Photoelectrons are removed with kinetic energy `1.864 xx 10^(-21)J`, when photons of light with energy ` 4.23 xx 10^(-19) J` fall on the metal. What is the minimum energy required per mole to remove an electron potassium metal?
Hint`: hv_(0)= hv-KE`
Energy required per mole `=hv_(0) xx 6.022 xx 10^(23)`

Explanation

To solve the problem, we need to find the minimum energy required to remove an electron from potassium metal per mole, given the kinetic energy of the photoelectrons and the energy of the incident photons.

### Step-by-Step Solution:

1. **Identify the given values**:
- Kinetic energy (KE) of the photoelectrons: \( KE = 1.864 \times 10^{-21} \, \text{J} \)
- Energy of the photons (E): \( E = 4.23 \times 10^{-19} \, \text{J} \)

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