Question
Calculate the net energy change in kilo joules per mole that takes place on formation of MgF 2 (s) from the elements: Mg(s)+F2(g)MgF2(s) The following
Calculate the net energy change in kilo joules per mole that takes place on formation of MgF 2 (s) from the elements:
Mg(s)+F2(g)⟶MgF2(s)
The following information is needed:
Heat of sublimation for Mg(s)= 147.7 kJ/mol
Eea for F(g)= −328 kJ/mol
Bond dissociation energy for F2(g)= 158 kJ/mol
Ei1 for Mg(g)= 737.7 kJ/mol
Electrostatic interactions in MgF2(s)= −2957 kJ/mol
Ei2 for Mg(g)= 1450.7 kJ/mol
Express your answer to four significant figures and include the appropriate units.
Ef=???
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General Chemistry
Authors: Darrell Ebbing, Steven D. Gammon
9th edition
978-0618857487, 618857486, 143904399X , 978-1439043998
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