Hey there!:
Given, energy, E = 703 kJ/mol
λ = ?
We need to do conversion of kJ/mol to J
So, E = 703 kJ/mol*1000 J*kJ *1 mole / 6.023*10²³
= 1.17*10-18 J
We know formula,
E = h*C/ λ
So, λ = h*C / E
= ( 6.626*10-34 J.s ) * ( 3.0*10⁸ m.s⁻¹ ) / ( 1.17*10⁻¹⁸ J )
= 1.70*10⁻⁷ m
So, 1 m = 1*10⁹ nm
So, 1.70*10⁻⁷ m = ?
= 170 nm
Hope that helps!
The longest possible wavelength of light that could ionize an atom of bismuth is 169 nm.
Given that the first ionization energy of Bi is 703 KJ/mol, we have to find the energy of the photon;
E = 703 × 10^3/6.02 × 10^23
E = 1.17 × 10^-18 J
From the formula;
E = hc/λ
h = Plank's constant
c = speed of light
λ = wavelength
Making λ the subject of the formula;
λ = hc//E
λ = 6.6 × 10^-34 × 3 × 10^8/1.17 × 10^-18
λ = 1.69 × 10^-7 or 169 nm
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