HomeHow many moles of water can be produced by burning 325g of octane in excess oxygen?
Wiki User
Answered 2016-03-27 12:24:48
Balanced equation: 2C8H18 + 25O2 ==> 16CO2 + 18H2O
moles of octane used: 325 g x 1 mole/114g = 2.85 moles octane
moles H2O produced: 18 moles H2O/2 moles C8H18 x 2.85 moles C8H18 = 25.65 moles H2O
Wiki User
Answered 2016-03-27 15:08:02
The chemical reaction is:
2 C8H18 + 25 O2 = 16 CO2 + 18 H2O
The answer is 25,66 moles.
Your Answer
Related Questions
octane + oxygen --> water + carbon dioxide
Burning a Fuel in Excess Oxygen.
Burning methane and oxygen produces two compounds when oxygen is available in excess: carbon dioxide and water.
The mass of heavy water produced when 7,00grams of oxygen reacts with excess D2 is 7,875 g.
The mass of water produced when 7,35 g of butane reacts with excess oxygen is 11,4 g.
All combustion (burning) of hydrocarbon in excess oxygen results in carbon dioxide (CO2) and water (H2O) In oxygen-restricted environments, Carbon monoxide will be produced (CO)
The mass of water produced when 5,33 g of butane reacts with excess oxygen is 8,25 g.
The equation for propane gas burning in excess oxygen is:C3H8 + 5 O2 = 3 CO2 + 4 H2O
Carbon Dioxide & Water, Complete burning with excess of oxygen gives out Carbon Dioxide(CO2) + Water , While incomplete burning with limited amount of oxygen gives out Carbon monoxide (CO) + Water
OxygenFood (glucose)Starch (excess food/glucose)
Octane + oxygen ---> carbon dioxide + water Lulu
Carbon dioxide and water if excess of oxygen (air) is provided.
Two molecules of octane has 16 carbon atoms. So 16 molecules of carbon dioxide will be formed when two molecules of octane are burned in presence of oxygen.
Heat. This is produced by the chemical reaction between a hydrocarbon and oxygen in the atmosphere.
The oxygen necessary for burning is not sufficient.
octane + oxygen -------> carbon dioxide + water
Keratin is the protein that contains carbon, hydrogen, and oxygen that makes fingernails and hooves, so the gases produced by burning will be carbon dioxide, carbon monoxide, and water vapor in varying degrees depending on temperature and available oxygen.
Whether air or oxygen is limiting or present in excess
Besides other this is carbonmonoxide, CO gas.
Carbon monoxide is produced when a fuel is burning with an insufficient oxygen supply.
oxygen has no burning point
It goes into the atmosphere as carbon dioxide. The heat produced by burning fuel comes from forming the carbon-oxygen chemical bonds that creates CO2.
2C8H18 + 25 O2 → 16CO2 + 18 H2O + energy so the reactants are octane (actually there are other hydrocarbons present too) and oxygen.
Octane reacts with oxygen to form carbon dioxide and water.
The chemical equation for complete burning of octane is: 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O. This equation shows that 25 moles of diatomic oxygen are required to completely burn each two moles of octane. The gram molecular mass of octane is 114.23 and the gram molecular mass of diatomic oxygen is 2(15.9994). Therefore, the ratio of the mass of oxygen required to completely burn any given mass of octane to the mass of the octane to be burned is 50(15.9994)/2(114.23) or 3.5016, to the justified number of significant digits (the same as the number of digits in the least precisely specified datum 114.23, and the mass of oxygen required to burn 19.8 g of octane is (3.5016)(19.8) or 69.3 grams to the justified number of significant digits, now limited by the less precisely specified datum 119.8.
Asked By Wiki User
What does it mean when the flag is not flying at the White House?
Asked By Wiki User
How many grams of carbs are recommended per day?
Asked By Wiki User
Is Duranice Pace husband dead?
Asked By Wiki User
What is Hugh hefner penis size?
Asked By Wiki User
Ano ang mensahe ng ating pambansang awit?
Asked By Wiki User
What classification instrument of tongatong?
Asked By Wiki User
Copyright © 2021 Multiply Media, LLC. All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply.