1. Dr. Vinu Johnson, Ph.D. Chemistry Faculty
Preparing for ACS Exam General Chemistry -1 (1411) Part -3 (Chapters 8 & 9)
Dr. Vinu Johnson, Ph.D.
Chemistry Faculty

2. What I will talk about this morning:
Overview of ACS exam strategies discussed in Part-1.
Review of concepts from
Chapters 1 to 4: Part-1
Chapters 5 to 7: Part-2
Chapters 8 & 9: Part-3
Credit: Quotesgram.com

3. Exam Details: 70 Questions with four answer choices
110 minutes = 1.57 minutes per question !
Serial number
Sign Check-in form at the beginning of the exam.
Sign Check-out form at the end of the exam.
DO NOT MARK OR WRITE ON THE EXAM BOOKLET. THERE WILL BE A PENALTY IF YOU DO SO !!!

4. Exam giving strategies:
You will face 3 categories of questions:
Certain
50/50
Clueless
Make these 3 categories on a scratch paper
Read the question carefully – Time Management.
Based on your confidence write that Q# in one of the three categories. If it is a “certain” answer, mark it on the scantron form. If not, skip the question.

5. Exam giving strategies:
Scantron form:
Use a good condition form.
Check the Question number.
Mark the box completely
Erase completely if selecting another answer choice. √

6. Exam Preparation:
Every Chapter has a Summary section at the end of the textbook– look at it.
Start from first chapter – look at your notes.
Refer to the review slides for what you should know from each chapter.
Work out at least one example of that topic.
Practice giving tests.

7. Exam Preparation: On the day of Exam:
Relax - STRESS is a Memory Buster !
Psych yourself up – be CONFIDENT.
Close your eyes and revise the concepts.
Leave early (consider any traffic delays)
Be sure to bring a scantron form, calculator & pencil.
Be sure to have snacked / cup of coffee to keep your energy level up.
Do breathing exercise if you feel anxious.
National Education Association (nea.org)

8. Review of Concepts

9. Part-1 (Video)
Introduction
Chapter 1
Chapter 2
Chapter 3
Chapter 4
Part-2 (PowerPoint)
Chapters 5 - 7

10. Review of Concepts

11. THERMOCHEMISTRY: CHEMICAL ENERGY
CHAPTER 8
THERMOCHEMISTRY: CHEMICAL ENERGY
6 – 7 Questions
Define energy. Potential and kinetic energy.
concepts of heat and temperature
Define and calculate PV work. Know whether work is being done by the system or on the system.
Differentiate between energy and enthalpy, and perform calculations interconverting the two. H vs E.
Given a balanced chemical equation and enthalpy change for a chemical reaction, calculate the enthalpy change per mole or per gram of each reactant and product
Perform calculations involving specific heat (or molar heat capacity), heat flow, and temperature change, Specific Heat.
Enthalpy calculations based on Hess Law, Heats of formation, Bond Dissociation

12. THERMOCHEMISTRY: CHEMICAL ENERGY
CHAPTER 8
THERMOCHEMISTRY: CHEMICAL ENERGY
10.0 g of a metal, initially at 25°C, are placed into 10.0 g of water, initially at 100°C. Which metal will have the highest final temperature? Shown after each metal is its specific heat in J/(g∙°C).
A) aluminum (0.902)
B) copper (0.385)
C) gold (0.129)
D) iron (0.450)

13. THERMOCHEMISTRY: CHEMICAL ENERGY
CHAPTER 8
THERMOCHEMISTRY: CHEMICAL ENERGY
Given: 4 NO2(g) + O2(g) → 2 N2O5(g) ΔH° = kJ
find ΔH° for N2O5(g) → 2 NO2(g) + 1/2 O2(g).
A) kJ
B) kJ
C) 55.1 kJ
D) kJ

14. THERMOCHEMISTRY: CHEMICAL ENERGY
CHAPTER 8
THERMOCHEMISTRY: CHEMICAL ENERGY
Use the given standard enthalpies of formation to calculate ΔH° for the following reaction
3 Fe2O3(s) + CO(g) → 2 Fe3O4(s) + CO2(g).
A) kJ
B) kJ
C) kJ
D) kJ

15. THERMOCHEMISTRY: CHEMICAL ENERGY
CHAPTER 8
THERMOCHEMISTRY: CHEMICAL ENERGY
Use the given average bond dissociation energies, D, to estimate ΔH for the reaction of methane, CH4(g), with fluorine according to the equation:
CH4(g) + 2 F2(g) → CF4(g) + 2 H2(g)
A) -716 kJ
B) -318 kJ
C) +318 kJ
D) +716 kJ

16. GASES: THEIR PROPERTIES AND BEHAVIOR
CHAPTER 9
GASES: THEIR PROPERTIES AND BEHAVIOR
7 Questions
Perform calculations converting between different units of pressure
Determine the pressure of a gas using an open-end manometer.
Understand visual representations of the gas laws.
the ideal gas law to calculate pressure, volume, moles of gas, or temperature, given the other three variables.
Perform stoichiometric calculations relating the mass of a reactant to the mass, moles, and volume or pressure of a gaseous product.
Daltons law of Partial Pressure, Rate of diffusion.

17. GASES: THEIR PROPERTIES AND BEHAVIOR
CHAPTER 9
GASES: THEIR PROPERTIES AND BEHAVIOR
How many grams of XeF6 are required to react with L of hydrogen gas at 2.46 atm and 45°C in the reaction shown below?
XeF6(s) + 3 H2(g) → Xe(g) + 6 HF(g)
A) 3.65 g
B) 4.46 g
C) 13.4 g
D) 40.2 g

18. GASES: THEIR PROPERTIES AND BEHAVIOR
CHAPTER 9
GASES: THEIR PROPERTIES AND BEHAVIOR
Which of the following gases has the highest average speed at 400K?
A) N2
B) O2
C) F2
D) Cl2

19. GASES: THEIR PROPERTIES AND BEHAVIOR
CHAPTER 9
GASES: THEIR PROPERTIES AND BEHAVIOR
How many molecules of N2 are in a mL container at 780 mm Hg and 135°C?
A) 7.01 × 1021 molecules
B) 7.38 × 1021 molecules
C) 2.12 × 1022 molecules
D) 2.23 × 1022 molecules

20. All the Best !