4 stoichiometry and the ideal gas law

# 4 stoichiometry and the ideal gas law - Mass of beaker with...

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Results and Discussion Purpose: To determine the identity of an unknown nitrite salt through reactions involving sulfamic acid, a nitrite salt, and the ideal gas law. Materials Used: 250 mL Erlenmeyer flask 500 mL Florence Flask 2 ringstands Pinch clamp 600 mL beaker Medicine dropper tip Rubber tubing Pipet bulb 10 x 75 mm culture tube 25.0 mL sulfamic acid solution Distilled water Unknown nitrite salt (of the general formula MNO 2 ) In order to determine the identity of an unknown nitrite salt of the general form MNO 2, the salt was dissolved in water and mixed with sulfamic acid. MNO 2 (aq) + HSO 3 NH2 (aq) MHSO 4 (aq) + H 2 O (l) + N 2 (g) The moles of nitrogen gas produced are related to the moles of MNO 2 that reacted with the sulfamic acid solution. As the sulfamic acid solution was slowly added to the unknown nitrite salt, water flowed into the 600 mL beaker as nitrogen gas was produced which displaced the water out. Calculations Mass of displaced water

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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 ºC 29.0 ºC = 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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4 stoichiometry and the ideal gas law - Mass of beaker with...

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