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The mass of reactants is equal to the mass of products.
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Most energy is produced by the breaking and reforming of molecular bonds. A car's combustion reaction in which fuel is converted into energy, co2 and water is a good example of this. Energy is rarely produced on the atomic level, such as a nuclear power plant or an atom bomb. Energy is produced this way through Einstein's E=mc^2. In an atomic reaction the mass of the products is slightly less then the mass of the reactants. Plug the change in mass into Einstein's equation and you get a lot of energy. To recap, most energy is made on the molecular level with endothermic (reactions which absorb energy) and exothermic reactions (reactions which emit energy), however a small amount takes place on the atomic level.
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The best example of the law of conservation of matter is complete combustion. If you were to burn something of known mass in a closed system, the system would have the same mass before and after combustion occurs.
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The answer is 24,15 g.
The mass of reactants is equal to the mass of products.
The mass of carbon dioxide is 878 g.
CO2 + Ca(OH)2 write a balanced equation for the combustion of benzene (C6H6)and find the mass of CO2 produced from the complete combustion of 25g benzene
Oxygen is NOT a PRODUCT (it is not produced) from the complete combustion of methane, it is a REACTANT (it is used in the reaction). The answer is therefore a mass of zero.
Burning 2 700 g of methane produce 70406 g of carbon dioxide.
According to Lavoisier: Mass reactants [total in] = mass products [total out] x g Methane + 32 g oxygen = 22 g carbon dioxide + 18 water x + 32 = 22 + 18 = 40 x = 40 - 32 = 8 g methane
Mass produced foods are foods that are produced by the thousands.
what is the mass in grams of oxygen, is needed to complete combustion of 6 L of methane?
During combustion carbon dioxide and water are released; ash is only the residue.
gears are best produced in mass production by