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# lab 5 - tube The initial temperature in the Erlenmeyer...

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Stoichiometry and the Ideal Gas Law By Robert Dutchen Lab Instructor: Samik Jhulki October 17, 2010

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Purpose: To determine the identity of an unknown nitrite salt involved in a reaction with sulfamic acid using the ideal gas law Procedure: The apparatus was assembled as shown in figure 5.1. Initially a 400 mL beaker was filled two-thirds of the way with water and a pipet bulb was used to remove air bubbles in the rubber tubing from the Erlenmeyer flask to the 400 mL beaker. 25 mL of Sulfamic acid and 70 mL of distilled water were added to the Erlenmeyer flask. Unknown nitrate salt #1 was placed into a 10x75 mm culture tube along with 3 mL of distilled water. Water was siphoned back into the Florence flask and the reaction was allowed to occur between the acid and salt with the 600 mL beaker replacing the 400 mL one. After all the salt reacted, the pressures were equalized by lifting the beaker. Observations: 1.208 g of unknown nitrate salt #1 was added to the culture
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Unformatted text preview: tube. The initial temperature in the Erlenmeyer flask was 24°C, the final temperature was 32°C. The average temperature was therefore 28°C (301.15 Kelvin). Atmospheric pressure within the lab room was 738 mmHg. The mass of the dry 600 mL beaker was 193.1 g. Results/Data: The mass of the 600 mL beaker at the conclusion of the experiment was 417.6 g, meaning the difference, or water displaced, was 224.5 g. This is the mass of the produced nitrogen gas, which is stoichiometrically equal to the moles of MNO 2 . P Total = P H2O + P N2 738 mmHg = 28.35 mmHg + P N2 P N2 = 709.65 mmHg D=M/V 0.997044g/cm³ = 224.5 g/V V= 223.8 cm 3 = 223.8 mL = .2238 L PV = nRT (.93375 atm)(0.2238 L) = n(0.08206 atm*L/mol*K)(301.15 K) n = .0085 mol N2 = .0085 mol MNO 2 Conclusion/Discussion: .0085 mol MNO 2 = 1.208 g 1 mol MNO 2 = 142.1 g 142.1 g – 46.0 g (NO 2 ) = 96. 1 g, which is closest to Rb in terms of weight...
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lab 5 - tube The initial temperature in the Erlenmeyer...

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