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12 carbon monoxides due to lack of enough oxygen when it was being formed
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∙ 10y ago
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What is the balanced equation for the combustion of hexane?
2c6h14 + 15o2 -> 12co2 + 14h2o Stupid site again!! All letters are capitals.
What is the balanced equation for the combustion of c3h6o?
Combustion reactions involve reacting a substance with oxygen to form oxides of the elements that made up the substance. In the case of C3H8 this means carbon dioxide and water: C3H8 + 5 O2 ----> 3 CO2 + 4 H2O
What is the balanced equation for the combustion of hexane?
2c6h14 + 15o2 -> 12co2 + 14h2o Stupid site again!! All letters are capitals.
What is the chemical equation for the complete combustion of 2-methylbutane?
I get 2C6H14+19O2------->12CO2+14H2O
How many moles of carbon dioxide are produced when 84.4 moles of hexane is burned?
Balanced equation first, 2C6H14 + 19O2 >> 12CO2 + 14H2O 84.4 moles hexane (12 moles CO2/2 moles C6H14) = 506.4 moles of CO2
What is the balance equation for the combustion of hexane?
2c6h14 + 15o2 -> 12co2 + 14h2o Stupid site again!! All letters are capitals.
What is a balanced chemical equation of if hexane combusts in the presence of oygen to form carbon dioxide and water?
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.
What is the balanced equation for the combustion of c3h6o?
Combustion reactions involve reacting a substance with oxygen to form oxides of the elements that made up the substance. In the case of C3H8 this means carbon dioxide and water: C3H8 + 5 O2 ----> 3 CO2 + 4 H2O
Can hydrocarbons burn?
Burning is a combustion reaction where the substance being burned reacts with oxygen to form simpler products. For example, the combustion of hexane follows the following balanced reaction: 2C6H14 + 19O2 --> 12CO2 + 14H2O The complete combustion of simple hydrocarbons containing only carbon and hydrogen always produces carbon dioxide and water. Incomplete combustion can also occur, where both carbon monoxide and carbon dioxide are formed in addition to water. Incomplete combustion is more likely to occur in oxygen poorer environments.
What is the balanced equation for the incomplete combustion of heptene C7H14?
Complete combustion is easy. Incomplete combustion is trickier, because there really isn't such a thing as the balanced equation for that, there are several possible balanced equations for that.
What is the balanced equation for the complete combustion of hexane?
The reaction is:C6H12 + 9 O2 = 6 CO2 + 6 H2O
What is the balanced equation for the complete combustion of 3-methyl-2-hexene?
Balanced reaction: C4H10 + 13/2 O2 --> 4CO2 + 5H2O
What is the balanced equation of C2H5NH2(g) plus O2(g) and rarrCO2(g) plus H2O(g) plus N2(g)?
4C2H5NH2(g)+ 15O2(g) --> 8CO2(g) + 14H2O(l) + 2N2(g)
How can you calculate the amount of carbon dioxide emitted from the burning of an object?
This can be done precisely under certain conditions, but in practice things aren't so simple. You need to know the exact chemical formula of the thing being burned (this can be difficult if you are burning wood, for instance, which is a complex mixture of thousands of compounds). You also have to assume that the combustion is complete -- in other words that all hydrocarbons are completely converted into carbon dioxide and water, which is not always the case in normal burning situations. The actual reactions that occur while burning something are very complicated in fact, but to a close approximation, you can figure out the amount of CO2 produced in the following way:First, write the balance equation for the combustion of the hydrocarbon. The reactants are the hydrocarbon itself and oxygen gas (O2). The products are carbon dioxide and water. See the Related Questions to the left for how to do this.Then use stoichiometry to figure out for a certain amount of hydrocarbon burned how much CO2 you will produce. See the Related Questions links to the left for how to do this also.See the Related Questions links to the left for detailed instructions on how to do each of these steps! Note that in both of the related questions, example problems have been worked out using the combustion of a hydrocarbon! Most of the work is done for you already! Just see the examples in the linked questions to the left.
