Let's evaluate each statement one by one:
The total spectral lines obtained from a single line during Zeeman effect is (2I +1 ).

This statement is correct. In the Zeeman effect, which occurs when the spectral lines split in the presence of a magnetic field, the number of split lines (spectral lines) is given by , where is the orbital angular momentum quantum number.
In the Lyman series as the energy liberated during transition increases then the distance between the spectral lines goes on decreasing.

This statement is incorrect. In the Lyman series of hydrogen, which involves transitions ending at the ground state , the energy liberated during transition decreases as you move to higher series (from Lyman to Paschen to Brackett, etc.). However, the wavelength (and thus the distance between spectral lines) increases as energy decreases. Therefore, the correct relationship is that as the energy decreases (transition to higher series), the distance between the spectral lines increases.

The highest probability of finding an electron in 1 s orbital is in the vicinity of the circumference.

This statement is incorrect. In the case of the 1 s orbital of hydrogen (and similarly for other s orbitals), the highest probability of finding the electron is at the nucleus (center) of the orbital, not at the circumference.
The highest probability of finding an electron in 1 s orbital is exactly at the middle between nucleus and circumference.

This statement is incorrect as well. The highest probability of finding an electron in the 1 s orbital is not exactly at the middle between the nucleus and the circumference (which would be the average radius). Instead, it is at the nucleus itself.

Conclusion:
The correct statement from the options given is only :
The total spectral lines obtained from a single line during Zeeman effect is (2l + 1).

Statements , , and are incorrect.