Today we learned about Limiting Reactions.
What is limiting reactions you may ask?
In Chemical reactions, usually one chemical gets used up first before the other, right? The Chemical used up first in a chemical reaction is called the limiting reactant (reagent).
Once it is used up, the reaction comes to a hold! Limiting reactants determines the quantity of products formed.
QUESTION: So how do we find the limiting reactants in a chemical equation?
ANSWER: To find the Limiting Reactant, assume one reactant is used up. Determine how much of this reaction is required!
kk... you ready?
Question: Nitrogen gas reacts with Hydrogen gas to produce ammonia. How many moles of Ammonia are produced when 0.65 moles of nitrogen gas react with 0.45 moles of hydrogen gas?
Balanced Chemical equation: N2+3H2 ---> 2NH3
N2= 28.0 g/mol
H2= 2.0 g/mol
NH3= 17.0 g/mol
REMEMBER= WHAT YOU NEED
WHAT YOU HAVE
Gets it????????????
Now lets try some theoretical yield questions.
Theoretical yield is ACTUAL divided by THEORETICAL times by 100.
This will leave you with a percent, and the theoretical yield of a reaction is the amount of products that SHOULD be formed.
Question: Determine the percent yield for the reaction between 3.73 g of Na and excess O2 if 5.34 g of Na2O2 is recovered.
2Na+ O2---> Na2O2
It's actually very simple :) Here's a video if you need a little extra help! Watch it!
Post by Ren Flores
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