How much CO2 would be produced if 100 grams of propane burned in oxygen.

Question

i really dont understand

thanx

Answer 1

Your balanced equation is: C3H6 + 5O2 = 3CO2 + 4H2O.  First find the weight of propane.

C = 12 x 3 = 36

H = 1 x 8 = 8

Added together, they total 44 grams / mole.  Given 100 grams, divide by 44 = 2.27 moles propane.  Now look at the ratio of propane to CO2 from the equation = 1:3.  If 2.27 equals 1 mole propane, multiply by 3 to find the moles of CO2: 2.27 x 3 = 6.82 moles of CO2.  Each mole of CO2 weighs (C = 12 + O = 16 x 2 = 32) 44 grams per mole and since you have 6.82 moles, multiply by 44 grams = 300 grams CO2

Answer 2

Lily...first balance the reaction

C3H8  + 5 O2 ------- 3CO2+ 4H2O

so 1mole of propane ( 44 grams/mole ) yields 3 moles of CO2

so 100 grams of propane = 100g/44grams/mole  = 2.27 moles

since the relationship is 1:3  then 2.27 moles of propane will yield 3X 2.27 = 6.81 moles   if each mole of CO2 weighs 44 ( 12 +( 2 X 16) ) then the grams of CO2 produced will be 6.81 moles X 44grams/mole =

299.8 grams = 300 grams

proof

44 grams pf propane  ( 1 mole ) will yield 132 grams ( 3 moles ) of CO2

so 44/132 = 100/x   solve for x = 13,200/44 = 300 grams