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# Solved: Consider the unbalanced equation for the ISBN: 9780321910295 34

## Solution for problem 27P Chapter 8

Introductory Chemistry | 5th Edition

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Problem 27P

PROBLEM 27P

Consider the unbalanced equation for the combustion of butane:

C4H10(g) + O2(g) → CO2(g) + H2O(g)

Balance the equation and determine how many moles of O2 are required to react completely with 4.9 mol of C4H10

Step-by-Step Solution:
Step 1 of 3

Solution 27P

Given unbalanced equation for the combustion of butane:

C4H10(g) + O2(g) → CO2(g) + H2O(g)

The balanced equation is as follows :

2C4H10 + 13O2 = 8CO2 + 10H2O

Now let’s determine how many moles of O2 are required to react completely with 4.9 mol of C4H10 :

The equation is in the ratio :

2 : 3 → 8 : 10

C4H10 : O2  is in the ratio of  2:13.

Since it only asks for the reactant side, we can cross out the product's side for now.

= 2C6H14(g)+13O2(g)

= 4.9...

Step 2 of 3

Step 3 of 3

##### ISBN: 9780321910295

Since the solution to 27P from 8 chapter was answered, more than 338 students have viewed the full step-by-step answer. The answer to “Consider the unbalanced equation for the combustion of butane:C4H10(g) + O2(g) ? CO2(g) + H2O(g)Balance the equation and determine how many moles of O2 are required to react completely with 4.9 mol of C4H10” is broken down into a number of easy to follow steps, and 34 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: equation, balance, combustion, completely, consider. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 27P from chapter: 8 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.

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