molar mass of a gas pre lab questions! 4 questions

timer Asked: Dec 6th, 2017
account_balance_wallet $15

Question description






CHEM 403 Exp 10 Experiment 10: MOLAR MASS OF A GAS* One of the important applications of the Ideal Gas Law is found in the experimental determination of the molar masses of gases and vapors. If the gas obeys the Ideal Gas Law, PV = nRT or n= PV RT (1) If the pressure P is in atmospheres, the volume V in liters, the temperature T in Kelvin, and the amount n in moles, then the gas constant R is equal to 0.0821 atm∙L/(mol∙K). From the measured values of P, V, and T for a sample of gas, Equation 1 can be used to find the number of moles of gas in the sample. The molar mass in grams, MM, is equal to the mass of the gas sample divided by the number of moles. MM = mass of gas sample n (2) This experiment involves measuring the molar mass of butane, C4H10, experimentally. A simple calculation using a periodic table would give the correct answer for the molar mass; however, you are going to conduct an experiment using the Ideal Gas Law in the lab to see how close you can come to the accepted value. You will measure the mass of the butane released from a pressurized container, and measure the volume of the gas that you collect. You can measure the temperature of the lab and atmospheric pressure, and use Equation 1 to find n, the number of moles of butane. Once you know the mass, and the number of moles, you can use Equation 2 to calculate an experimental molar mass. Procedure SAFETY WARNING: Butane is a flammable gas, and at NO TIME during this lab should there be any use of an open flame or other heat source! Determine the initial mass for the butane lighter provided by your instructor to the nearest 0.01 g. Set up a water basin for collecting a gas in an inverted graduated cylinder by water displacement. Fill a 100-mL graduated cylinder completely with water and carefully turn it upside down in the water basin so that there are no gas bubbles trapped in the cylinder. Using a ring stand and clamp, secure the graduated cylinder in place above the water basin. Submerge the butane lighter in the water basin and hold it directly underneath the graduated cylinder. Collect a sample of gas with a volume of approximately 70.0-90.0 mL. Take care to collect every bubble that leaves the lighter. If you miss a bubble, you will have to repeat the entire procedure beginning with re-weighing the clean and dry lighter. To perform your calculations correctly, the pressures inside and outside the graduated cylinder must be equal. Carefully adjust the cylinder up or down so that the water level inside the *Adapted from University of Florida’s Center for Precollegiate Learning and Training laboratory. CHEM 403 Exp 10 graduated cylinder is the same as the level outside the cylinder. This will equalize the pressure inside the graduated cylinder and is a key step in this experiment. Once the water levels are equal, record the volume of butane that has been collected in the cylinder. Measure and record the temperature of the water in the basin to 0.1 °C. This temperature will be used in your Ideal Gas Law calculation and will also be used to determine the vapor pressure of water in the graduated cylinder. Dry the lighter, then measure and record its mass to the nearest 0.01 gram. Refill your graduated cylinder with water and repeat the collection process for a second trial. Remeasure the temperature of the water after the second trial to account for any change. CHEM 403 – Exp 10 Name:______________________________ Section: _________ Data & Calculations Mass Trial 1 Trial 2 Initial mass of lighter ______________ g ______________ g Final mass of lighter ______________ g ______________ g Mass of butane collected ______________ g ______________ g Volume of gas collected* *after adjusting to equalize pressure ______________ mL ______________ mL Volume converted to liters ______________ L ______________ L Temperature of water in basin ______________ °C ______________ °C Temperature, in Kelvin, of butane (assume same temperature as water) ______________ K ______________ K Barometric pressure in laboratory, Ptotal ___________ mmHg ___________ mmHg Vapor pressure of water, Pwater (from Table provided by instructor) ___________ mmHg ___________ mmHg Pbutane (Ptotal – Pwater) ___________ mmHg ___________ mmHg Pbutane converted to atm (1 atm = 760 mmHg) ___________ atm ___________ atm Volume Temperature Pressure Number of moles Using Equation 1, calculate the number of moles of butane collected in each trial, using your experimental values of P (in atm), V (in L), T (in K), and R = 0.0821 atm∙L/(mol∙K). n (Trial 1) = _______________ mol n (Trial 2) = _______________ mol Experimental Molar Mass of Butane Using Equation 2, and your experimental values, calculate the molar mass of butane: MMexperimental (Trial 1) = _______________ g/mol MMexperimental (Trial 2) = _______________ g/mol MMexperimental (average) = _______________ g/mol Using a periodic table, calculate the accepted molar mass of butane, C4H10: MMaccepted = _______________ g/mol Calculate the percent error in your experimental value using the following equation: % error = |MMexperimental (average)–MMaccepted | MMaccepted x 100% % error = _______________ % CHEM 403 – Exp 10 Name:______________________________ Section: _________ Prelab Assignment In this experiment, there are several key steps that, if skipped, can have significant impact on the accuracy of your experimental molar mass of butane. For each of the following situations, explain which measured values (pressure, volume, temperature, mass of butane) would be affected, and follow the error through Equations 1 and/or 2 to determine how your experimental molar mass value would be affected. Would your molar mass value end up too high or too low? 1. During the butane gas collection, some of the butane bubbles were not collected in the graduated cylinder. 2. The water level in the graduated cylinder was not adjusted prior to recording the volume; the level of water in the graduated cylinder was above the water level. 3. You did not dry the butane lighter completely before obtaining a final mass. 4. You forgot to subtract the vapor pressure of water from the atmospheric pressure before performing your calculation of n.

Tutor Answer

Katrina S
School: Carnegie Mellon University

See attached solu...

flag Report DMCA

Goes above and beyond expectations !

Similar Questions
Hot Questions
Related Tags

Brown University

1271 Tutors

California Institute of Technology

2131 Tutors

Carnegie Mellon University

982 Tutors

Columbia University

1256 Tutors

Dartmouth University

2113 Tutors

Emory University

2279 Tutors

Harvard University

599 Tutors

Massachusetts Institute of Technology

2319 Tutors

New York University

1645 Tutors

Notre Dam University

1911 Tutors

Oklahoma University

2122 Tutors

Pennsylvania State University

932 Tutors

Princeton University

1211 Tutors

Stanford University

983 Tutors

University of California

1282 Tutors

Oxford University

123 Tutors

Yale University

2325 Tutors