If 1.50 mol of CaCl2 is mixed with 1.5 mol Na3PO4, the maximum amount in moles of Ca3(PO4)2 that can be formed is 2 Na3PO4 + 3CACl2 -> Ca3(PO4)2 + 6 NaCl
From the balanced equation we can say that
2 mole of Na3PO4 requires 3 mole of CaCl2 so
1.50 mole of Na3PO4 will require
= 1.50 mole of Na3PO4 *( 3 mole of CaCl2 / 2 mole of Na3PO4)
= 2.25 mole of CaCl2
But we have only 1.50 mole of CaCl2 which is in short so CaCl2 is limiting reactant
From the balanced equation we can say that
3 mole of CaCl2 produces 1 mole of Ca3(PO4)2 so
1.50 mole of CaCl2 will produce
= 1.50 mole of CaCl2 *(1 mole of Ca3(PO4)2 / 3 mole of CaCl2)
= 0.500 mole of Ca3(PO4)2
mass of 1 mole of Ca3(PO4)2 = 310.18 g so
the mass of 0.500 mole of Ca3(PO4)2 = 155 g
Therefore, the mass of Ca3(PO4)2 produced would be 155 g
If 1.50 mol of CaCl2 is mixed with 1.5 mol Na3PO4, the maximum amount in moles...
Balance the following chemical equations:
1.) CaCl2 + KOH
KCl + Ca(OH)2
2.) CaCl2 + Na3PO4
NaCl + Ca3(PO4)2
3.) CaCl2 + Li2CO3
KCl + CaCO3
4.) Fe(NO3)3 +
NaC2H3O2 + H2O
NaNO3 +
Fe3O(C2H3O2)6+
+ H3O+ + NO3-
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