The combustion of propane, C,Hg, in a gas fuelled car, produces CO,, which is expelled from the exhaust pipe as gas (g): C,H, . 502 3CO, 4H,0 What is the volume of CO, produced, during a day of summer, at the temperature of 40°Cand a pressure of 99.5 kPa when 19.5g of propane are burned in this reaction? (Note the molecular weight of C3Hs is 44.1 g mol). Select one: O a.24.0 m2 O b.31.2 dm O c 34.7 dm² O d.4.71 m? O e. 2.37 dm3
The combustion reaction of propane is given by the following equation-
C3H8 + 5O2 ---> 3CO2 + 5H2O
Given, weight of C3H8 = 19.5 g
then, moles of C3H8=given mass/molar mass
= 19.5g/44.1gmol-1
= 0.442 mol
From the reaction, we have seen that
1 mol of C3H8 react to form 3 moles of CO2
Then,
0.442 mol C3H8 produced=0.442×3 mol CO2
= 1.326 mol CO2
To calculate the volume, we use ideal gas equation- PV = nRT
Given, P = 99.5 kPa = 99.5 × 103 Pa
= 99.5 × 10-2 atm
= 0.995 atm
n = 1.326 mol
R = 0.083 L atm/mol K
T = 40°C = 313 K
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