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QUESTION 3 0.5 points Save Answer A flask is filled with 1.56 moles of a gas at 14.2 K and 636.7 mm Hg. The flask is then opened and an additional 1.56 moles are added. The temperature of the flask is then changed to 136.3 K. What is the pressure (in atm) of the flask under these final conditions? QUESTION 4 0.5 points Save Answer What is the density in g/L) of a gas with a molar mass of 177.9 g/mol at a pressure of 2.46 atm and a temperature of 73.02 °C? Click Save and Submit to save and submit. Click Save All Answers to save all answers.

Answer 1

kindly post different questions separately. please rate

3) PVL - DRT (ideal gas equation ) P. Pressure of gas R= ideal gas constant Ve volume of gas Te temperature na molo of gay Al constant volume P = P2 NITI Na Ta Here Piin, and Ti are initial pressure, moles and temperature respectarely. P2 ing and Tz are final pressure, mola and temperature respectively ni= 1.56 mol T = 14,2K Pi = 636.7 mm Hg = 0,838 atm ( 760 mm Hg = (atm) n2 = 1.56 mol + 1.56 mol = 3.12 mol Ta = 136.3k P2 = ? P2 = Pina Tz niti P2 = 0.838 at X 3.12 mol x 136.3k 156 mol X 14,2 12 P2 = 16.0 atm Hence final pressure is 16.0 catm