a. Write the balanced equation for the combustion of isooctane (C8 H18) to produce water vapor a

step 1 Hi there. In this problem, we are combusting isoctane. And they give us the formula for isoctane

A. Write the balanced equation for the combustion of...

Key Concepts

Combustion Reaction

A combustion reaction is a chemical process in which a fuel reacts with oxygen to release energy, typically producing carbon dioxide and water as the main products. Understanding this reaction is essential for energy production and environmental studies, as it involves complete oxidation of organic compounds.

Balanced Chemical Equations

Balanced chemical equations represent the conservation of mass by ensuring that the number of atoms of each element is the same on both sides of the equation. This balancing is fundamental not only for satisfying the law of conservation of mass but also for accurately carrying out stoichiometric calculations in any reaction.

Stoichiometry

Stoichiometry involves the quantitative analysis of reactants and products in a chemical reaction using the balanced equation. It provides the molar relationships needed to determine how much product will form from given quantities of reactants, making it crucial for both lab-scale reactions and industrial applications.

Theoretical Yield

The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant, as predicted by the stoichiometric relationships of the balanced equation. It is a key concept in assessing the efficiency of chemical processes and in planning for resource use in reactions.

Unit Conversions

Unit conversions are the process of converting measurements from one unit to another, such as volume to mass using a density value, or converting between different volume units. Mastery of unit conversions is essential for correctly applying stoichiometric calculations and analyzing real-world quantities in chemical reactions.

Transcript

00:01 Hi there.

00:02 In this problem, we are combusting isoctane.

00:07 And they give us the formula for isoctane.

00:09 It is c8, h18, and it combusts.

00:16 So in a combustion reaction, react with oxygen gas, and we produce water vapor and carbon dioxide.

00:36 And this isoctane would start off as a liquid.

00:40 All right, so we need to balance this first of all.

00:44 I see eight carbons, so i am going to put an eight there for a moment anyway.

00:51 And i also have 18 hydrogen.

00:53 So on the product side, it's h2, so nine times two gives me 18.

00:59 Now if i add up the oxygens on the product side, i have nine oxygens from the water and another 16 from the co2.

01:10 So that is 25.

01:12 So i would love to be able to put a 25 halves in front of the oxygen to balance that.

01:21 But we know that all coefficients have to be whole numbers.

01:25 We can't have a half of an oxygen molecule.

01:27 So to get rid of this half, i'm going to use a trick from math, and i am going to multiply everything through by two to get rid of that fraction that has a two in the denominator.

01:39 So two times one gives me two there.

01:41 2 times 25 halves gives me 25.

01:47 2 times 9 gives me 18, and 2 times 8 gives me 16.

01:58 Let's see if i can erase here.

02:03 Oops.

02:05 All right.

02:07 So we have 16 of those.

02:09 Let's also get rid of that.

02:12 Write that out a little cleaner.

02:16 All right, so we have our balanced equation here.

02:19 That was all we needed to do for part a.

02:22 For part b, they give us some information.

02:25 They say, first of all, let's assume that gasoline is 100 % isoctane.

02:29 It is not, but for the purpose of this problem, we are going to assume that.

02:36 And 1 .2 times 10 to the 10th gallons of this isoctane are burned.

02:47 That's the approximate annual consumption in the u .s.

02:54 So we also know the density of the gasoline is .692 grams per milliliter is going to come in handy.

03:09 And we want to know the theoretical yield of carbon dioxide that's going to be produced.

03:15 It doesn't really give us a unit here.

03:18 I am going to work it through to grams.

03:21 So we know how many grams of co2 are being produced.

03:25 Okay, so this is a stoichiometry problem.

03:27 We are going to start with the amount of the isoctane we have, and we're going to have to do some steps of conversion to get us to grams of co2...

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