If the energies of two light radiations E_1 a | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) According to Planck's quantum theory,the energy of a photon is given by the relation: $E = \frac{hc}{\lambda}$ This implies that energy is inverse

Vedclass · Accepted Answer

$4:1$

Vedclass · Answer

(B) According to Planck's quantum theory,the energy of a photon is given by the relation: $E = \frac{hc}{\lambda}$ This implies that energy is inversely proportional to wavelength: $E \propto \frac{1}{\lambda} \Rightarrow \lambda \propto \frac{1}{E}$ Given the energies $E_1 = 25 \ eV$ and $E_2 = 100 \ eV$,the ratio of their wavelengths is: $\frac{\lambda_1}{\lambda_2} = \frac{E_2}{E_1}$ Substituting the given values: $\frac{\lambda_1}{\lambda_2} = \frac{100 \ eV}{25 \ eV} = \frac{4}{1}$ Therefore,the ratio $\lambda_1: \lambda_2$ is $4:1$.

If the energies of two light radiations $E_1$ and $E_2$ are $25 \ eV$ and $100 \ eV$ respectively,then their respective wavelengths $\lambda_1$ and $\lambda_2$ would be in the ratio $\lambda_1: \lambda_2=$

Similar Questions

For a $H$ atom,the wavelength for the highest energy transition is $91.2 \ nm$. Calculate the corresponding wavelength for $He^{+}$ in $nm$.

For which of the following species,Bohr's theory is not applicable?

Which of the following transitions will emit the shortest wavelength?

Which hydrogen-like species will have the same radius as that of the $1^{st}$ Bohr orbit of a hydrogen atom?

The series limit for the Balmer series of $H$ atom spectra is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module