The combustion of octane, C8H18, proceeds according to the reaction 2C8H18 (l) + 25O2(g) ------> 16CO2 (g) + 18H2O(l)
If 562 mol of octane combusts, what volume of carbon dioxide is produced at 35 Celsius and 0.995 atm? In liters?
I have never attacked a problem like this. Please help. Thank you!
If 562 mol of octane combusts, what volume of carbon dioxide is produced at 35 Celsius and 0.995 atm? In liters?
I have never attacked a problem like this. Please help. Thank you!
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First, find the number of moles of CO2, using the fact that 16 moles of CO2 result from the combustion of 2 moles of octane
(562 mol C8H18) (16 mol CO2/2 mol C8H18) = 4496 mol CO2
Now use the Ideal Gas Law, PV = nRT and solve for V. Don't forget to change the temperature to Kelvin by adding 273.
PV = nRT
(.995 atm) V = (4496 mol)(.082057 L atm mol^-1 K^-1)(308 K)
V = 114,200 Liters
1.14 x 10^5 liters, with the correct number of significant figures.
(562 mol C8H18) (16 mol CO2/2 mol C8H18) = 4496 mol CO2
Now use the Ideal Gas Law, PV = nRT and solve for V. Don't forget to change the temperature to Kelvin by adding 273.
PV = nRT
(.995 atm) V = (4496 mol)(.082057 L atm mol^-1 K^-1)(308 K)
V = 114,200 Liters
1.14 x 10^5 liters, with the correct number of significant figures.