Nitrobenzene (C₆H₅NO₂) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C₆H₆) with nitric acid:
C₆H₆(l) + HNO₃(aq) → C₆H₅NO₂(l) + H₂O(l)
a. Identify the limiting reagent in the reaction of 27.5 g of nitric acid with 75 g of benzene.

Question

Nitrobenzene (C₆H₅NO₂) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C₆H₆) with nitric acid:

C₆H₆(l) + HNO₃(aq) → C₆H₅NO₂(l) + H₂O(l)

a. Identify the limiting reagent in the reaction of 27.5 g of nitric acid with 75 g of benzene.

Accepted Answer

Hello everyone today, we've been given a falling problem. The organic compound 13 dot natural benzene is an explosive agent and a manufacturing byproduct of TNT. A Samantha nitrate nitrobenzene with the aid of a sulfuric acid catalyst and heat proceeds completely to give a 13 dot nitrobenzene product, identify the limiting reagent. If 100 g of nitrobenzene, 100 g of nitric acid are reacted. So remember the limiting reagent is simply the reactant that is completely consumed in a reaction since it has the least amount. And it also determines the maximum amount of product that can form. So using stock geometry, we're gonna see which one of these reactions gives us that. So first we have our 1 3 by natural benzene. So we're gonna take what we were given first, which was our 100 g. And then we're going to multiply that by the Molar mass, which according to the periodic table, if we take all of their masses of carbon, hydrogen, nitrogen and oxygen multiply by how many we have. And then we add them together. We're gonna get 123.1 g. Lastly, we're gonna multiply by the multiple ratio that in one mole of our 13 day nitrobenzene, We produced one mole of our product. This gives us 0.81 moles of our product. We're then going to find for nitric acid. We had our 100 g multiplied by the molar mass, which the masses of our hydrogen nitrogen and oxygen multiplied by however many we have and add those together 63.02 g. Lastly, we're gonna multiply this by the ratio that we had one mole Of major gas at, according to our equation here, producing one mole of our product. This is gonna give us 1.586 moles of our product. So since 100 g of our nitro benzene gives the smallest number of moles of our product, it is going to be our limited reactant. So our answer is going to be our nitro benzene. And with that we've answered the question overall, I hope it's helped, and until next time.

Verified video answer for a similar problem:

Key Concepts

Limiting Reagent

Stoichiometry

Molar Mass