• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Determination of the molar mass of Magnesium from the reaction of magnesium and hydrochloric acid.

Extracts from this document...


Determination of the molar mass of Magnesium from the reaction of magnesium and hydrochloric acid. Aim of investigation. Determining the molar mass of magnesium by using the ideal gas equation and Dalton's law about partial pressure from the reaction of magnesium and hydrochloric acid. Hypothesis Mg(S)+2 HCl � H2(g)+mgcl2(aq) From the above reaction for one mole of mg, there is one mole of h2. By finding the mole of h2 formed (using ideal gas equation), the mole of mg used can be founded. The molar mass of mg is found from the mole using the formula: Molar mass(M)= Given mass(m) Amount of substance(n) Materials used Eudiometer, thermometer, barometer, measuring cylinder (1000 cm3), stand with clamp, magnesium ribbon and hydrochloric acid 35% (concentrated). Variables There are three variables in this experiment. * The independent variable is amount used for each reactant (magnesium and HCl). * The dependent variable is the amount of hydrogen gas produced. It varies according to the change for the magnesium used. ...read more.


Results after the experiment Amount of magnesium used (g) = 0.0590 Volume of h20+hcl in eudiometer= 63 cm3 Volume of h2 gas formed= 58.8 cm3 Pressure of room= 104.2 kpa Water vapor pressure at 22c= 2.6kpa Temperature of the room= 22 c Discussion and conclusion. Step one: - The Dalton's law of particle pressure states that the total pressure of a mixtures of gases is equal to the sum of the pressure of all of the constituent gases alone. For this experiment, the total pressure inside the eudiometer will be the sum of the pressure of the hydrogen gas formed and the water vapor. It can be expressed as follows: P eudiometer = Ph2+ P water vapor ....................................................Equation 1 Here the total pressure of the eudiometer is equal to the pressure of the room since it was lifted making its water level equal to the level of water in the measuring cylinder. The pressure of water vapor at 22c is equal to 2.6Kpa (refer to table 1). ...read more.


of a product when a limiting reactant is completely consumed. In this reaction, the limiting reactant is magnesium. Mg(S)+2 HCl � H2(g)+mgcl2(aq) 24 g 2 g .......where 24 and 2 are molar masses of mg and h2 0.0509 g X Then X is equal to = 2 g � 0.0509g = 0.0042 g of hydrogen gas 24 g This can be written in terms of amount of substance (n) for hydrogen gas: Amount of substance (n) = 0.0042 g 1 g = 0.0042 moles of hydrogen gas Actual yield: - is the amount of product actually obtained i.e. the quantity of product finally collected or isolated from a reaction. In this case, the actual amount of hydrogen gas obtained is 0.0024 moles. Then by applying equation 5 the percentage yield can be found. % yield = Actual yield � 100 Theoretical yield = 0.0024 � 100 0.0042 = 57.1% Usually actual yield is less than theoretical yield for many reasons. It could be problem with the apparatus used and errors in measurement etc. ?? ?? ?? ?? ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Experiment - The Empirical Formula of Magnesium Oxide

    These could cause random errors. Another random error could be that when the crucible lid was lifted, the produced powdered magnesium oxide might have escaped the crucible. The mass would then be heavier than it was weighed. As shown on the graph, R2 (the correlation coefficient)

  2. Hesss Law Lab, use Hesss law to find the enthalpy change of combustion of ...

    extent and my results are fairly accurate because they are lying just 4.5% below the table values. These points towards the fact that there are some small problems with the system for my results not being more accurate and I am going to discuss it in the paragraph below.

  1. Can one determine the coefficients of a balanced chemical equation by having the mass ...

    Record the properties of the product of the solution to ensure that the reaction is truly finished. Record all these properties in "Data Table 1 - Qualitative Data Table" and record it under "After Reaction". 13. Take the aluminum strip and wash it to ensure that any remaining copper

  2. The purpose of this investigation is to determine the effect varying temperatures have on ...

    and HCl to complete and Rate of Reaction Actual Temperature of HCl (�0.05�C) Mass of Mg (�0.01g) Average Time (�3s) Rate of Reaction (mol/s Need UNCERTAINTY) 10.5 0.02 20 0.00004 15.5 0.02 14 0.00006 29.5 0.02 13 0.00006 50.5 0.02 10 0.00008 69.5 0.02 9 0.00009 Figure 2: Actual temperature of HCl vs.

  1. Rate of reaction of Magnesium with Hydrochloric acid

    Measure 50 cm3 of 1 mol dm-3 hydrochloric acid using a measuring cylinder. Pour the acid into the 100 cm3 conical flask. 2. Set up apparatus as shown in the diagram. 3. When you are ready, add a 3 cm strip of magnesium ribbon to the flask, put the bung

  2. Lab report. Finding the molar enthalpy change of the reaction between Hydrochloric acid and ...

    A -34±4 Exp. B 35± 2 Exp. C 20±1 Using hess’s law we can determine that the final enthalpy change for the reaction would be . Then as I did before I added the uncertainties up getting a final value for the molar enthalpy change of the reaction to be -50± 7 .

  1. Measuring the fatty acid percentage of the reused sunflower oil after numerous times of ...

    Also the amount of potatoes must stay the same in each trial if the frying is made by using new oil for different numbers of frying. Like using the oil only for 5 times frying then renewing the oil for 10 times frying and doing this for others.

  2. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    The lid of the calorimeter was closed as quickly as possible to ensure that heat loss through convection currents was minimized. 6. Using the thermometer, the mixture was very gently stirred for a few seconds. 7. Every five seconds, the reading on the thermometer was read as accurately as possible and noted.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work