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# Limiting reactants and empirical formulae

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## Harvey Buckle

on 23 March 2016

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#### Transcript of Limiting reactants and empirical formulae

Aim
To know how to calculate the empirical formula
To know the significance of limiting reactants
Empirical formula
Watch the demonstration and perform the calculations

Mass magnesium = 2.39 g
Mass magnesium oxide = 3.78 g
Limiting reactant
Limiting Reactant - The reactant in a chemical reaction that limits the amount of product that can be formed. The reaction will stop when all of the limiting reactant is consumed.
Excess Reactant - The reactant in a chemical reaction that remains when a reaction stops when the limiting reactant is completely consumed. The excess reactant remains because there is nothing with which it can react.

Example Limiting Reactant Calculation:

A 2.00 g sample of ammonia is mixed with 4.00 g of oxygen. Which is the limiting reactant and how much excess reactant remains after the reaction has stopped?
And so...
Now...have a go at some calculations
Starter
If 11g of Carbon is reacted with 32g of Oxygen. How many moles of Carbon dioxide are made?
Solution
First, we need to create a balanced equation for the reaction:

4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)

Next we can use stoichiometry to calculate how much product is produced by each reactant. NOTE: It does not matter which product is chosen, but the same product must be used for both reactants so that the amounts can be compared.

Limiting reactants and empirical formulae
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