13.6eV is needed for ionisation of a hydrogen atom. An electron in a hydrogen atom in its ground state absorbs 1.50 times as much energy as the minimum energy required for it to escape ffrom the atom. What is the wavelength of the emitted electron? (`m_(e)= 9.109 xx 10^(-31)kg, e= 1.602 xx 10^(-19)` coulomb, `h= 6.63 xx 10^(-34) J.s`)

Explanation

To solve the problem, we will follow these steps:

### Step 1: Determine the energy absorbed by the electron
The energy required for ionization of a hydrogen atom is given as 13.6 eV. The electron absorbs 1.50 times this energy.

\[ \text{Energy absorbed} = 1.50 \times 13.6 \, \text{eV} = 20.4 \, \text{eV} \]
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