Problem: Consider the following unbalanced equation:Ca3(PO4)2 (s) + H2SO4 (aq) → CaSO4 (s) + H3PO4 (aq)What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?

FREE Expert Solution

To balance equation → number of atoms must be the same for both sides of reaction → add coefficients


Balanced: Ca3(PO4)2(s) + 3H2SO4(aq) → 3CaSO4(s) + 2H3PO4(aq)

Reactants                        Products

Ca - 3                                     Ca – 3

P - 2                                       P - 2

O - 12 20                                O - 20

H -2 6                                     H - 6

S - 1 3                                    S - 3


mass percent, H2SO4= mass H2SO4  total mass×100mass H2SO4=1.0 kg×103g1 kg×98100


mass H2SO4  980 g H2SO4


Determine limiting reactant  reactant that forms the less amount of product

  • determines the maximum mass of the product (H2O) formed.


Mole to mole comparison: 

  • 3 mol H2SO4 forms 3 mol CaSO4
  • 3 mol H2SO4 forms 2 mol H3PO4
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Problem Details

Consider the following unbalanced equation:

Ca3(PO4)2 (s) + H2SO4 (aq) → CaSO4 (s) + H3PO4 (aq)

What masses of calcium sulfate and phosphoric acid can be produced from the reaction of 1.0 kg calcium phosphate with 1.0 kg concentrated sulfuric acid (98% H2SO4 by mass)?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.