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| 1 . |
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Calculate the molar mass of a gas if 4.40 g occupies 3.50 L at 560. torr and 41°C. Online Text [Hint]
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| 2 . |
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Calculate the density of SO2 gas at 0.960 atm and 35°C. Online Text [Hint]
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| 3 . |
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Calculate the density of H2S gas at 0.122 atm and 25.0°C. Online Text [Hint]
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| 4 . |
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Magnesium can be used as a "getter" in evacuated enclosures to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the metal.) If an enclosure of 0.382 L has a partial pressure of O2 of 3.50 x 10-6 torr at 27°C, what mass of magnesium will react according to the following equation? 2Mg(s) + O2(g) --> 2MgO(s) Online Text [Hint]
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| 5 . |
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Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid: 2NH3(g) + H2SO4(aq) --> (NH4)2SO4(aq) Calculate the volume of NH3(g) needed at 20°C and 25.0 atm to react with 15.0 kg of H2SO4. Online Text [Hint]
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| 6 . |
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Industrially, methane is converted to ethane via the following reaction: 2CH4(g) + 1/2O2(g) --> C2H6(g) + H2O(g) Calculate the volume of O2(g) needed at 500°C and 10.0 atm to react with 1.00 kg of CH4(g). Online Text [Hint]
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| 7 . |
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In the body, glucose, C6H12O6, can react with oxygen in an aerobic environment via the reaction C6H12O6(s) + 6O2(g) --> 6CO2(g) + 6H2O(l) or it can decompose in an anaerobic environment via the reaction C6H12O6(s) --> 2CO2(g) + 2C2H5OH(l) 289.6 g of glucose can produce what volumes of CO2(g) in each of the environments at STP? Online Text [Hint]
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| 8 . |
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How many liters of H2O(g) at STP would be required to produce 7.5 g of NH3(g) according to the equation shown below? Mg3N2(s) + 6H2O(g) --> 3Mg(OH)2(aq) + 2NH3(g) Online Text [Hint]
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| 9 . |
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Which of the following samples of gas would occupy the greatest volume at standard temperature and pressure (STP)? Online Text [Hint]
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| 10 . |
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How many liters of H2 gas collected at 750 torr and 25°C can be produced when 25.0 mL of aqueous 3.00 M HCl is allowed to react with an excess of magnesium metal according to the equation: 2HCl(aq) + Mg(s) ----> MgCl2(aq) + H(g)Online Text [Hint]
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| 11 . |
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A sample of hydrogen gas was collected over water at 21°C and at a pressure equal to the atmospheric pressure of 748 torr. The volume of the sample was 512 mL. How many grams of H2 are in the sample? (The vapor pressure of water at 21°C is 18.7 torr.) Online Text [Hint]
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| 12 . |
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Hydrogen gas is produced when zinc reacts with sulfuric acid: Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g) If 159 mL of wet H2 is collected over water at 24°C and a barometric pressure of 738 torr, how many grams of Zn have been consumed? (The vapor pressure of water is tabulated in Appendix B of the textbook.) Online Text [Hint]
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