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

    the smallest whole number you can possibly find to get whole number: 1.2 x 5 = 6 1 x 5 = 5 The ratio of Mg to O is therefore 6:5 The empirical formula of Magnesium Oxide found for this trial is therefore Mg6O5 Trail 5.

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

    Finally figure 3, illustrates that as the temperature of the glycerin increase the mean time taken for marble to travel through 50mL of glycerin decreases. Also the graph illustrates that the time taken decreases as temperature increases in an inversely proportional manner.

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

    and 1.00 mol dm-3 HCl(aq) to reach it's maximum temperature, the greater the opportunity for heat to escape from the calorimeter as time goes on. To mitigate the effects of heat loss on the temperature change recorded during the investigation, regarding the neutralization reaction of 1.00 mol dm-3 HCl(aq)

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

    Enthalpy of reaction calculated for this trial = * ?HX (Trial 1) = = 249000J = -249kJ.mol-1. For Part X, Trial 2 Graphical analysis similar to that used in Part X, Trial 1 has been used to determine the maximum temperature reached in the duration of the reaction.

  1. How the concentration of hydrochloric acid affects the rate of the reaction with magnesium.

    x 10-4 2.0 65 9.2 x 10-4 2.5 32 1.8 x 10-3 Graph 1- The concentration of HCl plotted against the rate of reaction Conclusion In conclusion, the results I obtained supported my hypothesis because as it can be seen from the graph and the results above, the rate of reaction increases as the concentration of hydrochloric acid increases.

  2. Chemistry Investigation to find the Empirical Formula of Magnesium Oxide

    Suggestion for Improvements At the beginning of the experiment, the Bunsen burner was not under the crucible and We had to move the Bunsen burner directly under the crucible. Because of this it may have affected how much heat interacts with the magnesium.

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