What is the volume of
2.8 × 106 molecules He?
Answer in units of L
mols = #molecules/6.02E23
mols x 22.4L/mol = ?L
1.042E-16?
To find the volume of 2.8 × 10^6 molecules of helium (He) in liters (L), we need to use Avogadro's law which states that equal volumes of gases at the same temperature and pressure contain the same number of molecules.
Avogadro's number, which gives the number of molecules in one mole of a substance, is approximately 6.022 × 10^23.
First, let's find the number of moles in 2.8 × 10^6 molecules of He:
Number of moles = (Number of molecules) / (Avogadro's number)
Number of moles = (2.8 × 10^6) / (6.022 × 10^23)
Number of moles ≈ 4.64 × 10^-18 moles (rounded to 3 decimal places)
Next, we need to convert the number of moles to volume in liters using the ideal gas law equation, where V represents volume, n represents the number of moles, and R is the ideal gas constant (which is approximately 0.0821 L·atm/(mol·K)):
V = (n × R × T) / P
Since the question does not provide temperature (T) or pressure (P), we will assume standard temperature and pressure (STP):
Standard Temperature (T) = 273.15 K
Standard Pressure (P) = 1 atm
Plugging these values into the equation:
V = (4.64 × 10^-18 moles) × (0.0821 L·atm/(mol·K)) × (273.15 K) / (1 atm)
V ≈ 1.23 × 10^-17 L (rounded to 3 decimal places)
Therefore, the volume of 2.8 × 10^6 molecules of helium is approximately 1.23 × 10^-17 liters.
To find the volume of 2.8 × 106 molecules of helium (He) in liters, you need to use the ideal gas law equation and convert the units accordingly.
The ideal gas law equation is written as:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
In our case, the given information is the number of molecules (2.8 × 106) instead of the number of moles. To convert the number of molecules to moles, we need to use Avogadro's number, which states that there are 6.022 × 10^23 molecules in one mole of any substance.
So, let's do the calculations:
1. Convert from molecules to moles:
Number of moles (n) = Number of molecules / Avogadro's number
n = (2.8 × 106) / (6.022 × 10^23)
2. Now, substitute the values into the ideal gas law equation to find the volume:
PV = nRT
V = nRT / P
V = [(2.8 × 106) / (6.022 × 10^23)] * (0.0821 L·atm/(mol·K)) * (room temperature in Kelvin)
Note: Room temperature is generally around 298 K. However, if a specific temperature is given in the question, use that value.
3. Finally, solve for V to get the volume in liters.
By following these steps and plugging in the values, you can determine the volume of 2.8 × 106 molecules of helium (He) in liters.