By Jessica schneider
Using Stoichiometry is very simple . Here's and example using the reaction carbon and oxygen. Since this type of reaction is called synthesis. In synthesis you combine the two elements to make a compound. So using that information we can say that the balance equation is C + O yields to CO2
Finding molar mass is very easy to find all you need is a periodic table and sometimes a calculator. By using the periodic table I was able to find the molar mass of carbon (12.011) simply by looking at the atomic mass below the element symbol. Oxygen was different because I have two oxygen particles in the equation, so what I do is multiply 15.999 (molar mass of oxygen) times two which was 31.998. For carbon dioxide I add 12.011 and 31.998 and it equals 44.009
Mole to mole conversions
In this problem you would set up a big plus sign and put your given(from the question) in the top left hand corner. For example, if the question gave you 1.20 moles of Carbon and wants you to find out how many moles of Oxygen can you make you would put 1.2 moles of carbon in the top left hand corner. Next on the bottom right hand corner you will use coeficcients to change from element to element. So you will put a 1 in the bottom left hand corner since the coeficcient for Carbon is 1. In the top right hand corner you will put the coeficcient for oxygen(1)since you're solving for oxygen. The last step is to multiply by the top and divide by the bottom. Your answer should be 1.20 moles of oxygen.
Using the information from the video, and the given 12.1 g carbon find how many grams of CO2 can be made.
Your answer should be 44.34 g CO2
STOICHIOMETRY - Limiting Reactant & Excess Reactant Stoichiometry & Moles
For oxygen and CO2 and carbon and CO2 , oxygen is the limiting reactant and carbon is the excess.
Theoretical yield and limiting reactants can get very confused,but of your remember that theoretical is a number and that a limiting reactant is a element or compound you'll be fine. In the equation above the theoretical yeild is 16.91 g 02
Percent yield refers to the efficiency of a chemical reaction defined as the actual yield/theoretical yield x 100. theoretical yield. The amount of product that could possibly be produced in a given reaction, calculated according to the starting amount of the limiting reagent. In the equation the percent yield is 82.97%