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The Schrodinger wave equation for hydrog...

The Schrodinger wave equation for hydrogen atom is
`Psi_(2s)=(1)/(4sqrt(2pi))((1)/(a_(0)))^(3//2)(2-(r)/(a_(0)))e^(-sigma//a_(0))`
where `a_(0)` is Bohr's radius. If the radial node in 2s be at `r_(0)`, then `r_(0)` would be equal to :

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The correct Answer is:
A, B, C
b. `lambda = (h)/(mv)`("de Broglie's equation")`
`= (6.626 xx 10^(-34))/(100 xx 10^(-3) xx 100) = 6.626 xx 10^(-35) m `
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