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12 Dec 2019

According to the unbalanced chemical equation below, when 13.5 moles of phosphorus react with 40.0 moles of chlorine, what is the limiting reactant and how much excess reactant is left?

P4 + Cl2 ---> PCl5

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Related questions

1.Calculate the number of moles of SO3 formed when 14.0 moles of sulfur dioxide are mixed with 8.0 moles of oxygen.

2. a) Set up the ICE table for the reaction P4 + Cl2 --> 4PCl5 . Initially 84.5 g of phosphorus are mixed with an amount of chlorine. In the Change row calculate the mass of chlorine required to completely react with 84.5 g of phosphorus.

b) Calculate the mass of PCl5 produced when 84.5 g of phosphorus combines with the amount of chlorine calculated in part a.

Elemental phosphorus reacts with chlorine gas according to the equation: P4(s)+6Cl2(g)รขย†ย’4PCl3(l) A reaction mixture initially contains 45.79 g P4 and 132.0 g Cl2.

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

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When solid phosphorus (P4) reacts with oxygen gas, diphosphorus pentoxide is formed. Initially, 2.87 mol of phosphorous and 3.86 mol of oxygen are combined (assume 100% yield).

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