The reaction is:
C6H12 + 9 O2 = 6 CO2 + 6 H2O
2C6H14 + 19O2 ---> 14H2O + 12CO2 + energy
You need to have water, CO2 and energy all as resultants of the equation since hexane is an alkane and they all yield those results during combustion
C6H12(l)+9O2(g)---->6CO2(g)+6H2O(l)
Make sure you write a ONE headed arrow, Not the equillibrium one =)
for combustion of cyclohexene [C6H10], the reaction is shown below:
2 C6H10 (l) + 17 O2 (g) --> 12 CO2 (g) + 10 H2O (g)
C6H12(l)+9O2(g)---->6CO2(g)+6H2O(l) apex
C6h10+17/2o2---->6co2+5h2o
(1) c6h12 + 6 o2 ---> 6 h2o + 6 co2
2 c7h14 + 21o2 ----> 14co2 + 14h2o
C4h8 + 6 o2 = 4 co2 + 4 h2o.
This depends on how much hexane was being burned and how much oxygen was present.Because the complete combustion of carbon involves placing two moles of oxygen on one mole of carbon plus the formation of water, you would need 19 moles of diatomic oxygen for every one mole of hexane.1 C6H14 + 19 O2 --> 6 CO2 + 7 H2O
They are not reacting. but they are mixing together.
you can use the Clausius-Clapeyron equation if you know the temperature of hexane at 1.5 ATM
The balanced equation for complete combustion of heptane is C7H16 + 11O2 ---(ignition)---> 7CO2 + 8H2O. For each moelcule of heptane, you would need 11 molecules of oxygen gas.
Maybe this desription of 'soot' helps you: see 'Related links' just below this answering page.
Hexane + Oxygen -> Carbon Dioxide + Water - for full combustion Hexane + Oxygen -> Carbon + Carbon Monoxide + Water - for partial combustion
16.9
Yes*. The empirical equation for this reaction is: 2C6H14 + 19O2 ---> 12CO2 + 14H2O. * n-Hexane, burned in an Iron III-catalyzed environment of pure oxygen gas, is oxidized completely. Intermediate products, such as peroxides are formed but the final products are carbon dioxide and water.
2c6h14 + 15o2 -> 12co2 + 14h2o Stupid site again!! All letters are capitals.
This depends on how much hexane was being burned and how much oxygen was present.Because the complete combustion of carbon involves placing two moles of oxygen on one mole of carbon plus the formation of water, you would need 19 moles of diatomic oxygen for every one mole of hexane.1 C6H14 + 19 O2 --> 6 CO2 + 7 H2O
Hexane - lower heating value at 15,4 0C: 44,752 MJ/kg (3 856,66 kg/mol)
Balanced equation first, 2C6H14 + 19O2 >> 12CO2 + 14H2O 84.4 moles hexane (12 moles CO2/2 moles C6H14) = 506.4 moles of CO2
2c6h14 + 15o2 -> 12co2 + 14h2o Stupid site again!! All letters are capitals.
They are not reacting. but they are mixing together.
you can use the Clausius-Clapeyron equation if you know the temperature of hexane at 1.5 ATM
Kerosene is the liquid form of a combustible hydrocarbon mixture. The carbon chains are usually a mix of hexane to decahexane, which means there is no set chemical formula.
Maybe this desription of 'soot' helps you: see 'Related links' just below this answering page.