1 / 14

STANDARD MOLAR ENTHALPY OF FORMATION

STANDARD MOLAR ENTHALPY OF FORMATION. Enthalpy change when 1 mol of species is formed in its Standard State at a Specified Temperature from the most stable forms of its constituent elements in their standard forms (at the same temperature). MOST STABLE FORM OF ELEMENT.

zaza
Download Presentation

STANDARD MOLAR ENTHALPY OF FORMATION

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. STANDARD MOLAR ENTHALPY OF FORMATION • Enthalpy change when 1 mol of species is formed in its Standard State at a Specified Temperature from the most stable forms of its constituent elementsin their standard forms (at the same temperature).

  2. MOST STABLE FORM OF ELEMENT • = Form favored in Equilibrium at 1 Atmosphere and specified temp. (usually 298.15 K) • e. g. for C at 298.15 K and 1 atmos., most stable form is GRAPHITE (not diamond!)

  3. STANDARD ENTHALPY OF FORMATION FOR CO2 • Hf0 CO2(gas) = Standard Enthalpy of Reaction for: • C (s, graphite) + O2 (g) CO2(g) • Nomenclature: • Hf0Std. State at 25 0C understood Formation

  4. ENTHALPY OF FORMATION • N.B. Hf0 for an ELEMENT in its Standard State = 0 • If not in its Standard State = 0 • e.g. For C (s, graphite) C (s, diamond) H0 = 1.895 kJ mol–1

  5. CALCULATION OF H FROM TABLE OF H VALUES • 1. Break down steps of reaction into: • (a) Decomposition of Reactants into Elements in Standard Forms • (b) Formation of Products from Elements in Standard States • 2. Apply HESS’S LAW

  6. HESS’S LAW Add 2 (or more) Reactions to give New Reaction, then Add Enthalpies in same manner to give Enthalpy of New Reaction

  7. HESS’S LAW

  8. CALCULATE ENTHALPY OF FORMATION FOR CO • Need Reaction: C(s, graphite) + ½ O2 CO2 (g) H= ??

  9. CALCULATE ENTHALPY OF FORMATION FOR CO (cont.) I.C(s, graphite) + O2 (g) CO2 (g) , H0 = -393.5 kJ mol –1 II. CO2 (g) – ½ O2 (g) CO (g) , H0 = +283.0 kJ mol –1

  10. APPLICATION OF HESS’S LAW • ADD I + II: C(s, graphite) + O2 (g) CO2 (g) , H0 = -393.5 kJ mol –1 II. CO2 (g) – ½ O2 (g) CO (g) , H = + 283.0 kJ mol –1 C(s, graphite) + ½ O2 (g) CO (g) H0 = -393.5 kJ + 283.0 kJ = -110.5 kJ mol-1

  11. HESS’S LAW

  12. DIFFERENT ALLOTROPIC & PHYSICAL FORMS OF ELEMENTS • e.g.red, white and black P • different forms of S • C (graphite and diamond) • Spacing and arrangement of atoms is different in Graphite and Diamond, and requires energy input to effect the transition from one form to the other.

  13. BOND ENTHALPIES • Energy used to BREAK Specific Bond in Gas Phase Reaction • N.B.Bond Enthalpies are ALWAYS +.

More Related