   Chapter 4, Problem 7PS

Chapter
Section
Textbook Problem

The metals industry was a major source of air pollution years ago. One common process involved “roasting” metal sulfides in the air2 PbS(s) + 3 O2(g) 2 PbO(s) + 2 SO2(g)If 2.50 mol of PbS is heated in air, what amount of O2 is required for complete reaction? What amounts of PbO and SO2 are expected?

Interpretation Introduction

Interpretation:

It should be determined that the amount of oxygen required to complete the given reaction and the amount of products formed in the reaction. An amounts table for the given reaction also has to be set up.

Concept introduction:

• The number of moles of any substance can be determined  using the equation,

Numberofmole=GivenmassofthesubstanceMolarmass

• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• Limiting reagent: limiting reagent is a reactant, which consumes completely in the chemical reaction. The quantity of the product depends on this limiting reagent, it can be determined with the help of balanced chemical equation for the reaction.
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Amounts table is a table that shows the amounts of substances (reactants and products) in moles involved in the chemical reaction.
Explanation

Balanced chemical equation for the given reaction is,

2Pbs(s)+3O2(g)2PbO(s)+2SO2(g)

From the balanced equation it is clear that PbSandO2 are reacting in the ratio of 2:3

So,

The amount of O2 require to complete the reaction can be calculated from the amount of PbS

Therefore,

The amount of O2 required    =     2.50molPbS×3molO22molPbS=3.75mol

Similar to the above calculation it is possible to determine the amount of products produced in the reaction easily.

Here the stoichiometric ratio between the products (PbOandSO2 ) and reactant PbS is 1:1

Therefore,

The amount of PbO produced =   2.50molPbS×1molPbO1molPbS=2.50molPbO

The amount of SO2 produced =   2.50molPbS×1molSO21molPbS=2

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started 