(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

Medium

$A$ 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 Questions

Class 11

Chemistry Questions

Chapter

Structure of Atom

Subtopic

Atomic models and Planck's quantum theory

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According to the Bohr model for the hydrogen atom,the radius of stationary orbits is proportional to which of the following?

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The ionization energy of a hydrogen atom is $13.6 \, eV$. What is the energy required (in $eV$) to excite the electron from the ground state to the first excited state?

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An electron in a hydrogen atom in its ground state absorbs $2$ times as much energy as the minimum required for it to escape from the atom. The kinetic energy of the emitted electron is ............ $eV$.

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Find the value of wave number $(\bar{v})$ in terms of Rydberg's constant,when the transition of an electron takes place between two levels of $He^{+}$ ion whose sum is $4$ and difference is $2$.

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Write down the limitations of Bohr's model.

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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

According to the Bohr model for the hydrogen atom,the radius of stationary orbits is proportional to which of the following?

The ionization energy of a hydrogen atom is $13.6 \, eV$. What is the energy required (in $eV$) to excite the electron from the ground state to the first excited state?

An electron in a hydrogen atom in its ground state absorbs $2$ times as much energy as the minimum required for it to escape from the atom. The kinetic energy of the emitted electron is ............ $eV$.

Find the value of wave number $(\bar{v})$ in terms of Rydberg's constant,when the transition of an electron takes place between two levels of $He^{+}$ ion whose sum is $4$ and difference is $2$.

Write down the limitations of Bohr's model.

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