How many molecules of O2 are in a 3.5 liter container? How many atoms? Must show work.
Ah, calculations. Brace yourself for a hilarious ride!
To determine the number of molecules of O2 in a 3.5 liter container, we'll need to invoke some scientific magic. First things first, let's convert liters to moles because why not, right?
We know that 1 mole of a gas occupies approximately 22.4 liters at standard temperature and pressure. So, 3.5 liters divided by 22.4 liters/mole gives us the number of moles. Let's call it "x".
Now, the mole is like the unit of comedy in the scientific world. They like to wear disguises as Avogadro's number, which is approximately 6.022 x 10^23. It's like having an army of little comedians!
To find the number of molecules, we'll multiply the number of moles (x) by Avogadro's number. This will give us the answer you're seeking!
But wait, there's more! The whole setup is because we're dealing with oxygen gas (O2), so it comes in pairs. Each molecule of O2 contains two oxygen atoms. Brace yourself, math fans!
To find the number of atoms, we'll take the number of molecules we just calculated and multiply it by 2 since there are 2 oxygen atoms in each molecule of O2.
And voila! You've got the number of molecules and atoms of O2 in your 3.5 liter container. It's like a clown car full of oxygen!
I hope that added a few giggles to your day. Remember, oxygen may be serious business, but science can still be fun!
To determine the number of molecules of O2 in a 3.5 liter container, we'll need to use the Ideal Gas Law equation: PV = nRT. This equation relates the pressure (P), volume (V), number of moles (n), gas constant (R), and temperature (T) of an ideal gas.
First, we need to convert the volume from liters to cubic meters since the gas constant (R) is in SI units. 1 liter is equal to 0.001 cubic meters.
V = 3.5 liters × 0.001 cubic meters/liter
V = 0.0035 cubic meters
Next, we need to calculate the number of moles (n) of O2. Rearranging the Ideal Gas Law equation, we have n = PV / RT. The pressure (P) and temperature (T) conditions must be specified.
Assuming the pressure is at standard atmospheric pressure (1 atm) and the temperature is at standard temperature (273.15 K), we have:
P = 1 atm
T = 273.15 K
R = 0.0821 L·atm/(mol·K) (gas constant)
n = (P × V) / (R × T)
n = (1 atm × 0.0035 m³) / (0.0821 L·atm/mol·K × 273.15 K)
n ≈ 0.0001508 moles
To find the number of molecules, we'll use Avogadro's number, which states that there are 6.022 × 10^23 molecules in one mole.
Number of molecules = number of moles × Avogadro's number
Number of molecules = 0.0001508 moles × 6.022 × 10^23 molecules/mole
Number of molecules ≈ 9.075 × 10^19 molecules
Thus, there are approximately 9.075 × 10^19 molecules of O2 in a 3.5 liter container.
To determine the number of atoms in O2, we'll need to multiply the number of molecules by 2 since each O2 molecule consists of 2 oxygen atoms.
Number of atoms = number of molecules × 2
Number of atoms = 9.075 × 10^19 molecules × 2 atoms/molecule
Number of atoms ≈ 1.815 × 10^20 atoms
Therefore, there are approximately 1.815 × 10^20 atoms of oxygen in a 3.5 liter container of O2.
To calculate the number of molecules and atoms, we need to use the ideal gas law and Avogadro's number. The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Avogadro's number (N_A) represents the number of particles (molecules or atoms) in one mole of a substance and is approximately 6.022 x 10^23.
1. Convert the volume from liters to moles:
To do this, we'll need to know the pressure and temperature of the gas. Since these values are not given, we'll assume standard conditions (STP), where 1 mole of gas occupies 22.4 liters at 1 atmosphere (760 mmHg) and 273 K (0°C).
So, converting 3.5 liters to moles at STP:
n = V / 22.4
n = 3.5 / 22.4
n ≈ 0.15625 moles
2. Calculate the number of molecules:
The number of molecules can be calculated by multiplying the number of moles by Avogadro's number:
Number of molecules = n × N_A
Number of molecules = 0.15625 × 6.022 × 10^23
Number of molecules ≈ 9.331 × 10^22 molecules (rounded to 3 significant figures)
3. Calculate the number of atoms in O2:
Since each O2 molecule consists of two oxygen (O) atoms, we can multiply the number of molecules by 2 to find the number of atoms:
Number of atoms = Number of molecules × 2
Number of atoms ≈ 9.331 × 10^22 × 2
Number of atoms ≈ 1.8662 × 10^23 atoms (rounded to 3 significant figures)
Therefore, there are approximately 9.331 × 10^22 molecules of O2 and 1.8662 × 10^23 atoms of oxygen in the 3.5 liter container.
There are 6.02 x 10^23 molecules in a mole. So how many moles do you have in 3.5 L (I assume this is at STP.).
There are 22.4 L for a mole of any gas at STP; therefore, moles O2 will be
3.5 L x (1 mole/22.4 L) = moles O2.
Now you can calculate the number of molecules with the 6.02 x 10^23 value. The number of atoms, of course, is just twice the number of molecules.