   Chapter 3, Problem 168CWP

Chapter
Section
Textbook Problem

Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C 5 H 12 ( l ) + O 2 ( g ) → CO 2 ( g ) + H 2 O ( l ) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?

Interpretation Introduction

Interpretation: The mass of water produced in a given chemical reaction is to be calculated.

Explanation

Explanation

Given

The Mass of pentane (C5H12) is 20.4 g .

The Molar mass of (C5H12) is 72 g

The given chemical equation is,

C2H12(l)+O2(g)CO2(g)+H2O(l) .

In the combustion of pentane one mole of pentane (C5H12) gives one mole of water (H2O) .

The mass of H2O is considered to be x g .

The Molar mass of H2O is 18.0 g/mol .

The number of moles of H2O and (C5H12) is calculated by the formula,

Numberofmoles of H2O=Mass of H2OMolarmass of H2

For H2O ,

Substitute the value of Mass and Molar mass of H2O in the above expression

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