   Chapter 4.9, Problem 4.3ACP

Chapter
Section
Textbook Problem

Calculate the volume of water obtained from 1.00 liter of liquid oxygen. (a) 2.0 L (b) 1.28 L (c) 0.64 L (d) 1.0 L

Interpretation Introduction

Interpretation:

The volume of water obtained from 1.00L of liquid oxygen has to be determined.

Concept introduction:

• The relation between the number of moles and mass of the substance is ,

Numberofmole=MassingramMolarmass

Massingramofthesubstance=Numberofmole×Molarmass

• 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 mole (g/mol).
• Mass=Density×Volume
• Volume=MassDensity
• 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

Reason for the correct option:

The strategy map is,

VolO21A2molO23B4MassofH2O5VolH2O

Here A is the mass of O2 and B is the amount of H2O.

The balanced chemical equation for the reaction involving hydrogen and oxygen as a reactant is,

2H2+O22H2O

The amount of O2 available can be calculated as follows,

1.00×103mLO2×(1.14gO21mLO2)×(1molO232.00gO2)=35.625mol

From the amount of O2 number of moles of H2O(B) can be calculated. Stoichiometric ratio between O2 and H2O is 2:1

So,

The amount of  H2O35.625molO2×2molH2O1molO2=71

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