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Understanding Thermodynamics: Heat Transfer and Hess's Law in Chemistry

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16 diapositives · 302 Views · Oct 02, 2014

Explore the fundamentals of thermodynamics, focusing on energy relationships in chemical systems through key concepts like temperature, heat, and enthalpy (ΔH). Learn how to measure temperature in Celsius and Kelvin, understand energy in joules or calories, and grasp the significance of energy transfer during chemical reactions. Differentiate between exothermic and endothermic processes using real-world examples, and discover Hess's Law for calculating changes in enthalpy indirectly. This guide will enhance your understanding of energy dynamics in chemistry.

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  1. Heat & Hess’ LAW

  2. Thermodynamics and Hess’ law

  3. Thermodynamics • Study of energy relationships in a chemical system • We will look at energy in terms of three concepts • Temperature • Heat • Enthalpy (H)

  4. Key Terms that you should know/recognize Temperature - measurement of avg. KE of particles in an object Heat - heat is the transfer of energy btw 2 objects due to a ∆ temperature Enthalpy ( H) - total energy in a chemical system - we will be concerned with the TRANSFER of enthalpy (∆ H)

  5. Measuring All these “things” • Temperature ( Celsius and Kelvin) • Energy (joules or calories) • Ability of a system to do work or supply ( or produce) heat • Heat (CANNOT MEASURE) • We can only measure through changes in temperature

  6. Units of Energy • Calorie (cal) is the amount of energy needed to raise one gram of water by 1 °C. • kcal = energy needed to raise 1000 g of water 1 °C. • food calories = kcals. Tro's "Introductory Chemistry", Chapter 3

  7. Change in Heat • Example • Window in the winter time • Energy always flows in the same direction → • When does the energy flow stop?

  8. Enthalpy (H) Energy is stored in chemicals, found in bonds that hold atoms together As chemical rxn takes place, bonds break, new bonds are created, energy is exchanged Change in energy is change in enthalpy

  9. Exothermic vs. Endothermic • Energy can be released or absorbed • Heat releasing (Exothermic) Reactants --> Products + E H = (-) • Heat Absorbed (Endothermic) Reactants + E --> Products H = (+)

  10. S + O2 SO2 ∆H= -296 kJ/mol a. How much heat is released when 275 grams of sulfur is burned?

  11. S + O2 SO2 ∆H= -296 kJ/mol b. How much heat is released when 25 mol of sulfur is burned in excess oxygen?

  12. S + O2 SO2 ∆H= -296 kJ/mol c. How much heat is released when 150.0 grams of sulfur dioxide is produced?

  13. Hess’ Law Some chemical reactions we cannot carry out in a calorimeter they release or absorb tons of energy We must indirectly calculate the change in energy for these reactions We use Hess’ Law

  14. Hess’ Law • Before we discuss Hess’ Law we must first talk about Energy • Energy is a state function • This means that the pathway one uses to get from one energy level to another is not important

  15. Hess’ Law Change in enthalpy for any equation can be calculated without actually carrying out the reaction Just simply add up the H of other related experiments

  16. 2NO2 (g) --> N2O4 (g) N2(g) + 2O2(g) --> 2NO2 (g) H = 67.8 kJ N2(g) + 2O2 (g) --> N2O4 (g) H = 9.67 kJ