What is the volume of
2.8 × 10^6 molecules He?
Answer in units of L
mols Ha = 2.8E6 molecules/6.02E23 = ?
mols He x 22.4L/mol = L He.
I'm still not sure I'm doing this right.
I get 1.042E-16
To find the volume of 2.8 × 10^6 molecules of helium (He) in liters (L), we need to use the ideal gas law equation, which relates volume, pressure, temperature, and the number of moles of a gas.
The ideal gas law equation is: PV = nRT
Where:
- P is the pressure of the gas
- V is the volume of the gas
- n is the number of moles of the gas
- R is the ideal gas constant (0.0821 L·atm/mol·K)
- T is the temperature in Kelvin (K)
Since we are given the number of molecules (2.8 × 10^6 molecules) instead of the number of moles, we need to convert from molecules to moles. To do this, we use Avogadro's number, which states that one mole of any substance contains 6.022 × 10^23 particles (atoms, molecules, etc.).
So, to convert from molecules to moles, we divide the given number of molecules (2.8 × 10^6 molecules) by Avogadro's number (6.022 × 10^23 molecules/mol):
n = (2.8 × 10^6 molecules) / (6.022 × 10^23 molecules/mol)
Now we can substitute the values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
To solve for V, we need to know the values of P, R, and T. If the question does not provide these values, you would need to gather that information.
Once you have the values for P, R, and T, you can calculate the volume (V) in liters by substituting the numbers into the equation:
V = [(2.8 × 10^6 molecules) / (6.022 × 10^23 molecules/mol)] * (R * T / P)
Remember to convert the temperature to Kelvin if it is given in Celsius or Fahrenheit.