If 5 moles of p4 reacted with 22 moles cl2 according to the above reaction, determine:
a) how many moles pcl3 are produced

b) how many moles of p4 are left in excess after the reaction (if any)

c) how many moles of cl2 are left in excess after the reaction (if any)

Answer :

(a) The moles of = 2.44 moles

(b) The moles of left = 1.34 mole

(c) There is no amount left of because it is completely consumed in the reaction.

Explanation :

The balanced chemical reaction will be,

First we have to calculate excess and limiting reactant.

From the balanced chemical reaction, we conclude that

As, 6 moles of react with 1 mole of

So, 22 moles of react with moles of

From this we conclude that, is an excess reagent because the given moles are greater than the required moles and is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of from the limiting reactant's moles.

As, 6 moles of react to give 4 moles of

So, 3.66 moles of react to give moles of

The moles of = 2.44 moles

The moles of left = 5 - 3.66 = 1.34 mole

There is no amount left of because it is completely consumed in the reaction.

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