Step 1: Calculate the energy of the emitted photon.
Energy difference between two energy levels of hydrogen: \[ E = 13.6 \left( \frac{1}{1^2} - \frac{1}{2^2} \right) \text{eV} \] \[ E = 13.6 \left( 1 - \frac{1}{4} \right) = 13.6 \times \frac{3}{4} = 10.2 \, \text{eV} \] Convert to joules: \[ E = 10.2 \times 1.6 \times 10^{-19} = 1.632 \times 10^{-18} \, \text{J} \]
For a photon: \[ E = pc \Rightarrow p = \frac{E}{c} \] \[ p = \frac{1.632 \times 10^{-18}}{3 \times 10^8} = 5.44 \times 10^{-27} \, \text{kg·m/s} \]
The atom recoils with momentum equal and opposite to the photon’s: \[ p_{\text{atom}} = p_{\text{photon}} \] So, recoil speed: \[ v = \frac{p}{m} = \frac{5.44 \times 10^{-27}}{1.6 \times 10^{-27}} = 3.4 \, \text{m/s} \]
\[ v = \frac{x}{5} \Rightarrow 3.4 = \frac{x}{5} \] \[ x = 3.4 \times 5 = 17 \]
\[ \boxed{x = 17} \]
Step 1: Calculate Energy Difference (\(\Delta E\)):
- The energy levels for \(n = 1\) and \(n = 2\) in a hydrogen atom are given by:
\[ E_{n=1} = -13.6 \text{ eV}, \quad E_{n=2} = -3.4 \text{ eV} \]
- The energy difference \(\Delta E\) when the atom transitions from \(n = 2\) to \(n = 1\) is:
\[ \Delta E = E_{n=1} - E_{n=2} = -13.6 \text{ eV} + 3.4 \text{ eV} = 10.2 \text{ eV} \]
Step 2: Convert Energy to Joules:- \(1 \text{ eV} = 1.6 \times 10^{-19} \text{ J}\), so:
\[ \Delta E = 10.2 \times 1.6 \times 10^{-19} \text{ J} = 1.632 \times 10^{-18} \text{ J} \]
Step 3: Calculate Recoil Speed (\(v\)):
- Using \(v = \frac{\Delta E}{mc}\), where \(m = 1.6 \times 10^{-27} \text{ kg}\) and \(c = 3 \times 10^8 \text{ m/s}\):
\[ v = \frac{1.632 \times 10^{-18}}{1.6 \times 10^{-27} \times 3 \times 10^8} \]
- Simplify:
\[ v = 3.4 \text{ m/s} = \frac{17}{5} \text{ m/s} \]
Step 4: Determine \(x\):
- Since the recoil speed is \(\frac{x}{5}\), we have \(x = 17\).
So, the correct answer is: \(x = 17\)
A black body is at a temperature of 2880 K. The energy of radiation emitted by this body with wavelength between 499 nm and 500 nm is U1, between 999 nm and 1000 nm is U2 and between 1499 nm and 1500 nm is U3. The Wien's constant, b = 2.88×106 nm-K. Then,

What will be the equilibrium constant of the given reaction carried out in a \(5 \,L\) vessel and having equilibrium amounts of \(A_2\) and \(A\) as \(0.5\) mole and \(2 \times 10^{-6}\) mole respectively?
The reaction : \(A_2 \rightleftharpoons 2A\)