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

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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.

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