Outlines of Theoretical Chemistry
The book Outlines of Theoretical Chemistry was written by author Here you can read free online of Outlines of Theoretical Chemistry book, rate and share your impressions in comments. If you don't know what to write, just answer the question: Why is Outlines of Theoretical Chemistry a good or bad book?
Where can I read Outlines of Theoretical Chemistry for free?
In our eReader you can find the full English version of the book. Read Outlines of Theoretical Chemistry Online - link to read the book on full screen. Our eReader also allows you to upload and read Pdf, Txt, ePub and fb2 books. In the Mini eReder on the page below you can quickly view all pages of the book - Read Book Outlines of Theoretical Chemistry
In our eReader you can find the full English version of the book. Read Outlines of Theoretical Chemistry Online - link to read the book on full screen. Our eReader also allows you to upload and read Pdf, Txt, ePub and fb2 books. In the Mini eReder on the page below you can quickly view all pages of the book - Read Book Outlines of Theoretical Chemistry
What reading level is Outlines of Theoretical Chemistry book?
To quickly assess the difficulty of the text, read a short excerpt:
The following table contains a few of the results obtained by Bodenstein at 448 C. Hydrogen, b. Iodine, a. HI calculated, 2x. HI observed, 2z. 20. 57 5. 22 10. 19 10. 22 20. 60 14. 45 25. 54 25. 72 15. 75 11. 90 20. 65 20. 70 14. 47 38. 93 27. 77 27. 64 8. 10 2. 94 5. 64 5. 66 8. 07 9. 27 13. 47 13. 34 It is of interest to note that a change in pressure does not alter the equilibrium in this gaseous system. Making use of the partial pressures of the components of the gaseous system instead of t...he concentrations, we have Pff 2 * Ph _ j? rf ~ p ' PHI Now let the total pressure on the system be increased to n times its original value; then the partial pressures are all increased in the same proportion, and we have which is equivalent to the original expression, since n cancels out. The equilibrium is thus seen to be independent of the pres- sure. This is only true for those systems in which a change in volume does not occur. (b) Dissociation of Phosphorus Pentachloride. When phos- phorus pentachloride is vaporized it dissociates according to the following equation Applying the law of mass action, we have 320 THEORETICAL CHEMISTRY Starting with 1 mol of phosphorus pentachloride, which if undis- sociated would occupy the volume V, under atmospheric pressure, and letting a denote the degree of dissociation, the molecular con- centrations at equilibrium will be as follows: Cpa ' = Letting (1 + a) V = V, and substituting in the above equation, we have At 250 C.
What to read after Outlines of Theoretical Chemistry?
You can find similar books in the "Read Also" column, or choose other free books by Frederick Hutton Getman to read onlineMoreLess
To quickly assess the difficulty of the text, read a short excerpt:
The following table contains a few of the results obtained by Bodenstein at 448 C. Hydrogen, b. Iodine, a. HI calculated, 2x. HI observed, 2z. 20. 57 5. 22 10. 19 10. 22 20. 60 14. 45 25. 54 25. 72 15. 75 11. 90 20. 65 20. 70 14. 47 38. 93 27. 77 27. 64 8. 10 2. 94 5. 64 5. 66 8. 07 9. 27 13. 47 13. 34 It is of interest to note that a change in pressure does not alter the equilibrium in this gaseous system. Making use of the partial pressures of the components of the gaseous system instead of t...he concentrations, we have Pff 2 * Ph _ j? rf ~ p ' PHI Now let the total pressure on the system be increased to n times its original value; then the partial pressures are all increased in the same proportion, and we have which is equivalent to the original expression, since n cancels out. The equilibrium is thus seen to be independent of the pres- sure. This is only true for those systems in which a change in volume does not occur. (b) Dissociation of Phosphorus Pentachloride. When phos- phorus pentachloride is vaporized it dissociates according to the following equation Applying the law of mass action, we have 320 THEORETICAL CHEMISTRY Starting with 1 mol of phosphorus pentachloride, which if undis- sociated would occupy the volume V, under atmospheric pressure, and letting a denote the degree of dissociation, the molecular con- centrations at equilibrium will be as follows: Cpa ' = Letting (1 + a) V = V, and substituting in the above equation, we have At 250 C.
What to read after Outlines of Theoretical Chemistry?
You can find similar books in the "Read Also" column, or choose other free books by Frederick Hutton Getman to read onlineMoreLess
Write Review:
Guest
Read Also
8 / 10
User Reviews: