   Chapter 4.1, Problem 4.1CYU

Chapter
Section
Textbook Problem

What mass of oxygen, O2, is required to completely combust 454 g of propane, C3Hg? What masses of CO2 and H2O are produced?

Interpretation Introduction

Interpretation:

The mass of oxygen,O2 which is required to completely react with 454g of propane, C3H8 and the masses of CO2 and H2O produced should be determined.

Concept introduction:

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).
• 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.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
Explanation

Balanced chemical equation for the combustion reaction of propane is,

C3H8(g)+5O2(g)3CO2(g)+4H2O(l)

The amount (moles) of propane available can be calculated by using the equation

Numberofmole=GivenmassofthesubstanceMolarmass

454gC3H8×1molC3H844.10gC3H8=10.29molC3H8

Using the stoichiometric factor calculating the amount of oxygen required based on the amount of glucose as follows,

10.29molC3H8×5molO21molC3H8=51.45molO2

The mass of O2 required    =  51.45molO2×32

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