Home
Class 11
CHEMISTRY
Electromagnetic Radiation of wavelength ...

Electromagnetic Radiation of wavelength 242 nm is just sufficient to ionize the sodium atom. Calculate the ionization energy sodium in kJ `"mol"^(-1)`.

Answer

Step by step text solution for Electromagnetic Radiation of wavelength 242 nm is just sufficient to ionize the sodium atom. Calculate the ionization energy sodium in kJ "mol"^(-1). by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 11 exams.

Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • SUPER MODEL QUESTION PAPER (FOR PRACTICE)

    SUBHASH PUBLICATION|Exercise PART-C|24 Videos

  • SUPER MODEL QUESTION PAPER (FOR PRACTICE)

    SUBHASH PUBLICATION|Exercise PART-D|32 Videos

  • SUPER MODEL QUESTION PAPER (FOR PRACTICE)

    SUBHASH PUBLICATION|Exercise PART-E|17 Videos

  • SUPER MODEL QUESTION PAPER (FOR ANSWER)

    SUBHASH PUBLICATION|Exercise PART-E|19 Videos

Similar Questions

Explore conceptually related problems

For a metal the maximum wavelength required for photoelectron emission is 340 nm, find the work function. If the radiation of wavelength 250 nm falls on the surface of the given metal. Find the maximum kinetic energy of emitted photo electrons in eV. Given Planck's constant = 6.625 xx 10^(-34) Js , velocity of light in vacuum is 3 xx 10^(8)ms^(-1) .

Calculate the frequency of electromagnetic radiation having the wavelength 3 mu . Calculate the wave number corresponding to it. ( 1 mu = 10^(-6) m)

Knowledge Check

  • Calculate the energy needed to convert three moles of sodium atoms in the gaseous to sodium ions. The ionization energy of sodium is 495 kJ mol^(-1)

    A
    1485 kJ
    B
    495 kJ
    C
    148.5 kJ
    D
    None of these

  • The frequency of radiation emitted when the electron falls from n = 4 to n = 1 in a hydrogen atom will be (given ionization energy of H = 2.18 xx 10^(-18) J atom^(-1) and h = 6.625 xx 10^(-25) Js)

    A
    `1.03 xx 10^3s^(-1)`
    B
    `3.08 xx 10 ^15s^(-1)`
    C
    `2.00 xx 10^15 s^(-1)`
    D
    `1.54 xx 10^15 s^(-1)`

  • A monochromatic light source of frequency villuminates a metallic surface and ejects photoelectron. The electron with maximum energy are just able to ionize the hydrogen atom in the ground state. When the whole experiment is repeated with an incident radiation of frequency 5/6 v, the photoelectrons so emitted are able to excite the hydrogen atom beam which then emits a radiation of the wavelength 1215Å . Find the work function of the metal :

    A
    6.875 eV
    B
    8.756 eV
    C
    7.568 eV
    D
    5.687 eV

    • Similar Questions

    Explore conceptually related problems

    Heat of neutralisation of a weak acid HA by NaOH is -"12.13 kJ mol"^(-1) . Calculate the enthalpy of ionization of HA.

    The threshold wavelength of a photosensitive metal is 662.5 nm. If this metal is irradiated with a radiation of wavelength 331.3 nm, find the maximum kinetic energy of the photoelectrons. If the wavelength of radiation is increased to 496.5 nm, calculate the change in maximum kinetic energy of the photoelectrons. (Planck's constant h=6.625xx10^(-34) Js and speed of light in vacuum = 3xx10^8 ms^(-1) )

    The threshold wavelength of a photosensitive metal is 662.5 nm. If this metal is irradiated with a radiation of wavelength 331.3 nm, find the maximum kinetic energy of the photoelectrons. If the wavelength of radiation is increased to 496.5 nm, calculate the change in maximum kinetic energy of the photoelectrons. (Planck's constant h = 6.625 xx 10^(-34) Js and "speed of light in vacuum" = 3 xx 10^(8)ms^(-1) )

    Ultraviolet radiations of wavelengths 800 Å and 700 Å when allowed to fall on Hydrogen atoms in their ground state, were found to liberate electrons with maximum kinetic energies 1.96 eV and 4.18 eV respectively. Calculate Planck,s constant and work function or ionisation energy of the hydrogen atom.

    The minimum energy in electron volt required to strip off ten times ionized sodium atom (i.e, Z = 11) of its last electron is

    Home
    Profile