Purpose
To derive an experimental value of R and compare it to the published value. A known mass of a metal is reacted with hydrochloric acid to form hydrogen gas, H2. The volume, pressure, temperature and number of moles of the gas are calculated, allowing for the calculation of R.
Introduction
The ideal gas law, PV=nRT can be used to calculate the relative measure quantities of a sample of gas. Knowing three of the four measured quantities (n,P,V and T) we can calculate the fourth if R is known. In this lab we will experimentally determine R by generating a sample of gas and measuring the four quantities and calculating the gas constant by two methods. The procedure for this experiment is based on the chemical reaction between Mg and HCl to produce H2(g):
1 Mg(s) + 2 HCl(aq) ---> 1 MgCl2(aq) +1 H2(g)
The exact mass of Mg will be measured and using the above equation, the moles of H2 produced can be determined. (The reaction goes to completion) The experiment is done in a gas collection tube which is calibrated, so the volume will be easily read. Before measurements are taken, the gas system will be left to equilibrate to the ambient room temperature which can thus be easily measured. Determining the pressure however is a little more challenging. The hydrogen is collected in a eudiometer tube over an aqueous solution and thus after the reaction is complete, the pressure of the gas is that of the produced hydrogen and the vapor pressure of water (which is easy to find) . Therefore:
PH2(g) = Patm – PH2O
This of course assumes that the liquid levels in the beaker and in the eudiometer tube are the same. If there are not, we must correct for that. You know the pressure of the atmosphere and you will know the difference in P between the inside of the tube and the atmosphere, as measured by a ruler. Unfortunately, you measured P in mm of H2O, not mm Mg. To convert the pressure difference in terms of mm of Hg, you must divide mm H2O by 13.546 since Hg is 13.546 times as dense as water at room temperature. Thusly:
PH2 = Patm – Pdiff between tube and atmosphere – PH2O(g)
This is called the ‘dry’ pressure of H2(g) since there is no H2O(g) included in the pressure value. Make sure when you use this equation that all the units are the same (mm Hg).
PV=nRT is
called the ideal gas law as it assumes some fundamental properties of gases,
namely that the gas molecules have no volume and that their attractive forces
are zero which is not always a valid assumption. You will be
calculating the value of R using PV=nRT. You will also need to
calculate the relative error obtained in your experiment:
Lab 'Picture'
This report is NOT a short form memo per se. In your report, you need to include all data and calculations in a straight forward and easy to understand fashion. It should be crystal clear to the reader what you measured, what you calculated and how you calculated it. If you just have numbers (raw data and calcualtions) you will do poorly. You need to have words to support the data. Once sample calculation of EVERY single calculation you do is required. Think of this as a results section from a short form memo with the raw data included inside. Most of the points are coming from this one section, so be complete! You are calculating a value of R using the ideal gas law for each run. You must report your average values of R as well as percent error. As with any other lab in CEM 141, you also need to comment on this lab in terms of a learning experience and give at least one suggestion as to how to improve the experience.
Prelab questions: (To be written on separately on a piece of recycled paper)
1. What is the vapor pressure of water at 25 deg C ? Where did you get this information?
2. Calculate the value of R using the ideal gas law for the following data: Vdry H2 = 73.52 mL ; Pdry H2 = 635 torr ; massMg (which gets you moles of H2) = 0.0811 g ; T = 23.5 °C.
3. Your instructor will show you how to do setup the experiment, but you must know what information you need to determine for your three runs. Come up with some semblance of a data sheet. You will show this to your instructor on the way in. No data sheet, no lab.
~MEO 23Oct 2006