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11. Propane (C3H8) burns in oxygen to produce carbon dioxide gas and water vapor:(a) Write a balanced equation for this reaction. (b) Calculate the number of liters of carbon dioxide measured at STP that could be produced from 7.45 g of propane.

Question

11. Propane (C3H8) burns in oxygen to produce carbon dioxide gas and water vapor:
(a) Write a balanced equation for this reaction.
(b) Calculate the number of liters of carbon dioxide measured at STP that could be produced from 7.45 g of propane.

check_circleAnswer
Step 1

The unbalanced chemical reaction is as follows:

The above reaction can be balanced by balancing the number of atoms of each element on both sides of the given reaction. The balanced chemical reaction should follow the law of conservation of mass.

The balanced chemical reaction is as follows:

Equation (1) represents the required balanced equation.

C3H)02()Co2(8) + H2O{g)
3CO2 (g)+4H20g)
C3Hg(g)502(g) ->
(1)
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C3H)02()Co2(8) + H2O{g) 3CO2 (g)+4H20g) C3Hg(g)502(g) -> (1)

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Step 2

From the balanced equation (1), it is evident that 1 mole of C3H8 produces 3 moles of CO2.

Number of moles of C3H8 can be calculated by the use of formula given below as,

Mass of C3H8 is 7.45 g.

Molar mass of C3H8 is 44.09...

mass of CH
3**8
mumber of moles of C3Hg
molar mass of C,Hg
7.45 g
moles of CHg
44.09 g-mol-
0.1689 moles
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mass of CH 3**8 mumber of moles of C3Hg molar mass of C,Hg 7.45 g moles of CHg 44.09 g-mol- 0.1689 moles

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