• 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...

Introduction

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.

Middle

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.

Conclusion

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

    This causes the lower temperatures to have a lower amount of time taken for the marble to travel through the glycerin. This issue can be fixed by slightly dipping thermometer into the glycerin and making sure that only about 1 cm is in contact with glycerin.

  1. Enthalpy Change Design Lab (6/6)How does changing the initial temperature (19C, 25C, 35C, and ...

    Using a clean, dry 50.0 cm3 graduated cylinder, 40.0 cm3 of 1.00 mol dm-3 KOH(aq) were measured. These 40.0 cm3 of 1.00 mol dm-3 KOH(aq) in the graduated cylinder were then poured into a clean, dry 150 cm3 beaker, and was labelled 'KOH(aq)'.

  2. Lab Experiment : The change in mass when magnesium burns. (Finding the empirical formula ...

    4.Number of moles of oxygen atoms that were used. = 0.0080Mole (the number of moles of oxygen = mass / atomic weight . The atomic weight of magnesium is 16.0 g / mole ) 5.Simplest ratio: Mg = 0.0096Mole = 1.2 0.0080Mole Oxygen = 0.0080mole = 1 0.0080mole Multiply by

  1. Aim: To find the molar mass of butane, by finding the number of moles ...

    * We found the volume of water between the tip of the cylinder and the 0cm3, and included that in our calculations of the volume of water. Fair Test * After every trial, we dipped the lighter in ethanol and then shook it to dry to ensure that was minimal

  2. hess's law

    sulphate with water and hydrated copper (II) sulphate with water is an exothermic reaction. The heat energy gained due to rise in temperature was then lost to the surrounding as a gradual decrease in temperature was observed with time after the reaction had taken place and because the reaction was exothermic, the enthalpy change value obtained is negative.

  1. Hydrogen Gas Collection Lab CE (6/6) A sample of solid magnesium ribbon, measuring approximately ...

    (Johnson, n.d.) Assuming the temperature within the gas measuring tube is higher than what was measured by the thermometer measuring from the side of the 1000cm3 graduated cylinder, and the tap water surrounding the gas measuring tube, that means that of the 102.71 kPa +/- 0.01, less pressure is actually

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

    used to determine the maximum temperature reached in the duration of the reaction. Graph 3: Highest temperature reached in Part Y, Trial 1. Figure 3: Zoomed in view of the y-axis and horizontal line intersection. From the figure, the value for the maximum temperature reached can be safely estimated to be 34.6oC.

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