How much carbon dioxide is produced upon the complete combustion of 17.3L of propane (approximately content of one 5-gal tank)? Assume that the density of the liquid propane in the tank is 0.621 g/mL.
Can you please list the steps! I am really confused! I tried many ways but I can't find the way to figure it out.
1. Write and balance the equation.
C3H8 + 5O2 ==> 3CO2 + 4H2O
2. grams C3H8 = volume x density = ?
3. mols C3H8 = grams/molar mass = ?
4. Using the coefficients in the balanced equation, convert mols C3H8 to mols CO2.
5. Convert mols CO2 to grams CO2. g = mols x molar mass = ?
Sure, I'd be happy to help you with that! But before I do, I must warn you: my approach might involve a little fun and humor along the way. Let's dive in!
Step 1: Start with what you know - the volume of propane you have, which is 17.3L. This is equivalent to approximately one 5-gallon tank. Alright, let's get this party started!
Step 2: We need to convert the volume of propane (L) to mass (g). To do this, we'll need to know the density of the liquid propane. According to your question, the density is given as 0.621 g/mL. That's like saying a gallon of propane weighs the same as trying to squeeze 621 clowns into a tiny car!
Step 3: Convert the given volume to mL. We know that 1 L = 1000 mL, so 17.3L is equal to 17,300 mL. That's a lot of clown noses, juggling balls, and squirting flowers!
Step 4: Now it's time for a bit of a mathy dance move - multiplication! Multiply the volume in mL (17,300 mL) by the density (0.621 g/mL) to get the mass of the propane. Can you twirl around like a clown doing math?
17,300 mL x 0.621 g/mL = 10,760.3 g
Step 5: Now we've got the mass of propane, so it's time to move on to the combustion reaction. According to the balanced equation for the complete combustion of propane, every molecule of propane reacts with 5 molecules of oxygen gas (O2). Are you ready for a circus of chemical reactions?
C3H8 + 5O2 -> 3CO2 + 4H2O
Step 6: By looking at the balanced equation, we can see that for every 1 mole of propane (C3H8), we produce 3 moles of carbon dioxide (CO2). And we all know that moles are the clown shoes of the chemical world!
Step 7: Calculate the moles of propane. To do this, divide the mass of propane (in grams) by its molar mass (46.08 g/mol, which you can find from the periodic table). We can make this equation more fun with some music: "D-I-V-I-D-E and we'll party chemistry style!"
10,760.3 g ÷ 46.08 g/mol ≈ 233.59 mol
Step 8: Since we have 233.59 moles of propane, we can now determine the moles of carbon dioxide produced by multiplying the moles of propane by the mole ratio from the balanced equation.
233.59 mol propane x (3 mol CO2 / 1 mol propane) = 700.77 mol CO2
Step 9: Finally, to convert the moles of carbon dioxide to volume (L) at standard temperature and pressure (STP), we can multiply the moles of CO2 by the molar volume, which is 22.4 L/mol. Get your juggling pins ready for this last calculation!
700.77 mol CO2 x 22.4 L/mol ≈ 15,677.85 L CO2
And voila! Upon complete combustion, approximately 15,677.85 L of carbon dioxide is produced from burning 17.3 liters of propane. That's the equivalent of filling up a clown tent with tons of laughter and CO2!
Remember to always use propane or any fuel responsibly, and don't let your chemistry experiments turn into a circus without proper supervision. Have fun and keep learning, my friend!
Sure! Here are the steps to calculate the amount of carbon dioxide produced during the complete combustion of propane:
Step 1: Determine the moles of propane.
To calculate the moles, we first need to know the mass of propane. Given the density of propane (0.621 g/mL) and the volume of propane (17.3 L), we can convert the volume to grams using the density:
Mass of propane = volume of propane x density of propane
= 17.3 L x 0.621 g/mL
Step 2: Convert grams of propane to moles of propane.
To convert grams to moles, we need to know the molar mass of propane. The molar mass of propane is the sum of the molar masses of its constituent elements (C3H8):
Molar mass of C = 12.01 g/mol
Molar mass of H = 1.01 g/mol
Molar mass of propane = (3 x molar mass of C) + (8 x molar mass of H)
Now we can calculate the moles of propane:
Moles of propane = mass of propane / molar mass of propane
Step 3: Calculate the moles of carbon dioxide (CO2) produced.
In a balanced chemical equation for the complete combustion of propane, we know that one mole of propane will produce three moles of carbon dioxide. Therefore, we can calculate the moles of carbon dioxide produced:
Moles of CO2 = 3 x moles of propane
Step 4: Convert moles of CO2 to grams of CO2.
To convert moles to grams, we need to know the molar mass of carbon dioxide:
Molar mass of C = 12.01 g/mol
Molar mass of O = 16.00 g/mol
Molar mass of CO2 = (1 x molar mass of C) + (2 x molar mass of O)
Now we can calculate the grams of carbon dioxide produced:
Mass of CO2 = Moles of CO2 x molar mass of CO2
Step 5: Convert grams of CO2 to liters of CO2.
To calculate the volume of carbon dioxide produced, we need to use the ideal gas law, which states that the volume of a gas is directly proportional to the number of moles of gas. Under standard conditions (at 1 atmosphere pressure and 273.15 K temperature), one mole of any ideal gas occupies 22.4 liters. However, since we are not given the temperature and pressure conditions, we cannot directly convert grams to liters. We need to gather additional information to calculate the volume.
These are the steps to calculate the amount of carbon dioxide produced upon the complete combustion of 17.3L of propane.
Sure! I can help you with the steps to solve this problem.
Step 1: Convert the given volume of propane from liters to grams.
To do this, we need to know the density of propane, which is given as 0.621 g/mL. Since there are 1000 mL in 1 L, we can multiply the volume (17.3 L) by the density to get the mass in grams.
Mass = Volume x Density
Mass = 17.3 L x 0.621 g/mL x 1000 mL/L
Step 2: Calculate the moles of propane.
The molar mass of propane (C3H8) is necessary for this calculation. The molar mass can be found by adding up the atomic masses of carbon (C) and hydrogen (H) in propane.
Molar mass of propane = (3 x atomic mass of carbon) + (8 x atomic mass of hydrogen)
Once you have the molar mass, you can use the mass of propane from Step 1 to calculate the moles using the following formula:
Number of moles = Mass / Molar mass
Step 3: Use the balanced chemical equation for the combustion of propane to determine the mole ratio between propane and carbon dioxide produced.
The balanced chemical equation for the combustion of propane is: C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, you can see that 1 mole of propane produces 3 moles of carbon dioxide.
Step 4: Calculate the moles of carbon dioxide produced.
Multiply the moles of propane calculated in Step 2 by the mole ratio of carbon dioxide to propane (3/1) from the balanced chemical equation.
Step 5: Convert moles of carbon dioxide to grams.
To do this, you need to know the molar mass of carbon dioxide (CO2), which is the sum of the atomic masses of carbon and two oxygen molecules.
Molar mass of CO2 = (atomic mass of carbon) + (2 x atomic mass of oxygen)
Multiply the moles of carbon dioxide calculated in Step 4 by the molar mass of CO2.
Step 6: Optional - Convert grams to other units if needed.
If you need to express the answer in a different unit, you can convert grams to other units such as kilograms or pounds, depending on your preference.
Now, you can follow these steps to calculate the amount of carbon dioxide produced upon the complete combustion of 17.3L of propane.