I don't know ...........cheesecake
its the combustion of octane
The chemical equation for burning gasoline is: 2C8H18 + 25O2 -> 16CO2 + 18H2O.
2C8H18 + 25O2 -> 8CO2 + 18H2O No. I can see right off that you have 16 atoms of carbon on the reactant (left) side and only 8 atoms of carbon on the product (right) side. Let's see. 2C8H18 + 25O2 -> 16CO2 + 18H2O Now it is balanced.
octane + oxygen --> water + carbon dioxide
The balanced combustion reaction for octane would be: 2C8H18 + 25O2 → 16CO2 + 18H2O + heat
Reaction of octane combustion- 2C8H18+25O2= 16CO2+ 18H2O That mean from 228g octane (16*22.4dm3) = 358.4dm3 of CO2 is produced. {because volume of each mole is 22.4dm3} Now, from 10 kg of octane produced volume of CO2 is = (358.4*10000)/228 =(15719.298 dm3/1000)m3 =15.719 m3.
2c8h18 + 25o2--> 16co2 + 18h2o
it is -193 jk/g. or it is D.
The chemical equation for burning gasoline is: 2C8H18 + 25O2 -> 16CO2 + 18H2O.
2C8H18 + 25O2 -> 8CO2 + 18H2O No. I can see right off that you have 16 atoms of carbon on the reactant (left) side and only 8 atoms of carbon on the product (right) side. Let's see. 2C8H18 + 25O2 -> 16CO2 + 18H2O Now it is balanced.
Gasoline is a complex mixture of hydrocarbons. When combusted in an engine, the main chemical reaction is the oxidation of these hydrocarbons to produce carbon dioxide, water, and heat. The balanced chemical equation for the combustion of a simple hydrocarbon such as octane (C8H18) in gasoline would be: 2C8H18 + 25O2 -> 16CO2 + 18H2O + heat.
2C8H18 + 12.5O2 --------> 16CO2 + 18 H2O *As O2 is diatomic you can use half multiples when balancing.*
This is a typical combustion reaction in that it involves a hydrocarbon reacting with oxygen. The products of combustion reactions are always carbon dioxide and water, just in varying quantities.
The reaction is: C3H8 + 5 O2 -> 3 CO2 + 4 H2O
octane + oxygen -------> carbon dioxide + water
There are 18 moles of water produced in the reaction. This is determined by the stoichiometry of the balanced chemical equation, which shows that for every 2 moles of C8H18 consumed, 18 moles of H2O are produced.
octane + oxygen --> water + carbon dioxide
The balanced combustion reaction for octane would be: 2C8H18 + 25O2 → 16CO2 + 18H2O + heat