Lecture Notes for Ch. 6

Lecture Notes for Ch. 6 - Chem 1036 Chapter 6 1 of 23 Chem...

Info iconThis preview shows pages 1–4. Sign up to view the full content.

View Full Document Right Arrow Icon
Chem 1036 Chapter 6 1 of 23 Chapter 6 Thermochemistry Thermodynamics: Thermochemistry: System Surroundings Chem 1036 Chapter 6 2 of 23 First Law of Thermodynamics First Law: Potential Energy Kinetic Energy Potential Energy: Kinetic Energy: Internal Energy: Chem 1036 Chapter 6 3 of 23 Units of energy: q = w = E = q + w Chem 1036 Chapter 6 4 of 23 Work (w) work = (-) work = (+) rinted with FinePrint - purchase at www.fineprint.com
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Chem 1036 Chapter 6 5 of 23 Units of work: Example Problem : Consider the following reactions. Does the system do work on the surroundings or does the surroundings do work on the system? a. C 2 H 2 (g) + 2H 2 (g) C 2 H 6 (g) b. 2N 2 O 5 (g) 4NO 2 (g) + O 2 (g) Example Problem : A gas is heated, causing it to expand from a volume of 2.0 L to 4.5 L at 1 atm pressure. Calculate the work of the system in joules (watch the sign). 101.3 J = 1 L atm Chem 1036 Chapter 6 6 of 23 Heat (q) Heat: Example: 2Al(s) + Fe 2 O 3 (s) 2Fe(s) + Al 2 O 3 (s) Exothermic: Chem 1036 Chapter 6 7 of 23 Example: Ba(OH) 2 (s) + 2NH 4 SCN(s) Ba(SCN) 2 (aq) + 2NH 3 (aq) + 2H 2 O Endothermic: Reactants Reactants Products Products q < O Exothermic q > O Endothermic Chem 1036 Chapter 6 8 of 23 System Surroundings input Heat release Heat q > 0; q < 0 endothermic T decrease; T increase sys surr surr sys q < 0; q > 0 exothermic T increase; T decrease sys surr surr sys Work done on system Work done on surroundings w > 0; w < 0 system compressed sys surr w < 0; w > 0 system expands sys surr q + w positive q + w decreases Energy of system increases Energy of system decreases rinted with FinePrint - purchase at www.fineprint.com
Background image of page 2
Chem 1036 Chapter 6 9 of 23 Example Problem : A system absorbs 30 kJ of heat and does 13 kJ of work. Calculate the internal energy change of the system.
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 4
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 6

Lecture Notes for Ch. 6 - Chem 1036 Chapter 6 1 of 23 Chem...

This preview shows document pages 1 - 4. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online