M5 - excess reactant
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M5 - excess reactant
For M5 in the textbook, why is BrF3 the excess reactant and not the limiting reactant?
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Re: M5 - excess reactant
The problem gives you the balanced reaction and says that it requires 6 moles of ClO2 for 2 moles of BrF3. It then tells you that you have 6 moles of ClO2 and 5 moles of BrF3.
If you have 12 moles of ClO2 this means you only need 4 moles of BrF3. You can determined this from the equation because you have double the number of moles of ClO2 than it states in the reaction. Since you have 5 moles of BrF3, then BrF3 is in excess.
If you have 12 moles of ClO2 this means you only need 4 moles of BrF3. You can determined this from the equation because you have double the number of moles of ClO2 than it states in the reaction. Since you have 5 moles of BrF3, then BrF3 is in excess.
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Re: M5 - excess reactant
is the excess reactant because you have more moles of it than you need.
The problem says that you have 12 mol of and 5 mol of . You can use the mole ratio from the balanced equation to find out how many moles of you would need if you started with 12 moles of :
Moles of cancels and you are left with 4 moles of .
Since according to the balanced equation you only need 4 moles of but you have 5 moles, it is in excess.
Hope this helps!
The problem says that you have 12 mol of and 5 mol of . You can use the mole ratio from the balanced equation to find out how many moles of you would need if you started with 12 moles of :
Moles of cancels and you are left with 4 moles of .
Since according to the balanced equation you only need 4 moles of but you have 5 moles, it is in excess.
Hope this helps!
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