Propane is used as a fuel for camp stoves. It undergoes combustion to form carbon dioxide and water.
C3H3 +502 – 3 CO2 + 4H20
Determine the number of molecules of propane needed to produce 10.01 liters of carbon dioxide

In this case, according to the given chemical reaction and the fact that 22.4 L of a gas are occupied by 1 mol at standard pressure and temperature conditions, it will be possible for us to calculate the number of molecules of propane, by using the Avogadro's number, the 1:3 mole ratio with carbon dioxide and the aforementioned volume-mole ratio to obtain:

[tex]10.01LCO_2*\frac{1molCO_2}{22.4LCO_2}*\frac{1molC_3H_8 }{3molCO_2} *\frac{6.022x10^{23}molec\ C_3H_8}{1molC_3H_8} \\\\=8.97x10^{22}molecules C_3H_8[/tex]

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Propane is used as a fuel for camp stoves. It undergoes combustion to form carbon dioxide and water. C3H3 +502 – 3 CO2 + 4H20 Determine the number of molecules of propane needed to produce 10.01 liters of carbon dioxide

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Propane is used as a fuel for camp stoves. It undergoes combustion to form carbon dioxide and water.
C3H3 +502 – 3 CO2 + 4H20
Determine the number of molecules of propane needed to produce 10.01 liters of carbon dioxide