1
answer
0
watching
243
views
18 Nov 2019
The activation energy of the first-order decomposition of N2O into N2 and O is Ea= 250 kJ/mol. If the half-life of the reactant is t1/2= 7.5*10^6 s at 673K, what will it be at 773K?
The activation energy of the first-order decomposition of N2O into N2 and O is Ea= 250 kJ/mol. If the half-life of the reactant is t1/2= 7.5*10^6 s at 673K, what will it be at 773K?
Bunny GreenfelderLv2
4 May 2019
Related textbook solutions
Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232