Accelerated Chemistry Gas Laws Test Review/ Extra Practice

Accelerated Chemistry Gas Laws Test Review/ Extra Practice

<p>Name: Date: Pd: Partner:</p><p>Accelerated Chemistry Gas Laws Test Review/ Extra Practice</p><p>1. Would it be easier to drink water with a straw on the top or at the foot of Mt. Everest? Explain. – At the foot. A greater external air pressure pushing down on the surface of the liquid means only a small amount of air needs to be evacuated from the straw for there to be a great enough pressure difference for the liquid to rise up into the straw.</p><p>2. Samples of two substances, A and B, are in contact with each other. The mass of a molecule of substance A is twice the mass of a molecule of substance B. The average kinetic energy of the molecules in the two substances is the same. a. Compare the average velocities of the particles of substances A and B. – The average velocity of substance A is less than the average velocity of substance B.</p><p> b. How do the temperatures of the two substances compare? - The temperature of both samples is the same.</p><p> c. Will heat flow from one substance to the other? Explain your answer. – No, the average KE of substances A and B are the same. They are already at the same temperature. There will be no energy (or heat) flow.</p><p>3. Suppose you have two vials, one containing ammonia, and the other containing chlorine. When they are opened across the room, which would you expect to smell first? Why? - Ammonia. It has a smaller molar mass, therefore a larger average SPEED. It will diffuse more quickly.</p><p>4. Draw an open-end manometer to show the heights of mercury if a trapped gas has a pressure of 720 mm Hg and the atmospheric pressure is 760 mm Hg. Clearly the label the manometer to show the pressure of each gas and ∆ h. – We will discuss in class.</p><p>1 5. A scuba diver with a lung capacity of 5.2 L inhales a lungful of air at a depth of 4.5 m and a pressure of 5.5 atm. If the diver were to scent to the surface (where the pressure is 1.0 atm) while holding her breath, to what volume would the air in her lungs expand? – 29 L</p><p>6. The total pressure in a 11.7-L automobile tire is 44 psi at 11°C. By how much does the pressure in the tire rise if it warms to a temperature of 37°C and the volume remains at 11.7 L? – 48 psi, change of 4 psi.</p><p>-6 7. Tetrofluoroethylene, C2F4, effuses through a barrier at a rate of 4.6x10 mol/h. An unknown gas, consisting only of boron and hydrogen, effuses at the rate of 5.8x10-6 mol/h under the same conditions. What is the molar mass of the unknown gas? – 63 g/mol</p><p>8. A cylinder of compressed gas is labeled “Composition: 4.5 mol H2S, 3.0 mol CO2, 2.5 mol N2.” The pressure gauge attached to the cylinder reads 46 atm. Calculate the partial pressure of each gas, in atmospheres, in the cylinder. - H2S = 21 atm, CO2 = 14 atm, N2 = 11 atm</p><p>9. Solid zinc reacts with hydrochloric acid to produce zinc chloride and hydrogen gas. This reaction acts as a hydrogen generator for laboratory work and is collected by water displacement. Write the balanced equation. If 325 mL of hydrogen gas is collected over water at 25C at a total pressure of </p><p>2 748 mm Hg, how many grams of Zn reacted? (Use your Student Handout to determine the partial pressure of water vapor.)- 0.826 g Zn</p><p>10.Analysis of a gaseous chlorofluorocarbon, CClxFy shows that it contains 11.79% C and 69.57% Cl. In another experiment, you find that 0.107 g of the compound fills a 458 mL flask at 25˚C with a pressure of 21.3 mm Hg. What is the molecular formula of the compound? – C2Cl4F2</p><p>11.One of the cylinders of an automobile engine has a volume of 400. cm3. The engine takes in air at a pressure of 1.00 atm and a temperature of 15C and compresses the air to a volume of 50.0 cm3 at 77C. What is the final pressure of the gas in the cylinder? (The ratio of before and after volumes – in this case, 400:50 or 8:1 – is called the compression ratio.) – 9.72 atm</p><p>3</p>

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