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  • Chemistry in Context
  • Phases and Classification of Matter
  • Physical and Chemical Properties
  • Measurements
  • Measurement Uncertainty, Accuracy, and Precision
  • Mathematical Treatment of Measurement Results
  • Module for Testing Functions of Various Items to See How They Generate in the PDF
A photo collage shows a cup of black coffee, a hand covered in foamy soap, a remote control, and a gasoline pump nozzle inserted into a vehicle’s gas tank.
Chemical substances and processes are essential for our existence, providing sustenance, keeping us clean and healthy, fabricating electronic devices, enabling transportation, and much more. (credit “left”: modification of work by “vxla”/Flickr; credit “left middle”: modification of work by “the Italian voice”/Flickr; credit “right middle”: modification of work by Jason Trim; credit “right”: modification of work by “gosheshe”/Flickr)

Your alarm goes off and, after hitting “snooze” once or twice, you pry yourself out of bed. You make a cup of coffee to help you get going, and then you shower, get dressed, eat breakfast, and check your phone for messages. On your way to school, you stop to fill your car’s gas tank, almost making you late for the first day of chemistry class. As you find a seat in the classroom, you read the question projected on the screen: “Welcome to class! Why should we study chemistry?”

Do you have an answer? You may be studying chemistry because it fulfills an academic requirement, but if you consider your daily activities, you might find chemistry interesting for other reasons. Most everything you do and encounter during your day involves chemistry. Making coffee, cooking eggs, and toasting bread involve chemistry. The products you use—like soap and shampoo, the fabrics you wear, the electronics that keep you connected to your world, the gasoline that propels your car—all of these and more involve chemical substances and processes. Whether you are aware or not, chemistry is part of your everyday world. In this course, you will learn many of the essential principles underlying the chemistry of modern-day life.

Exam PDF eBook: 
Final Exam Review
Download Final Exam PDF eBook
17 Pages
English US
Educational Materials

Sample Questions from the Final Exam Review Exam

Question: When the following equation is balanced, the coefficient of oxygen is _____. __C4H10 (g) + ___O2 (g) ? ___CO2 (g) + ___H2O (l)\







Question: A 250-ml stoppered flask contains a substance that occupies 25.0 mL. Which of the following statements is TRUE about the substance in the flask? (Not sure of the correct answer)


The substance CANNOT be a solid

The substance CAN ONLY be a liquid

The substance CAN ONLY be a gas

The substance CANNOT be a gas

The substance CAN ONLY be a liquid

Question: Calculate the molarity of a 2.00L solution of glucose (C6H12O6) which contains 50.0 grams of glucose. ( Don't have the correct answer for this problem yet.)


180. M





Question: Which of the following NOT isoelectronic with the others? (not sure of the correct answer)


oxide ion

fluoride ion

sodium ion

magnesium ion

calcium ion

Question: Which of the following is an example of a physical property?






both b and c

Question: The change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surrounding is ______J



1.91 x 10^7




Question: Calculate the mass of ammonium nitrate that must be heated to generated 10.0 g N2O according to the following balanced chemical equation: NH4NO3 (s) ? N2O (g) + 2 H2O (l)


18.2 grams

0.227 grams

9.10 grams

80.1 grams

44.0 grams

Question: Which of the following substances would be classified as a homogeneous solution?



copper wire


soft drink

sodium chloride

Question: Which of the following is the highest temperature?



302 K


the freezing point of water

Question: The value of \Delta?Ho for the reaction below is -126 kJ. _________ kJ are released when 2.00 mol of NaOH is formed in the reaction. 2Na2O2 (s) + 2H2O (l) ? 4NaOH (s) + O2 (g) (don't have correct answer for yet)


-3.9 kJ

-7.8 kJ

-126 kJ

-252 kJ

-63 kJ

Question: Which of the ions listed below has the smallest radius? (Not sure of the correct answer)







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Prateek Ashtikar
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Miranda Reising
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