Asked by Basim

Estimate the change in energy when solid rubidium reacts with gaseous diatomic chlorine molecules. Express your answer in units of kJ/mole. Do not refer to the periodic table to solve this problem. The following data may be useful in your calculation:

Madelung Constant: 1.763
Born Exponent: 12
Heat of Vaporization of Rubidium: 75.77 kJ/mole
Ionization Energy of Rubidium: 4.177 eV
Covalent Radius of Rubidium: 2.16 Angstroms
Covalent Radius of Chlorine: 0.99 Angstroms
Electron Affinity of Chlorine: -349 kJ/mole
Dissociation Energy of Chlorine: 244 kJ/mole
Ionic Radius of Chlorine: 167 pm
Ionic Radius of Rubidium: 166 pm
Answered by a
delta H = Ecryst+Evaporization+E(Rb, ionization)+Edissociation+Eaffinity
Answered by chelo
that is what, not understand what you want to publicize.thanks for what you have done
Answered by b
-430.5
Answered by c
-422.24
Answered by amar chauhan
-435
by amar chauhan
Answered by Anonymous
amar I got -479 which was wrong can you break it down so I can see where I was wrong
Answered by Anonymous
I used the born haber cycle but got the wrong answer where in the notes can I double check my steps better?
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