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How many grams of oxygen are required to burn 4.8 mol of butane?
Wiki User
∙ 12y ago
The balanced equation for the reaction is 2 C4H10 + 13 O2 -> 8 CO2 + 10 H2O. This shows that 13 moles of diatomic oxygen are required to burn 2 moles of butane. By proportionality, (4.8/2)13 or 31.2 moles of oxygen are required to burn 4.8 moles of butane. This corresponds to 31.2(32) or 1.0 X 103 grams of oxygen.
Wiki User
∙ 12y ago
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How many moles of CO2 form when 58 grams of butane C4H10 burn in oxygen?
The answer is 3,99 moles of carbon dioxide.
How many moles of co2 form when 58.0 g of butane c4h10 burn oxygen?
4 moles
How many moles of CO2 form when 58.0 g of butane C4H10 burn in oxygen?
4 moles
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What element must be present in order for something to burn?
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