Materials needed for this exam include a scientific calculator and a periodic table. If you don’t have a scientific calculator, you can use the calculator available at desmos.com (https://www.desmos.com/scientific). A periodic table from your course is included below for you to use. You can also reference an interactive version (https://www.rsc.org/periodic-table) from the Royal Society of Chemistry website.
1. Solids, liquids, and gases are the three most commonly accepted phases of matter. Explain the properties of each phase, including their relative energy.
2. Explain the differences between an ideal gas and a real gas.
3. Explain the process of sublimation. Name one substance that sublimes at room temperature and pressure.
4. The mole is a counting number that allows scientists to describe how individual molecules and atoms react. If one mole of atoms or molecules is equal to 6.022 × 1023 atoms or molecules, how many molecules are in a 23.45 g sample of copper (II) hydroxide, Cu(OH)2? (MM of Cu(OH)2 is 97.562 g/mol) Express your answer to the correct number of significant figures and you must show all work in the form of dimensional analysis as shown in Lesson 4.
5. The density of water at 4.00°C is 0.967 g/mL. How many molecules of water are present in a 499.8 mL bottle of water? Express your answer to the correct number of significant figures and you must show all work in the form of dimensional analysis as shown in Lesson 4.
6. A manufacturing company is trying to produce a lightweight but strong cart for use by home gardeners. Explain which metal—titanium (Ti), iron (Fe), or zinc (Zn)—would be the best for this application and why?
7. Combustion reactions are a notable source of carbon dioxide in the environment. Using the following balanced equation, how many grams of carbon dioxide are formed when 100.00 g of propane (C3H8) is burned? Express your answer to the correct number of significant figures and you must show all work in the form of dimensional analysis as shown in Lesson 4.
8. To obtain pure lead, lead (II) sulfide is burned in an atmosphere of pure oxygen. The products of the reaction are lead and sulfur trioxide (SO3). Write a balanced chemical equation for this process.
