Given below are half cell reactions :
`MnO_(4)^(-)+8H^(+)+5e^(-)rarrMn^(2+)+4H_2O`
`E_(Mn^(2+)//MnO_4^(-))^(@) =-1.510 V`
`1/2O_2 +2H^(+)+2e^(-)rarrH_2O`
`E_(O_2//H_2O)^(@)=+1.223V`
Will the permanganate ion, `MnO_4^(-)` liberate `O_2` from water in the presence of an acid ?

Options

A. Yes, because `E_("cell")^@ = +0.287 V`
B. No, because `E_("cell")^@ = -0.287 V`
C. Yes, because `E_("cell")^@ = +2.733 V`
D. No, because `E_("cell")^@ = -2.733 V`