(A) According to Einstein's photoelectric equation: $E = W + K.E._{max}$ $K.E._{max} = E - W$ Energy of incident photon $E = \frac{hc}{\lambda} = \fra

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(A) According to Einstein's photoelectric equation: $E = W + K.E._{max}$ $K.E._{max} = E - W$ Energy of incident photon $E = \frac{hc}{\lambda} = \frac{6.63 \times 10^{-34} \times 3 \times 10^{8}}{300 \times 10^{-9}} = 6.63 \times 10^{-19} \ J$ Given work function $W = 4.41 \times 10^{-19} \ J$ $K.E._{max} = 6.63 \times 10^{-19} - 4.41 \times 10^{-19} = 2.22 \times 10^{-19} \ J$ Converting to $10^{-21} \ J$: $2.22 \times 10^{-19} \ J = 222 \times 10^{-21} \ J$ Thus,the value is $222$.

Class 11 Chemistry Structure of Atom Atomic models and Planck's quantum theory

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The work function of sodium metal is $4.41 \times 10^{-19} \ J$. If photons of wavelength $300 \ nm$ are incident on the metal,the kinetic energy of the ejected electrons will be $\left( \dots \right) \times 10^{-21} \ J$. (Given: $h = 6.63 \times 10^{-34} \ J \cdot s; c = 3 \times 10^{8} \ m/s$)

JEE MAIN 2020 All JEE MAIN

A
$222$
B
$225$
C
$200$
D
$198$

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Structure of Atom

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The work function of sodium metal is $4.41 \times 10^{-19} \ J$. If photons of wavelength $300 \ nm$ are incident on the metal,the kinetic energy of the ejected electrons will be $\left( \dots \right) \times 10^{-21} \ J$. (Given: $h = 6.63 \times 10^{-34} \ J \cdot s; c = 3 \times 10^{8} \ m/s$)

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The surface of sodium metal is irradiated with radiation of wavelength $x$ nm. The kinetic energy of ejected electrons is $2.8 \times 10^{-20}$ $J$. The work function of sodium is $2.3$ eV. The value of $x$ is . . . . . . $\times 10^2$ nm.

The third line in the Balmer series corresponds to an electronic transition between which Bohr's orbits in hydrogen?

The wavelength of a particle having an Einstein energy of $1.995 \times 10^{12} \ erg \ mol^{-1} \ photon^{-1}$ is .......... $\mathring{A}$.

The radii of the first,second,third,and fourth Bohr orbits of hydrogen are respectively:

Energy of an electron is given by $E = -2.178 \times 10^{-18} \ J \left( \frac{Z^2}{n^2} \right)$. Wavelength of light required to excite an electron in a hydrogen atom from level $n = 1$ to $n = 2$ will be:

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