I don't know ...........cheesecake
its the combustion of octane
Your equation is not well represented and therefore, cannot be balanced.
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.
2c8h18 + 25o2 ---> 16co2 + 18h2o
octane + oxygen --> water + carbon dioxide
The combustion reaction of octane is:2 C8H18 + 25 O2 = 16 CO2 + 18 H2OSo, the number of oxygen molecules is 25.The isomer trimethylpentane is used as standard in octane rating: the end of the scale at 100.
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
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.
2c8h18 + 25o2 ---> 16co2 + 18h2o
it is -193 jk/g. or it is D.
the reaction is from the combustion of Octane
yes....but it needs balancing.....the exact answer is 2C8H18 + 25o2 = 16co2 + 18h2o
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.
2C8H18 + 25O2 = 16CO2 + 18H2O Of course some times the reaction yields carbon monoxide as well, most of which is changed to CO2 in the catalytic convert.
octane + oxygen -------> carbon dioxide + water
octane + oxygen --> water + carbon dioxide
2C8H18 + 17O2 --> 16CO + 18H2O C8H18 + 8.5O2 --> 8CO + 9H2O half equation, halfs can be used in combustion.
Balanced equation. 2C8H18 + 25O2 -> 16CO2 + 18H2O 5.5 moles C8H18 (25 moles O2/2 moles C8H18) = 68.75 moles O2 needed