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Lecture Comments (15)

0 answers

Post by Yisrael Harris on May 21, 2013

The additional examples are visible only in expanded view, FYI.

5 answers

Last reply by: Tope Adedolapo
Thu Feb 23, 2017 11:49 AM

Post by charles adames on February 19, 2012

please stay on topic- there is a probability of a large number of students who use this website for help have problems focusing in class lectures because professors jump from topic to topic; you seem like a god instructure, considering the prevues videos, but refrain from bringing up in between topics, or side notes so you dont get the viwer lost. this is very important, because students have a limited amount of time to go over the material specially for some of us who attend an elite college but have problems with a particular subject- this lecture could have been shorten a bit more.

1 answer

Last reply by: rachel brower
Thu Jan 26, 2012 6:20 PM

Post by Lisa Ruszkiewicz on June 8, 2011

In example 2 the calculations are incorrect. (24.0 g Cl2* 266.68 g ALCL3) / 212.7g cl2 does not equal 32.6 g. It equals 30.09 g, unless there is something missing from the equation that was not written.

CL2 is still the limiting reagent, but having correct math is important

0 answers

Post by Michael Kirland on March 9, 2011

How do you make the measurement c21 h30 o2 in liquid measures?

1 answer

Last reply by: Zachary McCoy
Fri Jan 3, 2014 10:49 PM

Post by John Smith on November 1, 2010

I was always told that you MUST always add state symbols for all chemicals in a chemical reaction.

2 answers

Last reply by: Zachary McCoy
Fri Jan 3, 2014 10:48 PM

Post by Warren Thomas on August 11, 2010

I wish he would explain how he took adding al + cl2 from the question and changed it to 2al + 3cl2 = alcl3. Why is it 2al instead of just al? Why is it 3cl2 instead of just cl2? Where does the extra cl come from? The left side has cl2 and the right side has cl3.

Am I missing something?

Related Articles:

Balancing Equations, Limiting Reagents, Percentage Yield

  • Chemical equations show what happens in a reaction

  • Equations must be balanced in numbers and kinds of atoms

  • Practice balancing equations including complete combustion of C, H, O compounds in oxygen: products are carbon dioxide and water.

  • Use balanced chemical equations and moles to calculate relative masses of compounds that react: called stoichiometry

  • Redox: type of reactions where electrons are lost (ox or oxidation) or gained (red or reduction)

  • Reactions may be run where amounts of reagents aren’t exactly according to stoichiometry; there may be a reagent that limits amount of product – limiting reagent

  • Percentage yield of any reaction is based on limiting reagent and = actual yield/theoretical yield x 100%

Balancing Equations, Limiting Reagents, Percentage Yield

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

  • Intro 0:00
  • Balancing Chemical Equations 0:49
    • Atoms and Charges
    • Example: Mercury and Oxygen
    • Example: Combustion of a Hydrocarbon
  • Redox: Oxidation and Reduction 12:30
    • Example: Sodium and Chlorine
    • Electron Transfer
  • Limiting Reagent 22:25
    • Example: Nuts and Bolts
    • Example: Mercury and Oxygen
  • Reaction Formulas 32:03
    • Example: Iron Oxide and Carbon
    • Example: Benzene and Chlorine
  • Theoretical Yields, Actual Yields 42:13
    • Percentage Yield
    • Example
    • Theoretical Yield from Limiting Reagent
    • Example: Benzene and Chlorine
  • Additional Example 1
  • Additional Example 2