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?
Hing`: hv_(0)= hv-KE`
Energy required per mole `=hv_(0) xx 6.022 xx 10^(23)`

Explanation

To solve the problem, we will follow the steps outlined in the video transcript and the hints provided.

### Step-by-Step Solution:

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

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