Ask Question
1 July, 21:35

A hydrogen atom requires a minimum energy of 2.18*10^-18 J atom to remove an electron from its ground state level. Determine whether a blueviolet light with a wavelength of 434.0 nm can affect this process.

+4
Answers (1)
  1. 1 July, 23:59
    0
    Just find the energy of the blueviolet light with a wavelength of 434.0 nm using the formula:

    E = hc / lambda

    E = energy

    c = speed of light = 3 x 10^8 m/s

    h = planck's constant = 6.6 x 10^{-34} m^2 kg / s

    lambda = 434 nm = 434 x 10^{-9} m

    Putting these values (with appropriate units) in the above formula:

    we get: Energy, E = 4.5 x 10^{-19} J

    E = 0.45 x 10^{-18} J

    Now, the minimum energy is 2.18*10^-{18} J but our energy is 0.45 x 10^{-18} J which is less.

    Means the electron will not be removed
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A hydrogen atom requires a minimum energy of 2.18*10^-18 J atom to remove an electron from its ground state level. Determine whether a ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers