What is the theoretical yield (in grams) of phosphorus pentachloride when 3.85 g of phosphorus reacts with 25.8 g of chlorine according to the following reaction:
P4 (s) + 10 Cl2 (g) → 4 PCl5 (l)
Use the correct number of significant figures, fill in the number ONLY!
1)
Answer
2.48g
Explanation
P4(s) + 10Cl2(g) ------> 4PCl5(l)
stoichiometrically, 1mole of P4 reacts with two moles 10moles of Cl2
given moles of P4 = 4.69g/ 123.88g/mol = 0.03786mol
given moles of Cl2 = 12.66g/70.90g/mol = 0.1786mol
limiting reagent is Cl2
0.1786moles of Cl2 react with 0.01786moles of P4
Remaining moles of P4 = 0.03786mol - 0.01786mol = 0.02mol
mass of P4 reamaining = 0.02mol × 123.88g/mol = 2.48g
2)
Answer
Explanation
P4(s) + 10Cl2(g) -------> 4PCl5
given moles of P4 = 3.85g/123.88g/mol = 0.03108mol
given moles of Cl2 = 25.8g/ 70.90g/mol = 0.3639mol
limiting reagent is P4
stoichiometrically , 1mole of P4 gives 4moles of PCl5
0.03108moles of P4 gives 0.12432moles of PCl5
mass of PCl5 maximum can be produced = 0.12432mol × 208.22g/mol = 4.41g
Theoretical yield = 4.41g
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