P 4(s) + 5O 2(g) ------>P 4 O 10(g) if 2.50 g of phosphorus is ignited in a flas

Question

P4(s) + 5O2(g) ------>P4O10(g) if 2.50 g of phosphorus is ignited in a flask containing 750mL of oxygen at STP, how many grams of P4O10 are formed? which reactant is in excess and how much of it is leftover? P4(s) + 5O2(g) ------>P4O10(g) if 2.50 g of phosphorus is ignited in a flask containing 750mL of oxygen at STP, how many grams of P4O10 are formed? which reactant is in excess and how much of it is leftover? if 2.50 g of phosphorus is ignited in a flask containing 750mL of oxygen at STP, how many grams of P4O10 are formed? which reactant is in excess and how much of it is leftover?

Explanation / Answer

Molar mass of phosphorous = 31 gm/mol No. of moles of phosphorous = 2.5/31 moles = 0.08 moles No. of equivalents of P = 0.08 / 4 = 0.02 moles Volume of 1 mole O2 at STP = 22.414 L No. of moles of O2 = 0.75/22.414 moles =0.033 No. of equivalents of O2 = 0.033 x 2/5 =0.013 Clearly, P is in excess and O2 is limiting. No. of moles of P2O5 = no.of equivalents of O2 = 0.013 Amount of P left = 0.02 - 0.013 equivalents = 0.007equivalents of P No. of moles of P left = 0.007 x 4 = 0.028 moles

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