What mass of phosphorus pentachloride would be produced by the complete reaction of 6.66 g of P4? Report your answer to the hundredths of a gram without units.
Molar mass of P4 = 123.88 g/mol
mass of P4 = 6.66 g
mol of P4 = (mass)/(molar mass)
= 6.66/1.239*10^2
= 5.376*10^-2 mol
Balanced chemical equation is:
P4 + 10 Cl2 -> 4 PCl5
According to balanced equation
mol of PCl5 formed = (4/1)* moles of P4
= (4/1)*5.376*10^-2
= 0.215 mol
Molar mass of PCl5,
MM = 1*MM(P) + 5*MM(Cl)
= 1*30.97 + 5*35.45
= 208.22 g/mol
mass of PCl5 = number of mol * molar mass
= 0.215*2.082*10^2
= 44.78 g
Answer: 44.78 g
What mass of phosphorus pentachloride would be produced by the complete reaction of 6.66 g of...
What mass of phosphorus pentachloride would be produced by the complete reaction of 4.11 g of Cl2?
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!
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Please provide all steps and a detailed explanation
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