Problem: The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated.Find the mass of PH3 that forms from the reaction of 1.55 g NH3.

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FREE Expert Solution

Balanced equations for reactions: number of elements on both sides is equal.


  • 4NH3 + 5O2 → 4NO + 6H2
  • P+ 6NO → P4O6 + 3N2
  • P4O+ 6H2O + heat → PH3 + 3H3PO4


Mole-to-mole comparison:

  • 4 moles of NH3 form 4 moles NO
  • 6 moles NO forms 1 mol P4O6
  • 1 mol P4Oforms 1 mole of PH3 (overall)


Molar mass NH3 = 17 g/mol

Molar mass PH= 34 g/mol


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Problem Details

The reaction of NH3 and O2 forms NO and water. The NO can be used to convert P4 to P4O6, forming N2 in the process. The P4O6 can be treated with water to form H3PO3, which forms PH3 and H3PO4 when heated.

Find the mass of PH3 that forms from the reaction of 1.55 g NH3.

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Based on our data, we think this problem is relevant for Professor Dixon's class at UCF.