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Unformatted text preview: Mass of beaker with water: 394.6 g Mass of beaker after reaction: 668.1 g Mass of displaced water= 668.1 g 394.6 g = 273.5 g Volume of nitrogen gas Density = Mass/Volume Volume = Density x Mass Volume = 1.0 g/mL x 273.5 g Volume of displaced water = 273.5 mL = 0.2735 L = Volume of nitrogen gas Temperature in Kelvin Temperature in laboratory: 29.0 C 29.0 C = 302.0 K Pressure of nitrogen gas Pressure (from p. 68 in lab booklet): 30.04 mmHg P Total = P H20 + P N2 747 mmHg = 30.04 mmHg + P N2 P N2 = 716.96 mmHg = 0.93421 atm Moles of nitrogen gas produced PV = nRT (0.93421 atm)(0.2735 L) = n(0.082057)(302.0K) n = 0.01031 mol Evaluation of results: A possible source of error is that the system may not have been completely airtight, and then some nitrogen gas could have escaped. Some measurements could have been taken inaccurately, such as with the reading of the water at the end of the experiment....
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