Step 1: Using Einstein’s Photoelectric Equation The photoelectric equation is given by: \[ h f = \phi + K_{\text{max}} \] where:
- \( h f \) is the incident photon energy,
- \( \phi \) is the work function,
- \( K_{\text{max}} \) is the maximum kinetic energy of the emitted electrons. Photon energy is related to wavelength by: \[ E = \frac{hc}{\lambda} \] where:
- \( h c = 12400 \) eV·Å,
- \( \lambda \) is the wavelength in Å.
Step 2: Calculating Photon Energies For \(\lambda_1 = 3100\) Å: \[ E_1 = \frac{12400}{3100} = 4 \, eV \] For \(\lambda_2 = 1550\) Å: \[ E_2 = \frac{12400}{1550} = 8 \, eV \]
Step 3: Using the Given Condition Let the initial kinetic energy be \( K_1 \), and the final kinetic energy be \( K_2 = 3K_1 \). Using the photoelectric equation: \[ E_1 = \phi + K_1 \] \[ E_2 = \phi + 3K_1 \] Substituting values: \[ 4 = \phi + K_1 \] \[ 8 = \phi + 3K_1 \] Solving for \( \phi \): \[ (8 - 4) = (3K_1 - K_1) \] \[ 4 = 2K_1 \] \[ K_1 = 2 \, eV \] Substituting \( K_1 \) in \( \phi = 4 - K_1 \): \[ \phi = 4 - 2 = 2 \, eV \] Thus, the correct answer is \( \mathbf{(3)} \ 2 \, eV \).

Observe the following data given in the table. (\(K_H\) = Henry's law constant)
| Gas | CO₂ | Ar | HCHO | CH₄ |
|---|---|---|---|---|
| \(K_H\) (k bar at 298 K) | 1.67 | 40.3 | \(1.83 \times 10^{-5}\) | 0.413 |
The correct order of their solubility in water is
For a first order decomposition of a certain reaction, rate constant is given by the equation
\(\log k(s⁻¹) = 7.14 - \frac{1 \times 10^4 K}{T}\). The activation energy of the reaction (in kJ mol⁻¹) is (\(R = 8.3 J K⁻¹ mol⁻¹\))
Note: The provided value for R is 8.3. We will use the more precise value R=8.314 J K⁻¹ mol⁻¹ for accuracy, as is standard.