How many liters of carbon dioxide at 20 oC and 750 torr are produced when one gallon of toluene is burned?
C7H8 + 9O2 ==> 7CO2 + 4H2O
1 gallon toluene = about 3,785 mL
density = about 0.867 g/mL
mass toluene = 3785 mL x 0.867 g/mL = 3282 grams.
moles toluene = grams/molar mass = 3282/92 = about 36 moles.
From the equation above, 1 mole C7H8 will produce 7 moles CO2; therefore, 36 moles toluene will produce 7 x 36 = about 250 moles CO2..
PV = nRT– V=250 X 8.314 X 293 / 750 = 812 L
Three errors:
1. When I posted this work about 3 hours ago, you will note I used about several times. You need to go through the math and calculate the individual steps to more precision than that.
2. You used the wrong R. If you use pressure in torr you must use 0.08205 L*atm/mol*K
3. If you intend to use torr, you must convert that to atmospheres. 750 torr = (750/760) atm.
I thin the answer is closer to 6,000 L but check my math on that.
To determine the number of liters of carbon dioxide produced when one gallon of toluene is burned, we need to follow these steps:
1. Convert the volume of toluene from gallons to milliliters. One gallon is equal to approximately 3,785 milliliters.
2. Determine the density of toluene. In this case, the density is stated to be about 0.867 grams per milliliter.
3. Calculate the mass of toluene by multiplying the volume (in milliliters) by the density. In this case, the calculated mass is 3,785 mL x 0.867 g/mL = 3,282 grams.
4. Determine the number of moles of toluene by dividing the mass (in grams) by the molar mass of toluene. The molar mass of toluene is approximately 92 grams/mol. So the calculated moles of toluene is 3,282 g / 92 g/mol = 36 moles.
5. Use the balanced chemical equation provided to determine the ratio of moles of toluene to moles of carbon dioxide. From the equation C7H8 + 9O2 -> 7CO2 + 4H2O, we see that one mole of toluene produces 7 moles of carbon dioxide.
6. Multiply the number of moles of toluene by the ratio obtained in step 5 to calculate the moles of carbon dioxide produced. In this case, 36 moles of toluene will produce 7 x 36 = 252 moles of carbon dioxide.
7. Finally, apply the ideal gas law, PV = nRT, to calculate the volume of the carbon dioxide produced. The given conditions are 20°C (or 293 Kelvin) and 750 torr of pressure. Rearranging the equation to solve for volume:
V = (nRT) / P
= (252 moles x 0.0821 L/mol·K x 293 K) / 750 torr
= 812 liters (rounded to 3 significant figures)
Therefore, approximately 812 liters of carbon dioxide at 20°C and 750 torr are produced when one gallon of toluene is burned.