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The Synthesis and Determination of Empirical Formula for Magnesium Oxide Sample Essay

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Purpose:

To find the empirical expression for Mg oxide.

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Data Collection:

Table 1 Mass of empty crucible. crucible + Mg ( approximately 1cm pieces of a 15-cm piece of Mg thread ) . and crucible +MgxOy. ( mass measured with an analytical balance ) . The mass of crucible + MgxOy was obtained after a uninterrupted procedure of warming. allowing cool. heating with H2O adequate to plunge the content and allowing cool of the Mg.

Mass of Empty crucible ( g ) Mass of Crucible + Mg ( g ) Mass of Crucible +MgxOy ( g )

16. 04716. 21416. 294

Uncertainty of analytical balance = + 0. 002

*Note that because we are unsure if Mg has wholly reacted with O2 in the first warming. if all the Mg have reacted with O2 alternatively of N and if the H2O added has wholly vaporized in the 2nd warming ( with H2O ) . the information and the undermentioned computations may non be as accurate.

Data Presentation and Procession:

1. mass of crucible + Mg – mass of empty crucible =Mass of Mg

16. 214 ±0. 002 g

– 16. 047± 0. 002 g

0. 167 ± 0. 004 g

2. mass of crucible + MgxOy -mass of crucible +Mg = mass of O

16. 294 ±0. 002g

– 16. 214 ±0. 002g

0. 0800±0. 004

3. mass of Mg =0. 167± ( 0. 004/0. 167*100 % )

=0. 167±2 % g

4. mass of O = 0. 0800± ( 0. 004/0. 0800*100 % )

=0. 0800±5 % g

5. Mole O = ( 0. 0800±5 % g ) / ( 15. 999g/mol )

=0. 00500 ±5 % mol

6. Mole Mg = ( 0. 167±2 % g ) / ( 24. 305g/mol )

=0. 00687±2 % mol

7. Relative ratio of Mg = 0. 00687/0. 00500 ± ( 2 % +5 % ) mol

=1. 37±7 % mol

=1. 37± ( 7*1. 37/100 )

=1. 37±0. 1

8. Relative ratio of O = 0. 00500/0. 00500 ± ( 5 % +5 % )

=1. 00±10 %

=1. 00± ( 10*1. 00/100 )

=1. 00±0. 1

9. Empirical Formula= Mg1. 37±0. 1O1. 00±0. 1

=MgO

Table 2 Mass and comparative ratio of Mg and O and calculated empirical expression for Mg oxide as determined by its comparative ratio.

Mass of O± uncertainnesss ( g ) Mass of Mg ± uncertainnesss ( g ) Number of Mole ± % of uncertainnesss Relative ratio ± uncertaintiesEmpirical Formula

0. 167 ±0. 0040. 0800± 0. 004OMgOMgMgO

0. 00500± 5 % 0. 00687± 2 % 1. 00± 0. 11. 37± 0. 1

Evaluation:

Compare to the recognized one to one ratio of the empirical expression for Mg oxide. our deliberate empirical expression Mg1. 37±0. 1O1. 00±0. 1 suggests an instability ratio with less than one O atom for every Mg atom. This assurance about the proportion of Mg alternatively of O is due to the certainty of the mass of Mg ( a 15 centimeter Mg thread ) . and uncertainnesss of the mass of O whose value may alter because of some beginnings of mistake during the reaction with Mg ( with and without adding H2O ) . Two possible beginnings of mistake that may explicate the unequal presence of O atoms are the uncomplete reaction of Mg with O during the first warming ( without adding H2O ) and the reaction of Mg with N alternatively of O during the 2nd warming ( adding H2O ) . It is possible that non all of the Mg has reacted with O in the given warming clip during the first warming or/and H2O has non broken all the bonds between Mg and N ( N occurs of course with O during heating ) for Mg to respond with more O therefore cut downing the presence of O atoms.

Our experiment can be improved and beginnings of mistake can be eliminated. if we repeat the procedure of heating the content. allowing it to chill and mensurating its mass during the first and 2nd warming ( with and without adding H2O ) until the mass reaches a changeless value. In this manner. we can guarantee that all Mg has wholly reacted with O.

Cite this The Synthesis and Determination of Empirical Formula for Magnesium Oxide Sample Essay

The Synthesis and Determination of Empirical Formula for Magnesium Oxide Sample Essay. (2017, Oct 24). Retrieved from https://graduateway.com/the-synthesis-and-determination-of-empirical-formula-for-magnesium-oxide-essay-sample-essay/

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