What is the lowest energy of the spectral line emitted by the hydrogen atom in the Lyman series? (h = Planck’s constant, c = velocity of light, R = Rydberg’s constant)

Calculate the wavelength (in nanometer) associated with a proton moving at $1.0\times 10^{3}m{s}^{-1}1.0\; \backslash times\; 10^3ms^\{-1\}$.(mass of proton $=1.67\times 10^{-27}kg=\; 1.67\; \backslash times\; 10^\{-27\}kg$ and $h=6.63\times 10^{-34}Js)h\; =\; 6.63\; \backslash times\; 10^\{-34\}\; Js)$

The energy required to break one mole of Cl-Cl bonds in $C{l}_{2}Cl\_2$ is 242 kJ ${\text{mol}}^{-1}\backslash text\{mol\}^\{-1\}$. The longest 2 wavelength of light capable of breaking a single Cl-Cl bond is

The frequency of light emitted for the transition n = 4 to n = 2 of $H{e}^{+}He^+$ is equal to the transition in H atom corresponding to which of the following?

Which of the following statements is correct for an electron that has the quantum numbers n = 4 and m = -2?

What is the ratio of energies of an electron is 1st orbit of $H{e}^{+}He^+$and H?

Radius of which orbit of $H{e}^{+}He^+$ is one half as that of 4th orbit of $B{e}^{3+}Be^\{3+\}$?

In an atom, an electron is moving with a speed of 600 m/s with an accuracy of 0.005%. Certainty with which the position of an electron can be located is ($h=6.6\times 10^{-34}kg{m}^2{s}^{-1}h\; =\; 6.6\backslash times\; 10^\{-34\}\backslash ,kg\backslash ,m^2s^\{-1\}$ ; mass of electron $e_m=9.1\times 10^{-31}kge\_m=\; 9.1\; \backslash times\; 10^\{-31\}\; kg$)

Ionisation energy of $H{e}^{+}He^+$is $19.6\times 10^{-18}J19.6\; \backslash times\; 10^\{-18\}J$ atom${}^{-1}^\{-1\}$. The energy of the stationary state (n = 1) of $L{i}^{2+}Li^\{2+\}$is

 A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emission is at 680 nm, the other is at