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| 1 . |
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Which of the following is (are) characteristic of gases? Online Text [Hint]
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| 2 . |
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How high must a column of water be to exert a pressure equal to that of a 760.-mm column of mercury? (The density of water is 1.00 g/mL, whereas that of mercury is 13.6 g/mL.) Online Text [Hint]
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| 3 . |
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In the United States, barometric pressures are reported in inches of mercury (in. Hg). On a beautiful summer day in Chicago, the barometric pressure is 30.45 in. Hg. Convert this pressure to torr. Online Text [Hint]
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| 4 . |
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Suppose that a woman weighing 135 lb and wearing high-heeled shoes momentarily places all her weight on the heel of one foot. If the area of the heel is 0.500 in.2, calculate the pressure exerted on the underlying surface in kilopascals. (Remember that 1.00 atm = 14.7 lb/in.2.) Online Text [Hint]
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| 5 . |
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Br2 is a liquid with a density of 3.03 g/mL. Determine the pressure in atm exerted by a column containing Br2 at a height of 1000. mm. The density of mercury is 13.6 g/mL. Online Text [Hint]
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| 6 . |
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A fixed quantity of gas at a constant temperature exhibits a pressure of 737 torr and occupies a volume of 20.5 L. Use Boyle's law to calculate the volume the gas will occupy if the pressure is increased to 1.80 atm. Online Text [Hint]
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| 7 . |
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A fixed quantity of gas at a constant pressure has a temperature of 22°C and a volume of 55.60 L. Use Charles's law to determine the volume of the gas if the temperature is increased to 38°C. Online Text [Hint]
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| 8 . |
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A balloon originally had a volume of 4.39 L at 44°C and a pressure of 729 torr. To what temperature must the balloon be cooled to reduce its volume to 3.78 L if the pressure is constant? Online Text [Hint]
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| 9 . |
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If 50.75 g of a gas occupies 10.0 L at STP, what will be the volume in L occupied by 129.3 g of the gas at STP? Online Text [Hint]
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| 10 . |
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At 46°C and 0.880 atm pressure, a gas occupies a volume of 0.600 L. How many liters will it occupy at 0°C and 0.205 atm? Online Text [Hint]
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| 11 . |
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Consider the reaction: 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) What volume of H2 is required to react with 10.0 L of NO and what volume of N2 is produced at 300°C? Online Text [Hint]
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| 12 . |
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Nitrogen gas reacts with hydrogen gas to produce ammonia gas: N2(g) + 3H2(g) --> 2NH3(g) What volume of H2 is required to react with 3.00 L of N2 and what volume of NH3 is produced at 200°C? Online Text [Hint]
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