Chemistry Lab

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Chemistry Lab
Chemistry & Lab Event
Forum Threads 2017 2016 2015 2014
2013 2012 2011 2010
Tests 2017 2016
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Question Marathons 2017 2016 2015
This event was not held last year in Division B
Division C Champion Acton-Boxborough Regional High School

Chemistry Lab is an event where participants must learn the respective year's selected aspects of chemistry and perform a lab or a set of labs regarding those topics.

Since this events rotates topics, each topic constitutes its own page. For topic-specific information, please see those pages, as this page only contains general information that applies to all topics.

Past topics:

Season Topic(s)
2006 Thermodynamics
2009 Acids and Bases, Titration Race
2010 Kinetics, Aqueous Solutions
2011 Electrochemistry, Aqueous Solutions
2012 Electrochemistry, Periodicity
2013 Equilibrium, Periodicity
2014 Equilibrium, Stoichiometry
2015 Kinetics, Stoichiometry
2016 Kinetics, Gas Laws
2017 Thermodynamics, Gas Laws


  • 1 or 2 people per team.
  • Eye protection #4.
  • Lab coat
  • 50 minutes.
  • 1 double-sided Note Sheets (one per student)
  • Non-programmable, non-graphing calculator & pencil

Chemistry Topics


The Merriam-Webster dictionary defines stoichiometry as "a branch of chemistry that deals with the application of the laws of definite proportions and of the conservation of mass and energy to chemical activity". Stoichiometry deals with calculations about the masses (sometimes volumes) of reactants and products involved in a chemical reaction. It is a very mathematical part of chemistry. The most common stoichiometric problem will present you with a certain amount of a reactant and then ask how much of a product can be formed. Ex:: [math]2A + 3B \to 3C[/math], Given 25 grams B and unlimited A how much C will be produced. This is called a mass-mass problem. These problems can be solved in 4 simple steps.

  1. Make sure the chemical equation is correctly balanced.
  2. Using the molar mass of the given substance, convert the mass given in the problem to moles.
  3. Construct a molar proportion (two molar ratios set equal to each other) following the guidelines set out in other files. Use it to convert to moles of the unknown.
  4. Using the molar mass of the unknown substance, convert the moles just calculated to mass.

Other forms of stoichiometric problems are finding the limiting reactant and finding the percentage composition. You can find out more about these in the links below.

The process is very similar when given gases (using the ideal gas law), solutions (using molarity) or molecules (using Avogadro's number)

Stoichiometry can be approached in precisely the same way one would approach dimensional analysis. And, when in doubt, convert to moles.

Reaction Types

There are five main types of reactions (single displacement, double displacement, combustion, decomposition, and synthesis). Each of them has a specific form that they take. If you encounter problems dealing with reactions on the test, knowing the basic types can be very helpful because then you will be more likely to see the pattern and understand how to complete the reaction.

Single Displacement

An example of a single replacement reaction. Here, copper reacts in silver nitrate solution to form copper nitrate solution and silver metal. The copper nitrate solution is visible since copper cations are blue in solution.

Also called single replacement reactions. Single displacement reactions are oxidation-reduction reactions in which an element and a compound react to form another element and a compound. This reaction takes on the form

[math]A + BC \to AC + B[/math]

So the lone elemental reactant, A, forms a compound with C, forcing B out to become an element itself. In order for this to occur, A and B are usually metals that form a cation when compounded with C.

The direction in which the reaction proceeds depends on each element's position in the activity series. A has to be more likely to oxidize than B, because otherwise B will just simple stay in solution and A will remain untouched.

Double Displacement

Double displacement reactions are similar to single replacement, but they are usually not oxidation-reduction reactions. Instead of just one element being traded, double displacement reactions have two similarly formed compounds reacting to form other compounds.

[math]AB + CD \to AD + CB[/math]

This type of reaction is especially important in aqueous solutions, since most precipitation reactions are double displacement reactions. Precipitation occurs when AB and CD are both soluble in water, and when put together, either AD or BC is an insoluble compound and thus precipitates out of the solution. For more information about solubility, see Chem Lab/Aqueous Solutions.


Combustion reactions are redox reactions that produce fuel. Thus, combustion reactions are also exothermic reactions since they give off heat. The most common combustion reactions form carbon dioxide, water, and energy. For example, here is the combustion reaction for methane:

[math]CH_4 + 2O_2 \to CO_2 + 2H_2O + energy[/math]

Combustion can also occur with nitrogen instead of carbon. There is also combustion with only hydrogen and oxygen, and in this case only water forms as product.

[math]2H_2 + O_2 \to 2H_20 + energy[/math]

Since combustion reactions are among the most common exothermic reactions, it is a good idea to know the combustion reactions of several important compounds, or at least know how to go about finding it quickly. Since all of them have a similar form, you can guess what the products will be, which will make it easier. For example, for the combustion of a hydrocarbon in oxygen, the two products will be water and carbon dioxide, since the oxygen attaches itself to both carbon and hydrogen parts.


In decomposition, a compound decomposes into its constituent parts.

[math]AB \to A + B[/math]

This type of reaction usually occurs when the compound AB is unstable, since breaking a chemical bond requires energy. Since it takes energy to break a bond, the vast majority of decomposition reactions are endothermic.


Synthesis reactions are the opposite of decomposition reactions. These reactions have two elements or components bonding together to form a larger compound.

[math]A + B \to AB[/math]

Since this reaction forms a bond, it is exothermic.

Oxidation and Reduction

Main article: Chem Lab/Electrochemistry.

To remember Oxidation and Reduction just remember these simple acronym OIL RIG. Oxidation is Loss, Reduction is Gain. This is a simple way of remembering that whatever is oxidized loses electrons and whatever is Reduced gains electrons. The phrase LEO the lion says GER also works (Lose Electrons-Oxidation, Gain Electrons-Reduction)

Aqueous Solutions

Main article: Chem Lab/Aqueous Solutions.

An aqueous solution is a solution where the solute is dissolved in water.


Main article: Chem Lab/Equilibrium.


Main article: Chem Lab/Periodicity.

Periodicity refers to the pattern of physical and chemical properties in the periodic table. These patterns are referred to as periodic trends. For example, one periodic trend is that the atomic radius of an element increases as one moves down a group, and leftward on a period.


Main article: Thermodynamics.

Acids and Bases

Main article: Chem Lab/Acids and Bases


Main article: Chem Lab/Titration Race

Gas Laws

Main article: Chem Lab/Gas Laws

Event Strategy

Like all events, Chem Lab requires a strategy for you to be able to do your best.

  • It is very helpful if one or both partners has taken AP Chemistry, since some of the topics covered in this event are advanced and not covered in normal high school chemistry classes.
  • Try to split the work between you and your partner so that in studying, you can cover both topics.
  • If you get a longer test, ask if you can remove the staple and split the test, so that you can cover more of the test in less time.
  • Try to arrange your team so that you have one person who is good at quickly performing labs and one person who is good at computations and writing. This should facilitate the labs.
  • Make sure to work not just quickly, but efficiently, on the labs. Do them as quickly as you can, but if you end up with inaccurate results then going quickly didn't help you a whole lot. Also, do not take shortcuts unless you are absolutely, positively sure you can.
  • Make sure you have all of your protective equipment, as you may be disqualified if you do not have it.