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The mean free path of nitrogen molecules at a pressure of 1.0 atm and temperature 0°C is 0.8 × 10-7 m. If the number density of molecules is 2.7 × 1025 /m3 , then the molecular diameter (in Å) is.
    Correct answer is '3.2'. Can you explain this answer?
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    The mean free path of nitrogen molecules at a pressure of 1.0 atm and ...

    n = 2.7 × 1025 /m3

    d = 3.2 × 10-10 m
    ⇒ d = 3.2Å
    The correct answer is: 3.2
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    The mean free path of nitrogen molecules at a pressure of 1.0 atm and ...
    To calculate the mean free path of nitrogen molecules, we can use the following formula:

    mean free path = (k * T) / (sqrt(2) * π * d^2 * P)

    Where:
    k = Boltzmann constant (1.38 * 10^-23 J/K)
    T = temperature (in Kelvin)
    d = diameter of the nitrogen molecule (3.0 * 10^-10 m)
    P = pressure (in Pascal)

    First, we need to convert the pressure from atm to Pascal. 1 atm is equal to 101325 Pascal.

    So, P = 1 atm * 101325 Pa/atm = 101325 Pa

    Then, we need to convert the temperature from °C to Kelvin. The temperature is given as 0°C, so we add 273.15 to convert it to Kelvin.

    T = 0°C + 273.15 = 273.15 K

    Now we can substitute the values into the formula:

    mean free path = (1.38 * 10^-23 J/K * 273.15 K) / (sqrt(2) * π * (3.0 * 10^-10 m)^2 * 101325 Pa)

    Calculating this equation will give us the mean free path of nitrogen molecules.
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    The mean free path of nitrogen molecules at a pressure of 1.0 atm and temperature 0°C is 0.8 × 10-7 m. If the number density of molecules is 2.7 × 1025 /m3 , then the molecular diameter (in Å) is.Correct answer is '3.2'. Can you explain this answer?
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