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How can I use the amount of fuel to predict amount of product in a combustion reaction?
I am having some difficulty solving combustion reaction problems. I don't have problems balancing the equations, but when they are asking something like, 29.1 grams of butane reacts with excess oxygen to form carbon dioxide and water. How many grams of carbon dioxide form? Can you give me some pointers on how to approach this...?
Norm Rackison
Norm, try the following strategy.
 Write a balanced chemical equation for the combustion reaction.
For this problem, it's
C_{4}H_{10} + (13/2) O_{2} 5 H_{2}O + 4 CO_{2}
or
2 C_{4}H_{10} + 13 O_{2} 10 H_{2}O + 8 CO_{2}
if fractional coefficients bother you.
 Find moles of fuel from given information. You know you have 29.1 grams of butane. To convert grams to moles,
you must use the molecular weight. For butane, it's 4×12.011 + 10×18 = 58.124, so 58.124 g of butane is
equivalent to a mole of butane.
29.1 g butane

(  1 mol butane 58.124 g butane  ) 
= 0.50065 mol butane

(Notice this is an intermediate result so I'm not rounding off to the correct number of significant digits yet.)
 Convert moles of fuel to moles of product using mole ratios from the balanced chemical equation.
From the balanced equation, burning 2 moles of butane produces 8 moles of CO_{2}. So
0.50065 mol butane

(  8 mol CO_{2} 2 mol butane  ) 
= 226 mol CO_{2}

 Convert moles of product to desired units. You must convert moles of CO_{2} to grams of CO_{2}. The molecular
weight of CO_{2} is required:
226 mol CO_{2}

(  44.010 g CO_{2} 1 mol CO_{2}  ) 
= 88.1 g CO_{2}

 Check the answer. It makes sense that the mass of CO_{2} should be about triple the mass of butane, since 4 CO_{2} molecules weigh about 4×44 = 176 amu or about 3 times as much as one butane molecule (about 58.1 amu).
You can also check the answer by converting the 88.1 grams of CO_{2} obtained back into grams of butane. Do you get 29.1 g, within 3 significant figures?
Author: Fred Senese 
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General Chemistry Online! How can I use the amount of fuel to predict amount of product in a combustion reaction?
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