Problem: How many moles of lithium nitrate are theoretically produced if we start with 3.4 moles of Ca(NO3)2 and 2.4 moles Li3PO4 3 Ca(NO3)2 + 2 Li3PO4 → 6 LiNO3 + Ca3(PO4)2 A) 3.4 B) 6.8 C) 7.2 D) 8.6 

FREE Expert Solution

 From the problem, the balanced reaction is:

3 Ca(NO3)2 + 2 Li3PO4 → 6 LiNO3 + Ca3(PO4)2 


Notice that we are given the mole of both reactants: this means we need to determine the limiting reactant, which is the reactant that forms the less amount of product


This is because once the limiting reactant is all used up, the reaction can no longer proceed and make more products.

This means the limiting reactant determines the maximum mole of the product formed.



We need to perform a mole-to-mole comparison between each reactant and lithium nitrate (LiNO3). 


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Problem Details

How many moles of lithium nitrate are theoretically produced if we start with 3.4 moles of Ca(NO3)2 and 2.4 moles Li3PO4 


3 Ca(NO3)2 + 2 Li3PO4 → 6 LiNO3 + Ca3(PO4)2 

A) 3.4 

B) 6.8 

C) 7.2 

D) 8.6 

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. If you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems.