1. a) If the pressure in the closed container is initially 1.00 atmospheres in a volume V = 0.50 liters at a room temperature of 20 degrees Celsius, find the number of moles of air in the container. How many air molecules are in the container, and what is the mass of that air? (Take air as 80% N, and 20% O2) PV= nRT L I at m x 0. 5 L = N x 8. 314 J / mol . k x 293K 4n= 0.098 mois 0. 098 mols x 6.022 E 23 molecules / mol : 5.92E 23 molecules L molar mass of air : 28. 97 91 mol L 0. 098 mois x 28. 97 g/ mol : 2. 89 b) The water temperature is now increased. What will the pressure (in SI units) be at 30, 40, 50, and 60 C? PV = nRT; D= nRT V 4 . 0 . 0 9 8 mols x 8 . 314 J / mol . K x 333 k = 271. 3 1 . 0 . 0 9 8 mols x 8. 314 J / mol . K x 303 k = 246.8 atm arm 2. 0 . 0 9 8 mols x 8 . 314 J / mol . K x 313 K = 255.0 atm 3 . 0 . 0 9 8 mols x 8. 314 J / mol . K x 323 k= 263. 2 atm 2 1. c) Draw a plot (hand drawn is OK) of the pressure vs. temperature between 20 and 60 degrees C, labelling the axes, including units, and showing your data points. Sketch a line showing the ideal gas law. pressure 3 temp ( co )