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What is the balanced equation of Butane?
2C4H10 + 13O2 ---------> 8CO2 + 10H2O This is a combustion reaction because carbon dioxide and water are products. This equation is balanced because on both sides there are 8 carbon atoms, 20 hydrogen atoms, and 26 oxygen atoms. Also these are the lowest possible coefficients (because there cannot be fractional coefficients). The trick to balancing this equation is to realize that the oxygen reactant is diatomic (so it starts out as O2).
What coefficient would the H2O have after balancing C4H10 plus O2 CO2 plus H2O?
2c4h10 + 13o2 => 8co2 + 10h2o (I am having some trouble with my typography today, but all those letters above should be capitalized.)
How many moles of CO2 form when 58.0 g of butane C4H10 burn in oxygen?
For the combustion of butane C4H10, the balanced chemical equation is: 2C4H10 + 13O2 -> 8CO2 + 10H2O. First, calculate the moles of butane: 58.0 g / 58.12 g/mol = 1 mole. From the balanced equation, 2 moles of butane produce 8 moles of CO2, so 1 mole of butane will produce 4 moles of CO2.
What happens when 1mole O2 react with butane?
When 1 mole of O2 reacts with butane (C4H10), a combustion reaction occurs forming carbon dioxide (CO2) and water (H2O) as products. The balanced chemical equation for the reaction is 2C4H10 + 13O2 -> 8CO2 + 10H2O.
Does combustion reactions form precipitates?
Combustion reactions typically do not form precipitates because they involve the rapid oxidation of a substance in the presence of oxygen to produce heat, light, and new chemical compounds like carbon dioxide and water vapor. Precipitates are more commonly formed in reactions where two aqueous solutions are mixed, resulting in the formation of an insoluble solid that falls out of solution.
