Posts tagged CU Boulder
Chemical Equilibrium - ICE Tables
  • When a reaction is allowed to ‘run’ for some time, at some point it will no longer be favorable to continue forward or reverse and it will be at equilibrium

  • It is important to remember that equilibrium does not mean that the reactant concentrations and the product concentrations are equal, but that the rate of the forward reaction is equal to the rate of the reverse reaction until something were to change (add more reactants/products, temperature, etc.)

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The electrochemistry unit at CU begins with redox reactions. Make sure you understand the basics of this before continuing through this article.

A voltaic cell, a.k.a. a galvanic cell, requires several parts. In official terms, you’ll need a cathode, an anode, and a conductive substance (usually wire) and salt bridge connecting the two. Less formally, you’ll need

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Organizing Functions

While meeting with students in beginner level CSCI courses I have noticed a fairly common theme, many students are just typing code into a file with little to no organization. By the end of the project their code is so messy that the flow is almost impossible to follow. Because of this I have put together a simple set of rules for keeping your functions ordered.

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E2 Reactions

Elimination reactions are helpful in many situations, especially in synthesis when you have an alkane and need an alkene. Similar to substitution reactions, eliminations produce similar products but depend on different factors. Most notably, E1 reactions have a carbocation intermediate while E2 reactions do not (for more information on E1 reactions, see “SN1/E1 Reactions”). 

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