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Experiment B1: Molar Volume of a Gas, Lab Reports of Chemistry

College of Menominee Nation (CMN)Chemistry

Dalton’s law of partial pressures, Combined Gas law, with their sample data and calculation

Typology: Lab Reports

2020/2021

Uploaded on 05/11/2021

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1!
EXPERIMENT)B1:)MOLAR)VOLUME)OF)A)GAS)
)
Learning)Outcomes)
!
Upon!completion!of!this!lab,!the!student!will!be!able!to:!
!
1) Demonstrate!a!single!replacement!reaction.!)
2) Calculate!the!molar!volume!of!a!gas!at!STP!using!experimental!data.)
3) Calculate!the!molar!mass!of!a!metal!using!experimental!data.!!!)
)
Introduction)
!
Metals!that!are!above!hydrogen!in!the!activity!series!will!displace!hydrogen!from!an!
acid!and!produce!hydrogen!gas.!Magnesium!is!an!example!of!a!metal!that!is!more!
active!than!hydrogen!in!the!activity!series.!The!reaction!between!magnesium!metal!
and!aqueous!hydrochloric!acid!is!an!example!of!a!single!replacement!reaction!(a!
type!of!redox!reaction).!The!chemical!equation!for!this!reaction!is!shown!below:!
!
Mg(s)!+!2HCl(aq)!!!MgCl2(aq)!+!H2(g)!!!!Equation)1!
!
When!the!reaction!between!the!metal!and!the!acid!is!conducted!in!a!eudiometer,!the!
volume!of!the!hydrogen!gas!produced!can!be!easily!determined.!In!the!experiment!
described!below!magnesium!metal!will!be!reacted!with!an!excess!of!hydrochloric!
acid!and!the!volume!of!hydrogen!gas!produced!at!the!experimental!conditions!will!
be!determined.!!
!
According!to!Avogadro’s!law,!the!volume!of!one!mole!of!any!gas!at!Standard!
Temperature!and!Pressure!(STP!=!273!K!and!1!atm)!is!22.4!L.!!
!
Two!important!Gas!Laws!are!required!in!order!to!convert!the!experimentally!
determined!volume!of!hydrogen!gas!to!that!at!STP.!
!
1. Dalton’s!law!of!partial!pressures.!
2. Combined!gas!law.!!
!
Dalton’s)Law)of)Partial)Pressures)
!
According!to!Dalton’s!law!of!partial!pressures!in!a!mixture!of!non-reacting!gases,!the!
total!pressure!exerted!is!equal!to!the!sum!of!the!partial!pressures!of!the!individual!
gases.!!
!
For!instance,!if!there!is!a!mixture!of!two!gases!whose!individual!partial!pressures!
are!P1!and!P2,!then!the!total!pressure!exerted!by!the!two!gases,!PT!is!given!by:!
!
PT!=!P1!+!P2!!!!!!!Equation)2!
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EXPERIMENT B1: MOLAR VOLUME OF A GAS

Learning Outcomes

Upon completion of this lab, the student will be able to:

  1. Demonstrate a single replacement reaction.
  2. Calculate the molar volume of a gas at STP using experimental data.
  3. Calculate the molar mass of a metal using experimental data.

Introduction

Metals that are above hydrogen in the activity series will displace hydrogen from an acid and produce hydrogen gas. Magnesium is an example of a metal that is more active than hydrogen in the activity series. The reaction between magnesium metal and aqueous hydrochloric acid is an example of a single replacement reaction (a type of redox reaction). The chemical equation for this reaction is shown below: Mg(s) + 2HCl(aq)! MgCl2(aq) + H2(g) Equation 1 When the reaction between the metal and the acid is conducted in a eudiometer , the volume of the hydrogen gas produced can be easily determined. In the experiment described below magnesium metal will be reacted with an excess of hydrochloric acid and the volume of hydrogen gas produced at the experimental conditions will be determined. According to Avogadro’s law, the volume of one mole of any gas at Standard Temperature and Pressure (STP = 273 K and 1 atm) is 22.4 L. Two important Gas Laws are required in order to convert the experimentally determined volume of hydrogen gas to that at STP.

  1. Dalton’s law of partial pressures.
  2. Combined gas law. Dalton’s Law of Partial Pressures According to Dalton’s law of partial pressures in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases. For instance, if there is a mixture of two gases whose individual partial pressures are P 1 and P 2 , then the total pressure exerted by the two gases, PT is given by: PT = P 1 + P 2 Equation 2

In order to see how this law applies to the current experiment, it is important to understand the experimental set up. As stated above, the reaction between magnesium metal and aqueous hydrochloric acid will be conducted in a eudiometer. See Figure 1 below. FIGURE 1: EXPERIMENTAL SET UP The magnesium metal is attached to the stopper of the eudiometer. The aqueous hydrochloric acid is in the eudiometer. The inverted eudiometer is placed inside a water bath. When the metal comes in contact with the acid, the reaction produces hydrogen gas. The hydrogen gas fills the eudiometer. The reaction continues until all the magnesium metal (which is the limiting reagent in this experiment) is completely consumed. As shown in Figure 1, the H2(g) that is formed is combined with water vapor. The water vapor is a result of the vapor pressure of water found in the aqueous medium. Therefore, the two gases: H2(g) and H 2 O(g) are both found in the eduiometer. Assuming the surface of liquid in te eudiometer is level with the water outside, the total pressure of the gases inside the eudiometer is the same as the atmospheric pressure. A barometer that is found in the laboratory is used to determine the atmospheric pressure. Therefore, according to Dalton’s law: Water HCl(aq) Mg(s) H2(g) + H 2 O(g) Patm

Finally, the moles of H2(g) produced in the experiment must be determined in order to obtain the volume of one mole of the gas. The experiment is designed such that the magnesium metal is the limiting reagent. Therefore, if the mass of the magnesium metal is known, the moles of H2(g) produced can easily be determined using the reaction stoichiometery (Equation 1). Sample Data and Calculation In a certain experiment, 0.0369 grams of magnesium was reacted with excess HCl. The reaction resulted in 38.2 mL of H2(g) at 22°C. The barometric pressure was recorded as 749.2 mm of Hg. Calculate the molar volume of the gas at STP. Mass of magnesium metal = 0.0369 grams Atomic mass of magnesium metal = 24 grams/mol Moles of magnesium metal = 0.00154 moles Mg(s) + 2HCl(aq)! MgCl2(aq) + H2(g) Moles of H2(g) = Moles of Mg × € 1 mole H 2 1 mole Mg = 0.00154 moles Temperature of H2(g) = 22°C = 295 K = T 1 Calculate the PH2O using equation 5: € PH 2 O = exp 20.386 −

T

( mmHg PH2O = 19.89 mm of Hg Barometric pressure = 749.2 mm of Hg PH2 = 749.2 – 19.89 = 729.31 mm of Hg = P 1 Volume of H2(g) = 38.2 mL = 0.0382 L = V 1 At STP: Pressure = 760 mm of Hg = P 2 Temperature = 273 K = T 2 Use Equation 6 to solve for V 2 :

V 2 =

P 1 V 1

T 1

×

T 2

P 2

729.31 mmHg × 0.0382 L × 273 K 295 K × 760 mmHg

= 0.0339 L

Moles of H 2 = 0.00154 moles Therefore molar volume = €

0.0339 L

0.00154 moles

L

mol

Procedure

  1. Obtain a 50-mL eudiometer and a thermometer from the stockroom. Also obtain a buret stand and clamp from the laboratory.
  2. Place a 100-mL graduated cylinder in an empty 600-mL beaker. Clamp the graduated cylinder in place and fill the graduated cylinder with water to the rim.
  3. Cut a 2 - cm strip of magnesium metal and scrape the metal with sandpaper to remove any dark oxides.
  4. Measure the mass of the magnesium metal. [NOTE: The magnesium is the limiting reagent in this experiment]
  5. Coil the magnesium strip. Using the copper wire, attach the magnesium metal to the inside of the stopper for the eudiometer, by forming a wire cage around the magnesium metal.
  6. Add 10 mL of 6 M HCl into the eudiometer.
  7. Fill the remainder of the eudiometer with deionized water slowly, attempting the disturb the HCl as little as possible. [NOTE: Normally, concentrated acid is added to water for dilution purpose. In this step, the reverse process is being recommended. Care must be taken to avoid spills or splashing.]
  8. Seal the eudiometer with the stopper. Place the stoppered eudiometer above the 100 - mL graduated cylinder containing water and turn it upside down. Immerse the stopper end of the eudiometer completely under water.
  9. Clamp the eudiometer to the buret stand. The reaction between the magnesium metal and the HCl will start momentarily and hydrogen gas will collect in the eudiometer. The aqueous solution will be pushed out through the stopper into the 1 00 - mL graduated cylinder, which will overflow into the 600-mL beaker that the graduated cylinder is placed in.
  10. When the reaction is complete, move the eudiometer so that the level of the water in the eudiometer is equal with the water inside. If this is not possible, record the difference in height between the eudiometer and the graduated cylinder.
  11. Measure and record the volume of the hydrogen gas.
  12. Record the temperature of the water and assume this to be the temperature of the hydrogen gas.
  1. Record the barometric pressure.
  2. Empty the contents of the eudiometer into the 600-mL beaker and the contents of the 600-mL beaker into the waste container provided by the instructor. Rinse the eudiometer with deionized water.
  3. Repeat steps 3- 14.

Calculations

MOLAR VOLUME OF A GAS AT STP

Trial 1 Trial 2 Mass of magnesium, grams Atomic mass of magnesium (grams/mol) Moles of Magnesium Moles of H2(g) (use stoichiometry) Temperature of H2(g) (T 1 in Kelvin) Volume of H2(g) (V 1 in L) Barometric pressure (PT in mm of Hg) € PH 2 O ( g ) (mm of Hg) (use Equation 5) € PH 2 ( g ) (same as P 1 ) (mm of Hg) (use Equation 4) Volume of H2(g) at STP (V 2 in L) (use Equation 6) Molar volume of H2(g) at STP (L/mol) Percent error

ATOMIC MASS OF A METAL

Assume that the identity of the metal used in the experiment (i.e., magnesium) is unknown. Assume also that the stoichiometry of the reaction between the unknown metal M and HCl is as follows: M(s) + 2HCl(aq) !MCl2(aq) + H2(g) Using the data collected, calculate the atomic mass of the metal M Trial 1 Trial 2 Temperature of H2(g) (T 1 in Kelvin) Volume of H2(g) (V in L) Barometric pressure (PT in mm of Hg) € PH 2 O ( g ) (mm of Hg) (use Equation 5) € PH 2 ( g ) (mm of Hg) (use Equation 4) Moles of H2(g) produced (HINT: PV = nRT) Moles of metal (use stoichiometry) Mass of metal in grams (from the data table) Atomic mass of metal € grams moles

Average value of Atomic mass € grams moles