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Experiment 4

# Experiment 4 - T= 22 ° C 273= 295 K.965 atm.329 L =...

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Stoichiometry and the Ideal Gas Law

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Results and Discussion: The identity of an unknown nitrate salt was determined by using a procedure that involves the reaction between sufamic acid and a nitrate salt, as well as the ideal gas law. The reaction is as follows: MNO 2 (aq) + HSO 3 NH 2 (aq) MHSO 4 (aq) + H 2 O (l) + N 2 (g) where M represents the alkali metal cation whose identity is to be determined by using the ideal gas law. The nitrogen gas produced from the reaction traveled to a water-filled flask and displaced a volume of water into a beaker. Thus, the volume of displaced H 2 O was equivalent to the amount of displaced N 2 . The volume was then used in the ideal gas law equation. PV= nRT P= 753.6 mmHg Ptotal= P H2O + P N2 P H2O = 19.83 mmHg P N2 = 753.6 mmHg- 19.83 mmHg =733.77 mmHg x (1 atm/ 760 mmHg) = .965 atm Mass H 2 O= 329.1 g/ (1.00 g/mL) x (1 L/1000 mL) Volume H 2 O = V N2 = .329 L n=? R= 0.08206 mmHg L/ mol K (K= degrees Kelvin)
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Unformatted text preview: T= 22 ° C + 273= 295 K (.965 atm)(.329 L) = n (.08206 mmHg L/ mol K) (295 K) n= .0131 mol N 2 .0131 mol N 2 x (1 mol N 2 / 1 mol MNO 2 ) = .0131 mol MNO 2 Mass MNO 2 = 1.2 g Molar Mass= 1.2 g MNO 2 / .0131 mol MNO 2 = 91.60 g/ mol Molar Mass – Mass of Nitrogen – Mass of Oxygen = Mass of M 90.60 g - 14. 01 g – 2( 16.00 g) = 45.59 g Given that the calculated mass of the cation does not correlate exactly to a particular cation, it will be assumed that the cation is K + , whose mass is closest to the calculated mass. Conclusion The identity of the unknown nitrite salt, 3385, is KNO 2 . When compared to the periodic table, the mass of the cation was closest to that of potassium, or K. The fact that the calculated mass of the cation does not directly match the masses on the periodic table is most probably due to human error, such as while massing the nitrite salt....
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