The wave number of a light whose time period is 2.0 × 10–10 s would be:
1. 16.66 m-1
2. 1.66 m-1
3. 32.34 m-1
4. 12.34 m-1
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The number of photons of light with a wavelength of 4000 pm that provide 1J of energy would be:
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
Electromagnetic radiation of wavelength 242 nm is just sufficient to ionise sodium atom. The ionisation energy of sodium in kJ mol-1 is -
1. 494
2. 4.94
3. 516
4. 0.50
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
A 25-watt bulb emits monochromatic yellow light with a wave length of 0.57µm. The rate of emission of quanta per second would be :
1. 7.17×10-19 s-1
2. 4.13×1016s-1
3 . 7.17×1019 s-1
4 . 1.26 ×1020s-1
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The wavelength of light emitted when the electron in a H atom undergoes the transition from an energy level with n = 4 to an energy level with n = 2, is :
1. 586 mm
2. 486 nm
3. 523 nm
4. 416 pm
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The energy associated with the fifth orbit of a hydrogen atom is :
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The wave number for the longest wavelength transition in the Balmer series of atomic hydrogen would be -
1. \(1 . 1 . 52 \times \left(10\right)^{6} m^{- 1}\)
2. \(2 . 3 . 14 \times \left(10\right)^{6} \left(cm\right)^{- 1}\)
3. \(3 . 15 . 2 \times \left(10\right)^{6} m^{- 1}\)
4. \(4 . 1 . 52 \times \left(10\right)^{6} \left(cm\right)^{- 1}\)
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The energy of an electron in an H - atom is given by \(E_n=(-2.18 \times10^{-18})/n^2~\mathrm J.\) The shortest wavelength of light that can be used to remove an electron completely from \(n = 2\) orbit will be:
1. | \(3647~\mathring{\mathrm A}\) | 2. | \(5132~\mathring{\mathrm A}\) |
3. | \(3017~\mathring{\mathrm A}\) | 4. | None of these |
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The wavelength of an electron moving with a velocity of 2.05 × 107 m s-1 would be:
\(1 .\) \(4 . 65\) \(\times\) \(\left(10\right)^{- 12}\) \(m\)
\(2 .\) \(3 . 55\) \(\times\) \(\left(10\right)^{-11}\) \(m\)
\(3 .\) \(2 . 34\) \(\times\) \(\left(10\right)^{11}\) \(m\)
\(4 .\) \(6 . 43\) \(\times\) \(\left(10\right)^{ -11}\) \(m\)
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.
The kinetic energy of an electron is \(3.0 \times 10^{-25}~ \mathrm J.\) Its wave length would be:
1. | \(8.96 \times 10^{-7}~ \mathrm m\) | 2. | \(4.37 \times 10^{-6}~ \mathrm m\) |
3. | \(1.32 \times 10^{-7}~ \mathrm m\) | 4. | \(2.89 \times 10^{-4}~ \mathrm m\) |
To unlock all the explanations of this course, you need to be enrolled.
To unlock all the explanations of this course, you need to be enrolled.