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Question

Considering natural gas in a laboratory burner to be pure methane, CH4, calculate the number of grams of carbon dioxide that would result from the complete burning of 35.0L of methane, measured at 749 torr and 22 degrees.

 

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Answer 1

First, you must write a correctly balanced equation for the reaction.

CH4 + 2O2 ==> CO2 + 2H2O

Next, find moles CH4 in 35.0 L at 749 torr and 22 degrees C:  PV = nRT and solve for n

n = PV/RT = (749 torr/760 torr/atm)(35.0 L)/(0.0821 Latm/Kmole)(295K) = 1.42 moles CH4

Next, using stoichiometry of the balanced equation, find moles of CO2 produced from this amount of CH4

1.42 moles CH4 x 1 moles CO2/mole CH4 = 1.42 moles CO2 produced

Finally, convert this to grams:  1.42 moles CO2 x 44 g/mole = 62.48 grams = 62.5 g (to 3 significant figures)