This is a 6 point assignment
Objectives: After completing this unit, students should be able to:
- Define terms such as energy, work, kinetic energy, potential energy, system, surroundings, state function, and enthalpy.
- State and apply the first law of thermodynamics.
- Relate changes in enthalpy to changes in internal energy.
- Distinguish between exothermic and endothermic processes.
- Given the change in enthalpy for a reaction, calculate the heat transferred for a given amount of reactant.
- Using the relationship: q = Sp Ht x m x ΔT, determine the values of one of the variables given the values of the others.
- Solve calorimetry problems using heat gain equals heat loss and q = Sp Ht x m x ΔT.
- Calculate ΔH for a reaction given ΔH values for reactions that can be combined (Hess’ Law) to yield the reaction of interest.
- Calculate the change in enthalpy for a reaction given the standard enthalpy of formation of reactants and products.
- Write equations that represent the standard enthalpy of formation of a substance.
Reading and Homework Exercises
Table of Contents from: OpenStax Chemistry 2e: Chapter 5
Introduction
5.1 Energy Basics
Questions 1-5 check your understanding of specific heat and heat capacity and your ability to solve problems using these properties.
Question 1:
Question 2:
Question 3:
Question 4:
Question 5:
5.2 Calorimetry
Questions 6-8 check your understanding of calorimetry problems and your ability to solve problems using the principle of heat loss = heat gain
Question 6:
Question 7:
Question 8:
5.3 Enthalpy
Questions 9 and 10 check your understanding of heat, work, and the first law of thermodynamics
Question 9:
Question 10:
Question 11 checks your understanding of the idea of state functions
Question 11:
Questions 12-15 check your understanding of heat of reaction
Please answer questions 12 and 13 for the reaction:
2 C3H6 + 9 O2 → 6 CO2 + 6 H2O
ΔH= -4116 kJ
Question 12:
Question 13:
Please answer questions 14 and 15 for the reaction:
2 H2O → 2 H2 + O2
ΔH= 572 kJ
Question 14:
Question 15:
Questions 16 and 17 check your understanding of Hess’s Law and your ability to use Hess’s law to calculate heat of reaction:
Question 16: Calculate the heat of reaction (ΔH) for the reaction:
Zn + S + 2 O2 → ZnSO4
given the following information:
Zn + S → ZnS ΔH = -206.0 kJ
ZnS + 2 O2 → ZnSO4 ΔH = -776.8 kJ
Question 17: Given the gas phase reactions:
NO + O3 → NO2 + O2 ΔH = -198.9 kJ
O3 → 3/2 O2 ΔH = -142.3 kJ
O2 → 2 O ΔH = 495.0 kJ
Calculate the heat of reaction (ΔH) for the reaction:
NO + O → NO2
Questions 18-22 check your understanding of Standard Enthalpies of Formation and your ability to use them to calculate heat of reaction:
Question 18:
Question 19:
Question 20:
For the reaction:
2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O(g)
Using the data in Appendix G, answer the following questions:
Question 21:
Question 22: