Statement-1: The possible number of electrons in a subshell is $(4\mathrm{l} + 2)$. 

Statement-2: The possible number of orientations of a subshell are $(2\mathrm{l} + 1)$.

There are "2l+ 1" orbitals in each of the quantum number "l" subshells. No more than two electrons can be positioned in each orbital in accordance with Pauli's exclusion principle. Thus, the maximum number of electrons is simply equal to two times the number of orbitals used, or 
2(2l +1) =$4\mathrm{l}+2$

Number of subshells that can exist in one subshell,
 = $2\mathrm{l} + 1$