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How many grams of carbon dioxide is produced from the combustion of B grams of hexane?
The combustion of hexane (C6H14) produces carbon dioxide (CO2) according to the reaction: C6H14 + 7O2 → 6CO2 + 7H2O. For every 1 gram of hexane burned, approximately 3.03 grams of carbon dioxide are produced. Therefore, from the combustion of B grams of hexane, the amount of carbon dioxide produced would be approximately 3.03B grams.
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How many moles of carbon dioxide are produced when 84.4 moles of hexane is burned?
To determine the number of moles of carbon dioxide produced when hexane is burned, we need to consider the balanced chemical equation for the combustion of hexane, which is C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O. From the balanced equation, we can see that for every mole of hexane burned, 6 moles of carbon dioxide are produced. Therefore, if 84.4 moles of hexane is burned, 6 * 84.4 = 506.4 moles of carbon dioxide would be produced.
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.
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 energy released in the combustion of hexane?
The energy released in the combustion of hexane is approximately 46.8 megajoules per gram of hexane combusted.
What is the Balanced equation for the complete combustion of c6h14?
The balanced equation for the complete combustion of hexane (C6H14) is: [ \text{C}6\text{H}{14} + 9 \text{O}_2 \rightarrow 6 \text{CO}_2 + 7 \text{H}_2\text{O} ] This equation indicates that one molecule of hexane reacts with nine molecules of oxygen to produce six molecules of carbon dioxide and seven molecules of water.
What is the word equation for burning petrol in an engine?
Hexane + Oxygen -> Carbon Dioxide + Water - for full combustion Hexane + Oxygen -> Carbon + Carbon Monoxide + Water - for partial combustion
How many moles of carbon dioxide are produced when 84.4 moles of hexane is burned?
To determine the number of moles of carbon dioxide produced when hexane is burned, we need to consider the balanced chemical equation for the combustion of hexane, which is C6H14 + 19/2 O2 -> 6 CO2 + 7 H2O. From the balanced equation, we can see that for every mole of hexane burned, 6 moles of carbon dioxide are produced. Therefore, if 84.4 moles of hexane is burned, 6 * 84.4 = 506.4 moles of carbon dioxide would be produced.
What mass of carbon dioxide is produced by the complete combustion of 5.50 grams of hexane?
The chemical formula of hexane is C6H14. To find the mass of CO2 produced, first calculate the molar mass of hexane. Then use stoichiometry to find the molar ratio between hexane and CO2. Finally, calculate the mass of CO2 produced using this ratio and the given mass of hexane.
Why combustion of hexane produce no soot?
Combustion of hexane produces no soot because it is a clean-burning hydrocarbon with a simple molecular structure. When hexane combusts, it forms carbon dioxide and water vapor as the main products, without leaving behind carbon particles that would create soot.
If hexane was burned in a limited supply of oxygen the combustion would not be complete?
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
What mass of carbon dioxide can be produced from 25.0g of C6H14 and excess oxygen?
The gram molecular mass of hexane is 86.18. Therefore, 25.0 g of hexane constitute 25.0/86.18 or 0.290 moles. Each mole of hexane contains six carbon atoms and therefore will produce six molecules of carbon dioxide by burning in an excess of oxygen. 6 X 0.290 = 1.74 moles of carbon dioxide. The gram molecular mass of carbon dioxide is 44.00. Therefore, the mass of carbon dioxide produced will be 1.74 X 44.00 or 76.6 grams of carbon dioxide, to the justified number of significant digits.
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.
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.
Hexane and oxygen gas as a reaction?
When hexane (C6H14) reacts with oxygen gas (O2) in the presence of heat or a spark, combustion occurs producing carbon dioxide (CO2) and water (H2O) as the main products. The balanced chemical equation for this reaction is: 2 C6H14 + 19 O2 -> 12 CO2 + 14 H2O.
What is the energy released in the combustion of hexane?
The energy released in the combustion of hexane is approximately 46.8 megajoules per gram of hexane combusted.
Why benzene burns with sooty flame why not hexane?
Benzene burns with a sooty flame due to its incomplete combustion, which results in the formation of carbon particles (soot). Hexane, on the other hand, is a saturated hydrocarbon and tends to undergo complete combustion, resulting in a cleaner flame with less soot formation.
What is the Balanced equation for the complete combustion of c6h14?
The balanced equation for the complete combustion of hexane (C6H14) is: [ \text{C}6\text{H}{14} + 9 \text{O}_2 \rightarrow 6 \text{CO}_2 + 7 \text{H}_2\text{O} ] This equation indicates that one molecule of hexane reacts with nine molecules of oxygen to produce six molecules of carbon dioxide and seven molecules of water.
