Basically, it is coefficients in balanced equations which tells us the number of moles reacted or produced!
3x + Y ---> 2Z
*WHAT YOU NEED OVER WHAT YOU HAVE
Some examples:
If 0.16 mol of methane are consumed in a combustion reaction how many moles of CO2 are produced?
Let's start off by what we are given!
The formula for methane is CH4. We know that Combustion reactions produce Carbon Dioxide (CO2) and water (H2O)
So it will look like this: CH4 ---> Co2 + H2O
But we aren't finished here because since theres oxygen atoms on the right side, we must have oxygen atoms on the left side of the equation as well. Remember that Oxygen is diatomic so our new equation will look like this:
CH4 + O2 ---> CO2 + H20
Balance the equation and get:
CH4 + 2O2 ---> CO2 + 2H20
Given 0.15 mols, we are asked to find how many moles of CO2 are produced
0.15mol x what we need (Carbon Dioxide) over what we have already (methane).....
0.15 mol x 1CO2
1 CH4
= 0.15 mol of CO2
Do you get it? Kinda? Not really? Okay let's try some more!
How many moles of Aluminum Oxide are required to produce 1.8 mol of pure aluminum?
Note: Decomposition Reaction, Balance the Equation
2Al2O3 --> 4Al + 3O2
Given 1.8 mol, looking for Aluminum Oxide moles, given pure aluminum
1.8 mol x 2Al
4Al
= 0.90 mol of Aluminum Oxide
Lets do one last one than we're done I promise:
How many moles of hydrogen will be produced if 0.44 mol of CaH2 reacts according to the following equation?
CaH2+ 2 H2O --> Ca(OH)2 + 2H2
0.44mol x 2H
1Ca
= 0.88 mol
Nice work! Post by REN FLORES
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