(B) $(B)$$\lambda = 0.57 \times 10^{-6} \ m$$E_{\text{photon}} = \frac{hc}{\lambda}$$\text{Power} = \frac{\text{Total Energy}}{\text{Time}} = \frac{n

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(B) $(B)$$\lambda = 0.57 \times 10^{-6} \ m$$E_{\text{photon}} = \frac{hc}{\lambda}$$\text{Power} = \frac{\text{Total Energy}}{\text{Time}} = \frac{n \times hc}{\lambda \times t}$$\text{Power} = \frac{14.33 \times 10^{19} \times 6.626 \times 10^{-34} \times 3 \times 10^8}{0.57 \times 10^{-6}}$$\text{Power} = \frac{28.49 \times 10^{-7}}{0.57 \times 10^{-6}} \approx 50 \ W$

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

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$A$ bulb emits monochromatic yellow light of the wavelength $0.57 \ \mu m$. If the rate of emission of quanta per second of the bulb is $14.33 \times 10^{19}$, the power of the bulb (in $Watt$) is $.....$

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A
$25$
B
$50$
C
$75$
D
$100$

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Class 11

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Chapter

Structure of Atom

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Atomic models and Planck's quantum theory

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$A$ bulb emits monochromatic yellow light of the wavelength $0.57 \ \mu m$. If the rate of emission of quanta per second of the bulb is $14.33 \times 10^{19}$, the power of the bulb (in $Watt$) is $.....$

Similar Questions

If the first emission in the Lyman series of a hydrogen atom occurs at $121.5 \ nm$,what will be the energy difference between the first and second orbits in $kJ/mol$?

The radius of the first orbit of $Li^{2+}$ is $X \mathring{A}$. The radius of the third orbit of $He^{+}$ (in $\mathring{A}$) is (in $X$)

The energy of an electron in a hydrogen atom in its ground state is $-13.6 \ eV$. The energy of the level corresponding to the quantum number equal to $5$ is ............. $eV$.

The radius of the second Bohr orbit,in terms of the Bohr radius,$a_{0}$,in $Li^{2+}$ is

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