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weqwewe [10]
2 years ago
13

A hydrogen-like ion is an ion containing only one electron. The energies of the electron in a hydrogen-like ion are given by the

following equation where n is the principal quantum number and Z is the atomic number of the element. En = −(2.18 10-18 J)Z2 (1/n2) Calculate the ionization energy (in kJ/mol) of the He+ ion.
Chemistry
2 answers:
Afina-wow [57]2 years ago
4 0

Answer:

oh ya z

Explanation:

i did it in my head

yan [13]2 years ago
3 0

Answer:

The ionization energy (in kJ/mol) of the helium ion is 21,004.73 kJ/mol .

Explanation:

E_n = -(2.18 10-18 J)\times \frac{Z^2}{n^2}

Z = atomic mass

n = principal quantum number

Energy of the electron in n=1,

E_1= -(2.18 10^{-18} J)\times \frac{4^2}{1^2}=-3.488\times 10^{-17} J

Energy of the electron in n = ∞

E_{\infty}= -(2.18 10^{-18} J)\times \frac{2^2}{\infty ^2}=0 J

Ionization energy of the He^+ ion:

I.E=E_{infty}-E_1=0-(-3.488\times 10^{-17} J)=3.488\times 10^{-17} J

I.E=3.488\times 10^{-20} kJ

To convert in into kj/mol multiply it with N_A=6.022\times 10^{23} mol^{-1}

I.E=3.488\times 10^{-20} kJ\times 6.022\times 10^{23} mol^{-1}=21,004.73kJ/mol

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<u>Answer:</u> The final equation has hydroxide ions which indicate that the reaction has occurred in a basic medium.

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Reduction half-reaction: MnO_4^-+2H_2O+3e^-\rightarrow MnO_2+4OH^-

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Reduction half-reaction: MnO_4^-+2H_2O+3e^-\rightarrow MnO_2+4OH^-             ( × 2)

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Reduction half-reaction: 2MnO_4^-+4H_2O+3e^-\rightarrow 2MnO_2+8OH^-

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Overall redox reaction: 3NO_2^-+2MnO_4^-+H_2O\rightarrow 3NO_3^-+2MnO_2+2OH^-

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