Download the App!

Get 24/7 study help with the Numerade app for iOS and Android! Enter your email for an invite.

Octane $\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)$ is a component of gasoline. Complete combustion of octane yields $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CO}_{2} .$ Incomplete combustion produces $\mathrm{H}_{2} \mathrm{O}$ and $\mathrm{CO},$ which not only reduces the efficiency of the engine using the fuel but is also toxic. In a certain test run, 1.000 gal of octane is burned in an engine. The total mass of $\mathrm{CO}, \mathrm{CO}_{2},$ and $\mathrm{H}_{2} \mathrm{O}$ produced is $11.53 \mathrm{kg} .$ Calculatethe efficiency of the process; that is, calculate the fraction of octane converted to $\mathrm{CO}_{2}$. The density of octane is $2.650 \mathrm{kg} / \mathrm{gal}$

Get the answer to your homework problem.

Try Numerade free for 7 days

Like

Report

$86.1 \%$

Chemistry 101

Chapter 3

Mass Relationships in Chemical Reactions

Chemical reactions and Stoichiometry

Carleton College

University of Maryland - University College

Lectures

04:02

A chemical reaction is a process that leads to the transformation of one set of chemical substances to another. Chemical reactions can be either spontaneous, requiring no input of energy, or non-spontaneous, typically following the input of some type of energy, such as heat, light or electricity. Chemical reactions are usually characterized by a chemical change, and they yield one or more products after the reaction is complete. Chemical reactions are described with chemical equations, which symbolically present the starting materials, end products, and sometimes intermediate products and reaction conditions. Chemical reactions happen at a characteristic reaction rate at a given temperature and chemical concentration. Typically, reaction rates increase with increasing temperature because there is more thermal energy available to reach the activation energy necessary for breaking bonds between atoms.

08:02

In chemistry, a combination reaction is a chemical reaction in which two or more reactants combine to form more than one product. In a decomposition reaction, one reactant splits into two or more products.

13:43

answer please

03:03

The complete combustion o…

07:55

The complete combustion of…

14:11

00:49

The combustion of gasoline…

03:14

So, given information, we have complete combustion of obtained combustion of obtaineth. Reaction of complete combustion of ocean is to moline plus 25 moles of oxygen 16 mole of c o 2 plus 18 molah 2, o and incomplete combustion of octane tools of obtained plus 17 moles of oxygen and 16 moles 2 plus 18 moles of h, 2 o The volume of obtain is v is equal to 1.00 gallon and the density, a bogaine is d, is equal to 2.652 .650 kg per gallon. The total mass of c o 2 c, o and h, o is mass mass of product is equal to 11.53 kg. Is equal to l, 1530 grand? Let us calculate calculate the friction of ocanconverted to c o 2. First, we will find the mass have obtained. So massarone is equal to density into volume is equal to 2.650 kilogram per gallon into 1.000. Gallon is equal to 2.650. Kilogram is equal to 2.650 into 10 raise to the power 3 gram. Now we will find the number of moles of obanobtain the molar mass octane mass of obtained is equal to 8 into molar mass of carbon plus 18 into molar. Mass of hydrogen is equal to 8 into molar. Mass of carbon is 12.011 gram per mole, plus a 18 into molar. Mass of hydrogen is 1.008 gram per mole. The calculated molar mass of octane is 114.232 gram per mole. The number of moles of obtained is number of moles of obtain is equal to is equal to mass of obtain divided by molar. Mass of obtain is equal to mass of obtains 2.650 into 10, raise to the power 3 gram divided by molar mass of octane 114.232 gram per mole is equal to 23.198198 mole gram, gram cancelled and left it left small, so the molars m number of moles of Obtained is 23.198 moleson. Now we will find the number of moles in the mass of water find the number of moles and mass of watchers since 2, moles of obtained produce produces 18 moles of water in 23.198. Moles of octane will produce so number of moles of water is equal to number of moles of obtained into 18 mole of water divided by 2. Molofwater is equal to 23.198 mole obtain into 18 mole of water divided by 2. Water is equal to 208.782 mole of water, hence the mass of water is the mass of water, is mass of water, is equal to number of moles of water into molar. Mass of water is equal to 208.782 mole water into 18.015. Gram per mole. Mass of water is equal to 3761.21 gramnow. We will find the mass and number of moles of number of moles of c o 2 and c o carbon dioxide and carbon monoxide. So mass of c, o 2 and co is equal to mass of c o plus mass of co, 2 plus mass of h, 2 o mint mass of c o plus mass of co. 2 is equal to mass of product. Minus mass of waters so is equal to 11530 gram. Minus 3761.21 gram is equal to 7768.79 gramsince 2 moles of octane produces 16 mole of c o and co 223.198 will produce, will produce number of moles of c o 2 and co is equal to number of moles of octane into 16 mole of water divided by 2 mole, co, 2 and c o is equal to 23.198 mole obtain into 16 mole of water divided by 2 mole of c o 2 and co is equal to 185.584 mole, co, 2 and c o po. Therefore, therefore, the c o 2 and co product molar mass is molar mass of c o 2 into co is equal to mass of c o 2 into co, divided by number of moles of c o 2 co is equal to mass of cote 7768.79 gram divided By divided by 185.584, mole, co 2 into co is equal to 41.86 gram per mole. Finally, we can calculate the friction and the friction of octane, converted to c o 2 x so x, into molar mass of c o 2 plus 1 minus x into molar. Mass of rononoxide is equal to molar mass of c o 22 co so x, into moral mass of carbon dioxide, 44.099 gram per mole plus 1 minus x and to molar mass of carbon monoxide is 28.010. Gram per mole is equal to molar. Mass of carbon dioxide and carbon monoxide is equal to 41.860 gram per mole so x into 44.099 gram per mole plus 28.010 gram per mole. Minus 28.010 gram per mole into x is equal to 41.860 gram per mole and 16.089 gram per mole into x is equal to 13.850, and x is equal to 0.861 into 100 percent, is equal to 86.1 percent? Is the final result?

View More Answers From This Book

Find Another Textbook

Numerade Educator