Answer Happy

Data for exp7: MM of a gas Mass of flask filled with air Mass of flask filled with gas Mass of flask filled with water Group 1 35.080 35.150 140.150 Group 2 35.120 35.190 140.190 Group 3 35.130 35.200 140.200 Use the masses given in the table instead of the masses in the example datasheet. Just change the values of m1, m2 and m3, and follow the same sequence for calculating the molar mass of the tested gas, and the percentage error.
Results & Calculations. m1 = 1- Mass of flask filled with air 2- Mass of flask filled with gas m2 = 3- Mass of flask filled with water m3 = 6.0 6.0 g g 4- Room temperature = 21°C + 273 = 296 K 5- Atmospheric pressure = 760 mmHg = 1 atm 6- Density of air under conditions of experiment = 7- Mass of water = m3 - m1 = g 8- Density of water = 1g / cm3 9- Volume of water = m 10- V.H₂O = V. flask = V. 11- Mass of air m air dair x Vair =step 6 x step 10 = 12- Mass of empty flask = m1 m air = step 1 - step 11 = 13- Mass of gas = m2 - m flask = step 2 - step 12 = g 14- Molar mass of a gas = m .gas x RXT/PxV 15- MM = step. 13 g x (0.0821 L.atm/ K.mol) x 296 K 1atm x step. 10 x 10-3 L g/mol H₂O / d H₂O = step 7/ step 8 = gas = V. air = cm3 g g/cm³ bo g cm³ 5.0 g 16 MM of the gas = 17- The gas is 18- The theoretical Molar Mass from periodic table = 19-% Error (Actual MM - Theoretical MM) / Theoretical MM x 100 = % g/mol