CHEMISTRY 11_ TEXTBOOK_ Chapter 10 Review PDF

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NELSON TEXTBOOK CHEMISTRY GRADE 11 CHAPTER 10...

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Chapter 10 Understanding Concepts

1. From his experimental work with gases, John Dalton developed the law of partial pressures. State Dalton’s law of partial pressures (a) in a sentence; (b) as a mathematical equation. 2. Using the kinetic molecular theory, explain Dalton’s law of partial pressures. 3. A sample of sour natural gas contains gases with the following partial pressures: 230 kPa methane, 13 kPa ethane, and 7 kPa hydrogen sulfide. Calculate the total pressure of the sour natural gas mixture. 4. Oxygen gas generated by the decomposition of potassium chlorate is collected at SATP by the downward displacement of water. Calculate the partial pressure of the oxygen, assuming it is saturated with water vapour. (The vapour pressure of water is given in Table 3 of Section 10.1.) 5. From his experimental work with chemical reactions involving gases, Joseph Gay-Lussac developed the law of combining volumes. (a) Using your own words, state the law of combining volumes in a sentence. (b) Use the law of combining volumes to predict the volume of each gas produced when 5.00 L of oxygen gas is consumed in the complete combustion of trinitrotoluene, TNT. Assume all gases are measured at the same temperature and pressure. 4 C7H5(NO2)3(s)  21 O2(g)

(b) Bulbs heat up as they generate light. What will the pressure be inside a light bulb when the temperature rises to 200°C? (c) A steel tank contains 50.0 kg of compressed argon. If one fluorescent tube has an internal volume of 0.915 L, how many tubes can be filled from the tank? Assume a pressure of 100.4 kPa inside each tube when the temperature is 20°C. 9. One of the major sources of atmospheric sulfur dioxide, SO2(g), is the extraction of metals from their sulfide ores. Metal extraction often involves heating the metal sulfide in air to form the metal oxide and sulfur dioxide, for example, 2 ZnS(s)  3 O2(g)

2 ZnO(s)  2 SO2(g)

What volume of sulfur dioxide at SATP is produced by the reaction of 1.00 t of zinc sulfide with an excess of oxygen? 10. Sulfur dioxide released to the atmosphere forms acid rain, but it can also attack calcium carbonate directly (as seen in the sculpture in Figure 1). 2 CaCO3(s)  2 SO2(g)  O2(g)

2 CaSO4(s)  2 CO2(g)

If 500 kL of sulfur dioxide reacts at STP, (a) What volume of carbon dioxide gas at STP is produced? (b) What mass of calcium carbonate is consumed?

28 CO2(g)  6 N2(g)  10 H2O(g)

6. Amedeo Avogadro proposed an idea to explain the law of combining volumes. Avogadro’s idea is sometimes called a principle, a hypothesis, a law, and a theory. Is Avogadro’s idea empirical or theoretical? Explain your answer. 7. Disastrous explosions have resulted from the unsafe storage and handling of the fertilizer ammonium nitrate, which can decompose rapidly. 2 NH4NO3(s)

2 N2(g)  4 H2O(g)  O2(g)

What volume of gases measured at SATP is produced by the decomposition of 1.00 mol of ammonium nitrate? 8. Argon is used in incandescant light bulbs and fluorescent tubes at a pressure of 400 Pa above atmospheric pressure. (a) What amount of argon is required to fill a 125-mL light bulb when the temperature is 20°C and atmospheric pressure is 100.0 kPa? 492 Chapter 10

Figure 1

11. Sulfur trioxide in the atmosphere reacts with rainwater to form sulfuric acid. SO3(g)  H2O(l)

H2SO4(aq)

If 1.00 t of atmospheric sulfur trioxide dissolves in rainwater, what volume of 0.12 mmol/L sulfuric acid could be formed? 12. In a demonstration of the decomposition of water by electrolysis, 50.0 mL of hydrogen gas is produced at 23°C and 103 kPa. (a) What volume of oxygen gas is produced at the same temperature and pressure? (b) What would be the volume of hydrogen produced if it was measured at STP? (c) What mass of water is decomposed? 13. After 2.00 mol of N2(g) and 3.00 mol of H2(g) are added to a reaction vessel, the total pressure is measured at 200 kPa. Calculate the partial pressure of each gas in the vessel. 14. How does the molar volume of a gas change (a) when temperature increases? (b) when pressure increases?

Applying Inquiry Skills 15. Complete the Prediction, Analysis, and Evaluation sections of the following investigation report. Question What is the molar volume of propane, C3H8(g), at STP? Prediction (a) Predict the answer to the Question and state the basis for your Prediction. Experimental Design A small propane cylinder sold for home maintenance applications provides the propane gas that is collected at ambient pressure by water displacement. Evidence initial mass of propane cylinder  426.79 g final mass of propane cylinder  424.92 g volume of gas collected  1065 mL ambient pressure  98.23 kPa ambient temperature  21.0°C Analysis (b) Based on the Evidence, what is the answer to the Question? (The pressure must be adjusted to correct for the vapour pressure of water; see Table 3, Section 10.1.) Evaluation (c) Calculate the percentage difference. Does the answer based on the Evidence agree with your predicted value?

(d) Based on your evaluation of the Prediction, evaluate the authority you used to make your Prediction. 16. A cylinder of compressed gas is known to contain a noble gas. Design an experiment to identify the gas by its molar mass.

Making Connections 17. List one natural and one technological use or source for each of the following gases: (a) oxygen (b) methane (c) helium (d) air (e) water vapour (f) carbon dioxide 18. In the 1930s, chemists produced a series of synthetic chemicals called Freons. Some common Freons are CFCl3(g), CF2Cl2(g), C2F3Cl3(g), and C2F4Cl2(g). (a) What were some of the initial uses of Freons? (b) Why has the production of Freons been banned in many countries, including Canada? (c) What volume does 1.00 kg of escaped CF2Cl2(g) occupy at SATP? 19. Ethanethiol, C2H5SH(g), is a very smelly compound that is added to natural gas so that gas leaks can be detected easily. When the natural gas is burned, the ethanethiol undergoes combustion as well: 2 C2H5SH(g)  9 O2(g)

4 CO2(g)  6 H2O(g)  2 SO2(g)

(a) Calculate the volume at SATP of each gas produced when 1.00 g of ethanethiol is burned. (b) Discuss some of the risks and benefits of adding ethanethiol to natural gas. 20. Ontario’s Air Quality Index (AQI) network includes 33 state-of-the-art air quality monitoring stations across the province. Each AQI site monitors some or all of the six most common air pollutants: sulfur dioxide, ozone, nitrogen dioxide, total reduced sulfur compounds, carbon monoxide, and suspended particles. Locate the AQI station closest to your school, and research the source of the most common pollutant and the health risks associated with it. Prepare a one-page summary of your findings. Follow the links for Nelson Chemistry 11, Chapter 10 Review. GO TO www.science.nelson.com

Gas Mixtures and Reactions 493...