University:
Seattle Pacific University
Course:
CHM 1211 | General Chemistry I
Academic year:

2020
Views:

479

Pages:

2
Author:

Leilani Contreras

Ammonium nitrite (NH4NO2) decomposes upon heating to form N2 gas. NH4NO2(s) --> N2(g) + 2H2O When a sample of NH4NO2 is decomposed in a test tube 511 ml N2 is collected over water at 26oC and 745 torr total pressure. How many grams of NH4NO2 were decomposed? Total pressure of gas 745 torr Net pressure of gas = total pressure – water vapor pressure =(745 -25) torr = 720 Pressure in atm = 720torr X = 0.9473 Temperature = 26 o C = 299.149 K PV = nRT n= = =0.0197 moles molar mass of amm. nitrite =64.05g/mol grams of ammonium nitrite=0.01971 mols x 64.0520g/mol = 1.26 g ANSWER Ammonium nitrite (NH4NO2) decomposes upon heating to form N2 gas. NH4NO2(s) --> N2(g) + 2H2O When a sample of NH4NO2 is decomposed in a test tube 616 ml N2 is collected over water at 26oC and 766 torr total pressure. How many grams of NH4NO2 were decomposed? Total pressure of gas 766 torr Net pressure of gas = total pressure – water vapor pressure =(766 -25) torr = 741 Pressure in atm = 741torr X = 0.97499 Temperature = 26 o C = 299.149 K PV = nRT n= = =2.4454183320463604E-2 moles molar mass of amm. nitrite =64.0520g/mol grams of ammonium nitrite=2.4454E-2 mols x 64.052g/mol = 1.57 g ANSWER