{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

Stoichiometry and the Ideal Gas Law

# Stoichiometry and the Ideal Gas Law - Temperature of H 2 O...

This preview shows pages 1–2. Sign up to view the full content.

Stoichiometry and the Ideal Gas Law By Julian Remouns Lab Instructor: Pasquale Iacono October 16, 2007

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
Results and Discussion: The identity of an unknown nitrite salt was determined by reacting the salt with sulfamic acid (HSO 3 NH 2 ) in the reaction: MNO 2 (aq) + HSO 3 NH 2 (aq) MHSO 4 (aq) + H 2 O (l) + N 2 (g), where M + is an alkali metal cation (Li + , Na + , K + , or Rb +) and the ideal gas law, PV=nRT, where P is pressure in atmospheres, V is volume in liters, T is temperature in Kelvin, n is the number of moles and R is the universal gas constant. Beaker with water (before reaction): 422.8g Nitrite Salt: 0.445g 70mL distilled water + 25mL sulfamic acid in flask Pressure in lab: 748mmHg = 98.4atm
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Temperature of H 2 O: 27 ° C + 273.15= 300.15K Pressure in H 2 O: 26.74mmHg = 3.52atm Beaker with water (after reaction): 682.4g 259.6g of water displaced = 259.6g of N 2 produced P total = P H2O +P N 98.4atm = 3.52atm + P N P N = 94.9atm V= 259.6g/ 0.9965g/mL = 260.5mL= 0.2605L PV=nRT 94.9atm (0.2605L) = n(0.08206atm ⋅ L/mol ⋅ K)(300.15K) (24.72 atm ⋅ L)/(24.63atm ⋅ L/mol) = n n N = 1.00mol 259.6g N 2 (1mol/28.0134g N 2 )= 9.267mol N 2 Conclusion: The nitrite salt was determined to be . The accuracy of the experiment was determined by calculating a percent error of %error = | |/ =...
View Full Document

{[ snackBarMessage ]}