3 3 1 3 3 3 6 3 3 3 5 10 Data (work) experiment (1) Height of Sample = 0.569 g Flask + lover 79.0389 790389 Temp. of bath 37152 369k Barometric preshere = 762.762 mmHg 762.762 mmilty T = 15 >> of flask + Sample + lover = 79.607 g Volume 278 ml = (12) 0.8649 79.9029 278ml Calculations As outlined in the introduction, calculate the number of moles of sample that were present for each trial using the Ideal Gas Law (PV = nRT). Assume that the pressure of the gas at the time you take the temperature measurement is the same as the atmospheric pressure, and that the volume of the gas is equal to the volume of the flask. Then, using that number of moles and the weight of the sample, calculate the molar mass for each trial. Be sure that your units are consistent with the value of R (the ideal gas constant) that you use. Calculate a separate value of molar mass for each trial. Calculate the average value and the percent difference between the two values. If you trust one result more than the other, state which one and explain your reasoning.