Teaching and tutoring were two solutions - no pun intended! So for the past 13 years, I've been teaching all levels of HS chemistry and have served as an advisor and coach of Chemistry Olympics and Robotics teams.

Since much of chemistry is based at the molecular level, it can be difficult for students to visualize and understand. I excel at finding ways to explain concepts that seem very abstract to students by returning to basic concepts and building knowledge in chemistry’s language (formulas and equations) and its visuals (diagrams and graphs). Together we’ll build your confidence and reduce your fear of chemistry!

Education

MS Chemical Engineering and Applied Chemistry
Columbia University in the City of New York
BS Chemical Engineering
Columbia University in the City of New York

Educator Statistics

Numerade tutor for 5 years
2070 Students Helped

Topics Covered

Atoms, Molecules, and Ions: Understanding the Building Blocks of Matter
Understanding Electronic Structure: A Comprehensive Guide
Understanding Chemical Bonding: The Key to Molecular Structure
Unlocking the Power of Thermodynamics: A Comprehensive Guide
Energy of a System
Energy in Thermal Processes
Understanding Acids and Bases: A Comprehensive Guide
Aqueous Solutions
Understanding Chemical Equilibrium: A Comprehensive Guide
Explore the Fascinating World of Nuclear Chemistry
Mastering Chemical Reactions and Stoichiometry for Optimal Results
Effective Solutions for Your Business Needs
Unlocking the Power of Composition: Tips and Techniques
Unlocking the Power of Periodic Table Properties | Boost Your Knowledge
Discover the Power of Liquids: Boost Your Health and Wellness Today!
Acid-Base Equilibria: Understanding the Balance
Discover the Wonders of Chemistry: Your Introductory Guide
Discover the Power of Gases: Benefits and Applications
Unlocking the Power of Chemical Reactions: A Comprehensive Guide
Explore the Fascinating World of Molecular Geometry - Discover More!
Exploring the Fascinating World of Thermochemistry | Learn More Today
Discover the Power of Solids for Your Everyday Needs
Understanding Structure and Bonding: A Comprehensive Guide
Unlocking the Wonders of Organic Chemistry: An Introduction

Christopher's Textbook Answer Videos

04:12
Chemistry: Structure and Properties

The propane fuel (C3H8) used in gas barbeques burns according to a thermochemical equation:

If a pork roast must absorb 1.6 * 103 kJ to fully cook, and if only 10% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?

Chapter 9: Thermochemistry
Christopher Nilsen
04:26
Chemistry: Structure and Properties

The lattice energy of CsF is -744 kJ>mol whereas that of BaO is-3029 kJ>mol. Explain this large difference in lattice energy.

Chapter 9: Thermochemistry
Christopher Nilsen
01:51
Chemistry: Structure and Properties

Write a balanced equation for the photosynthesis reaction in which gaseous carbon dioxide and liquid water react in the presence of chlorophyll to produce aqueous glucose (C6H12O6) and oxygen gas.

Chapter 7: Chemical Reactions and Chemical Quantities
Christopher Nilsen
07:40
Chemistry: Structure and Properties

Write a balanced chemical equation for each reaction.
a. Solid copper reacts with solid sulfur to form solid copper(I) sulfide.
b. Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.
c. Sulfur dioxide gas reacts with oxygen gas to form sulfur trioxide gas.
d. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.

Chapter 7: Chemical Reactions and Chemical Quantities
Christopher Nilsen
03:24
Chemistry: Structure and Properties

A piece of dry ice (solid carbon dioxide) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the carbon dioxide ends up in the balloon, what is the volume of the balloon at a temperature of 22 C and a pressure of 742 mmHg?

Chapter 10: Gases
Christopher Nilsen
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Christopher's Quick Ask Videos

07:40
Chemistry 101

Write a balanced chemical equation for each reaction.
a. Solid copper reacts with solid sulfur to form solid copper(I) sulfide.
b. Solid iron(III) oxide reacts with hydrogen gas to form solid iron and liquid water.
c. Sulfur dioxide gas reacts with oxygen gas to form sulfur trioxide gas.
d. Gaseous ammonia (NH3) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water.

Christopher Nilsen
01:50
Chemistry 101

Write a balanced equation for the photosynthesis reaction in which gaseous carbon dioxide and liquid water react in the presence of chlorophyll to produce aqueous glucose (C6H12O6) and oxygen gas.

Christopher Nilsen
07:58
Chemistry 101

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.
a. 2 K(s) + Cl2(g)-2 KCl(s)
b. 2 K(s) + Br2(l)-2 KBr(s)
c. 4 Cr(s) + 3 O2(g)-2 Cr2O3(s)
d. 2 Sr(s) + O2(g)-2 SrO(s)

Christopher Nilsen
08:56
Chemistry 101

Many computer chips are manufactured from silicon, which occurs in nature as SiO2. When SiO2 is heated to melting, it reacts with solid carbon to form liquid silicon and carbon monoxide gas. In an industrial preparation of silicon, 155.8 kg of SiO2 reacts with 78.3 kg of carbon to produce 66.1 kg of silicon. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

Christopher Nilsen
09:51
Chemistry 101

Determine whether or not each reaction is a redox reaction. For each redox reaction, identify the oxidizing agent and the reducing agent.
a. Al(s) + 3 Ag+(aq)-Al3+(aq) + 3 Ag(s)
b. SO3(g) + H2O(l)-H2SO4(aq)
c. Ba(s) + Cl2(g)-BaCl2(s)
d. Mg(s) + Br2(l)-MgBr2(s)

Christopher Nilsen
05:21
Chemistry 102

Pick the compound with the highest boiling point in each pair.
Explain your reasoning.
a. NH3 or CH4
b. CS2 or CO2
c. CO2 or NO2

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