[dhammikai]

Hi friends,
Could you please give me the answer of following question

Calculate the energy needed to remove the lectron from hydrogen (H) atom and from hydrogen ion (H⁺). Energy equation for any atom
E=[-4.34x10^-18]J/n²
So, I calculate as follows;
ΔE=E₂-E₁
ΔE=-4.34x10^-18(1/0-1/1)
ΔE=-4.34x10^-18 J

Then, if that required enegry is given as light. Calculate the wavelength in(nm) of the photon to associated with this transistion.
So I calculate this part as follows;

-4.34x10^-18=hc/λ
λ=[6.625x10^-34/4.34x10^-18)x3.0x10⁸
=4.5x10^-8m


And calculate the enrgy required for the formation of a mole hygrogen ions (H⁺)

So I need help for answer last part and please check my method for answers that I made here.

Thanks

[Corribus]

Your procedure seems generally right, although I didn't check for math or unit errors.  In this regard it helps to write out all the units in each step.  Also, I'm not sure what "(1/0)" is supposed to be.  I assume you mean "(1/∞)", but be careful with this kind of stuff.  Also you should specify where the term -4.34x10^-18 is coming from.

For the last part you need to solve, here is a hint: your answer to the first part is the amount of energy to remove a single electron from a single hydrogen atom.  You need to know how much energy is required to remove a mole of electrons from a mole of hydrogen atoms.  How do you do this?