If 7.68 gram of phosphorous solid is mixed with 1.00 L of Chlorine gas at STP to form P2Cl5 according to the following unbalanced chemical reaction P4 (s) + Cl2 (g) →P2Cl5 (g) The molar mass of P4 is 123.88 g/mol. The molar mass of P2Cl5 is 208.22 g/mol. A) Balance the reaction. B) Which reactant is the limiting reactant? C)Calculate the theoretical yield in grams.
If 7.68 gram of phosphorous solid is mixed with 1.00 L of Chlorine gas at STP to form P2Cl5 according to the following unbalanced chemical reaction P4 (s) + Cl2 (g) →P2Cl5 (g) The molar mass of P4 is 123.88 g/mol. The molar mass of P2Cl5 is 208.22 g/mol. A) Balance the reaction. B) Which reactant is the limiting reactant? C)Calculate the theoretical yield in grams.
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If 7.68 gram of phosphorous solid is mixed with 1.00 L of Chlorine gas at STP to form P2Cl5 according to the following unbalanced
P4 (s) + Cl2 (g) →P2Cl5 (g)
The molar mass of P4 is 123.88 g/mol.
The molar mass of P2Cl5 is 208.22 g/mol.
A) Balance the reaction.
B) Which reactant is the limiting reactant?
C)Calculate the theoretical yield in grams.
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