   # Water can be synthesized according to the following unbalanced chemical equation: H2+ O 2 → H 2 O a. Balance the equation. b. How many moles of H 2 O can be produced if you have 2.72 mol of O 2 and an unlimited amount of H 2 ? c. How many moles of H 2 would be necessary to produce 10.0 g of water? d. How many grams of water would be formed by the complete reaction of 2.5 g of H 2 ? ### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

#### Solutions

Chapter
Section ### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 4, Problem 53E
Textbook Problem
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## Water can be synthesized according to the following unbalanced chemical equation: H2+ O 2 →  H 2 O a. Balance the equation.b. How many moles of H 2 O can be produced if you have 2.72 mol of O 2 and an unlimited amount of H 2 ?c. How many moles of H 2 would be necessary to produce 10.0 g of water?d. How many grams of water would be formed by the complete reaction of 2.5 g of H 2 ?

Interpretation Introduction

Interpretation:

The chemical equation is to be balanced. Also, the number of moles of H2O, number of moles of H2, and the number of grams of water are to be determined.

Concept introduction:

A chemical equation is a symbolic depiction of a chemical reaction that contains symbols and formula.

In a chemical reaction, the starting substances on the left side are known as reactants, while the substances on the right side are known as products.

A conversion factor is a numerical ratio, which is used in order to convert one unit into another.

The chemical formula represents the precise number of atoms in a molecule, but not their structural arrangement.

### Explanation of Solution

a) The balance equation

Oxygen atom is balanced by multiplying the coefficient 2 with H2O in the product part as follows:

H2+O22H2O

In the next step, H atom is balanced by multiplying the coefficient 2 with H2 in the reactant part as follows:

2H2+O22H2O

b) Number of moles of H2O produced with 2.72mol of O2 and an unlimited amount of H2.

The equivalence is obtained between moles of O2 and moles of H2O with the help of the chemical formula as follows:

2mol H2O1mol O2

In order to obtain the moles of H2O, the conversion factor proceeds as follows:

2.72mol O2×2mol H2O1mol O2=5.44mol H2O

Therefore, the moles of water are 5.44 mol.

c) Number of moles of H2 necessary to produce 10.0g of water

The equivalence is obtained between grams of H2O and moles of H2O with the help of the chemical formula as follows:

1mol H2O18.02g H2O

In order to obtain the moles of H2O, the conversion factor proceeds as follows:

10.0 g H2O×1mol H2O18.02H2O=0.555mol H2O

Here,

Molarmass of H2O=18

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