what is the mass of butane gas, c4h10, that can be held in a 3.00 L container at STP?
is it 0.13?
Well, I'm not a gas expert, but let's give it a whirl! So, to figure out the mass of butane gas (C4H10) that can be held in a 3.00 L container at STP (standard temperature and pressure), we'll need to use the ideal gas law and some molar mass magic.
First, we'll need to find the number of moles of butane gas in the container. We know that at STP, one mole of gas occupies 22.4 liters. So, using this ratio, we can calculate the number of moles of butane gas in the 3.00 L container.
Next, we need to find the molar mass of butane gas (C4H10). By adding up the atomic masses of the atoms in one molecule of butane, we get a molar mass of approximately 58.12 g/mol.
Finally, to find the mass of butane gas in the 3.00 L container, we can multiply the number of moles of butane gas by its molar mass.
But hey, you asked for humor, right? So, let me give you a dad joke to make the chemistry a little easier to digest: Why did the butane molecule never make it to the party? Because it was too busy being a gas-tastic introvert!
Now, back to business. Get your calculator ready because I'm about to do some math. I'm not a big math fan, but hey, I'll do it for you. Give me a sec...
Alright, after some calculating (or as I like to call it, number acrobatics), it turns out that the mass of butane gas that can be held in a 3.00 L container at STP is approximately 88.24 grams. Voilà!
I hope that adds a little lightheartedness to your gas calculations! Just remember, don't take my answers too seriously, unless you're brewing up some wacky chemistry experiments. Then maybe double-check with a real scientist.
To find the mass of butane gas (C4H10) that can be held in a 3.00 L container at STP (Standard Temperature and Pressure), we need to follow a series of steps.
1. Determine the molar mass of butane gas (C4H10).
- The molar mass is the sum of the atomic masses of all the atoms in the chemical formula.
- Carbon (C) has an atomic mass of 12.01 g/mol, and there are 4 carbon atoms in butane.
- Hydrogen (H) has an atomic mass of 1.01 g/mol, and there are 10 hydrogen atoms in butane.
- Calculating the molar mass: (4 * 12.01 g/mol) + (10 * 1.01 g/mol) = 58.12 g/mol.
2. Use the ideal gas law to calculate the moles of butane gas.
- The ideal gas law equation is: PV = nRT.
- P = pressure (STP is 1 atm).
- V = volume (3.00 L).
- n = moles of gas (what we need to find).
- R = ideal gas constant (0.0821 L·atm/mol·K).
- T = temperature (STP is 273.15 K).
- Rearranging the equation: n = PV / RT.
- Plugging in the values: n = (1 atm * 3.00 L) / (0.0821 L·atm/mol·K * 273.15 K) ≈ 0.131 mol.
3. Calculate the mass of butane gas using the moles and molar mass.
- Mass = moles * molar mass.
- Plugging in the values: Mass = 0.131 mol * 58.12 g/mol ≈ 7.61 g.
Therefore, the mass of butane gas (C4H10) that can be held in a 3.00 L container at STP is approximately 7.61 grams.
sadasda
1 mole C4H10 occupies 22.4 L @ STP and has a mass of 58 g.
So 3 L will be (3/22.4) = ? mols
I'll let you take it from there. I shall be happy to check your work if you post it.