When solid phosphorus (p4) reacts with oxygen gas, diphosphorus pentoxide is formed. initially 2.87 mol of phosphorus and 3.86 mol of oxygen are combined. (assume 100% yield). a) write a balanced equation for the reaction. b) what is the limiting reactant? c) how many miles of excess reactant remain after the reaction is complete?

Answer :

(a) The balanced chemical reaction will be,

(b) The limiting reactant is .

(c) The remaining moles of excess reactant,  is 0.94 moles.

Solution : Given,

Moles of = 2.87 mole

Moles of = 3.86 mole

First we have to calculate the limiting and excess reagent.

The balanced chemical reaction will be,

From the balanced reaction we conclude that

As, 2 mole of react with 1 mole of

So, 3.86 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 remaining moles of excess reactant, .

Remaining moles of excess reactant = Given moles of excess reactant - Required moles of excess reactant

Remaining moles of excess reactant = 2.87 - 1.93 = 0.94 moles

The remaining moles of excess reactant,  is 0.94 moles.

the answer is d.) potassium