Answered step by step
Verified Expert Solution
Link Copied!

Question

1 Approved Answer

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=???

 

Step by Step Solution

3.45 Rating (161 Votes )

There are 3 Steps involved in it

Step: 1

blur-text-image

Get Instant Access to Expert-Tailored Solutions

See step-by-step solutions with expert insights and AI powered tools for academic success

Step: 2

blur-text-image_2

Step: 3

blur-text-image_3

Ace Your Homework with AI

Get the answers you need in no time with our AI-driven, step-by-step assistance

Get Started

Recommended Textbook for

General Chemistry

Authors: Darrell Ebbing, Steven D. Gammon

9th edition

978-0618857487, 618857486, 143904399X , 978-1439043998

More Books

Students also viewed these Chemistry questions