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Solved: A loud classroom demonstration involves igniting a

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 99P Chapter 8

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 99P

PROBLEM 99P

A loud classroom demonstration involves igniting a hydrogen-filled balloon. The hydrogen within the balloon reacts explosively with oxygen in the air to form water according to this reaction:

2 H2(g) + O2(g) → 2 H2O(g)

If the balloon is filled with a mixture of hydrogen and oxygen, the explosion is even louder than if the balloon is filled with only hydrogen; the intensity of the explosion depends on the relative amounts of oxygen and hydrogen within the balloon. Consider the molecular views representing different amounts of hydrogen and oxygen in four different balloons. Based on the balanced chemical equation, which balloon will make the loudest explosion?

Step-by-Step Solution:

Solution 99P :

Step 1:

Given reaction:

2 H2(g) + O2(g) → 2 H2O(g)

 

Here, we have to determine which balloon makes the loudest explosion, based on the balanced chemical reaction.

In the balloon, oxygen atom is represented in red color and hydrogen in white color.

Step 2:

Now, let’s examine all the balloons :

balloon (a)  :

It has 11 molecules of hydrogen and 2 molecules of oxygen :

We know to form 1 molecule of water, we need 2 molecules of hydrogen and 1 molecule of oxygen. We are given the reaction :

        2 H2(g) + O2(g) → 2 H2O(g)

Now, let’s calculate the number of moles of H2O that can be formed from 11 molecules of H2 :

                

                = 11 H2 

= 11 H2O.  

Now, let’s calculate the number of moles of H2O that can be formed from 2 molecules of O2 :

                

                = 2 O2 

= 4 H2O.  

From the above calculation, we see that there are enough molecules of H2 to form 11 molecules of H2O. Therefore, O2 is the limiting reactant. Thus, 4 molecules of water is formed during the explosion.

Step 3:

balloon (b) :

It has 8 molecules of hydrogen and 4 molecules of oxygen :

Now, let’s calculate the number of moles of H2O that can be formed from 8 molecules of H2 :

                

                = 8 H2 

= 8 H2O.  

Now, let’s calculate the number of moles of H2O that can be formed from 4 molecules of O2 :

                

                = 4 O2 

= 8 H2O.  

From the above calculation, we see that there are enough molecules of H2 to form 8 molecules of H2O. Therefore, O2 is the limiting reactant. Thus, 8 molecules of water is formed during the explosion.

Step 4 of 5

Chapter 8, Problem 99P is Solved
Step 5 of 5

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The answer to “A loud classroom demonstration involves igniting a hydrogen-filled balloon. The hydrogen within the balloon reacts explosively with oxygen in the air to form water according to this reaction:2 H2(g) + O2(g) ? 2 H2O(g)If the balloon is filled with a mixture of hydrogen and oxygen, the explosion is even louder than if the balloon is filled with only hydrogen; the intensity of the explosion depends on the relative amounts of oxygen and hydrogen within the balloon. Consider the molecular views representing different amounts of hydrogen and oxygen in four different balloons. Based on the balanced chemical equation, which balloon will make the loudest explosion?” is broken down into a number of easy to follow steps, and 104 words. This full solution covers the following key subjects: hydrogen, balloon, oxygen, explosion, filled. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Since the solution to 99P from 8 chapter was answered, more than 2592 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 99P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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