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

# Heating of Magnesium Lab

Extracts from this document...

Introduction

The Heating of Magnesium Lab Purpose: The purpose of this experiment is to determine the chemical formula using the produce from a chemical reaction. Materials: - Magnesium ribbon - Electronic balance - Crucible and lid - Ring clamp - Clay triangle - Steel wool - Bunsen burner - Safety goggles - Ceramic pad Procedure: 1. Measure the mass of a clean, dry crucible, and lid. 2. Get approximately 10cm of magnesium ribbon, and polish it with steel wool. 3. Find the mass of the magnesium and place it in a loose coil at the bottom of the crucible. 4. Place the crucible in the clay triangle on the ring clamp that is mounted on the retort stand. Make sure the ring clamp is placed just above the height of the Bunsen burner flame. Place the lid on the crucible so that it is slightly ajar. 5. Heat the crucible with the Bunsen burner until it no longer glows. Do not look directly at the glowing ribbon. ...read more.

Middle

0.136g � 0.01g Mass of crucible & MgO 25.650 � 0.01g Calculations: Empirical Formula Work Mass of MgO Mass of magnesium = 0.136 g � 0.01g Mass of MgO = (Mass of MgO + crucible) - mass of crucible = 25.650 � 0.01g - 25.429g � 0.01g = 0.221 � 0.02g Mass of Oxygen= Mass of MgO - Mass of Magnesium ribbon = 0.221g � 0.02g - 0.136 g � 0.01g = 0.085g � 0.03g Percent composition of a 100g sample Magnesium Oxygen Mass of Mg Mass of MgO 0.136g � 0.01g Oxygen = 100% - percent composition of Mg 0.221g � 0.02g = 100% - 38% = 62% --> 62g of 100g sample = 38% --> 38g of 100g sample Molar Ratio Moles (n) = mass (m) Molar mass (MM) Magnesium Oxygen n= 62g/24.3050g/molecule n= 38g/15.9994g/molecule n= 2.6 moles n= 2.4 moles =2.6 moles: 2.4 moles = 1.1:1 Empirical Formula =Mg1.1O Molar Equivalency M.E. = moles (n) Balancing # Magnesium Oxygen M.E. ...read more.

Conclusion

= 0.221g - 0.22g x 100 0.22g = 0.45% error 6)Percent Yield Yield= Experimental yield x 100 Theoretical yield Experimental yield-->Mass of MgO= 0.221g Theoretical yield--->Mass of MgO= 0.22g = (0.221g/0.22g) * 100 = 100.5% yield In conclusion the empirical formula for MgO proves that the lowest ratios of the atoms of oxygen and magnesium have close to the same ratio. Any discrepancies were possibly a result of an error in some of the equipment that was used to weigh the magnesium and oxygen. This could explain why the empirical formula was 1:1.04 as there is a chance that the preciseness of the scale might have been incorrect, also next time the lab is done, the mass of the lid after the experiment should be taken into account as the magnesium oxide might have been evident upon it as well as there were grey streaks after the experiment on the lid. Furthermore, if we did the experiment more times (held more trials) we could've got an average or at least made sure the behavior we noticed stayed consistent. ?? ?? ?? ?? 1 ...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

# Related International Baccalaureate Chemistry essays

1. ## Experiment - The Empirical Formula of Magnesium Oxide

This graph presents the same information as the graph shown above except that it excludes the most obvious outlier point (0.006, 0.001). As a result, the gradient increased (became 0.694) and the R2 value got closer to 1. Conclusion and Evaluation Conclusion and Justification According to the processed data, the

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. ## Energetics Design Lab

* Designing an air tight hole on the lid which can easily be manipulated for the sodium carbonate to be dropped in. This would limit the heat loss of the reaction from the delay of putting the lid on after dropping the copper in.

2. ## Percent Yield Lab. This experiment has proven that KI is the limiting reagent ...

7. The solid in the funnel was placed into the incubator over night. 8. The dry solid was weighed. 9. The solution left was poured into a two beakers and KI was added. Observations Reactants Into Solutions Qualitative Properties Pb(NO3)2 (aq)

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

it would not be possible to draw a good graph using points that are unevenly spaced apart Time interval is taken to be 5 seconds between each reading. Room temperature and pressure Conditions under which the experiments are performed should remain constant The experiments were carried out in the same room and on the same day.

2. ## The purpose of this lab was to calculate the heat of formation for magnesium ...

0.1253g ± 0.0001g ±0.0001g = 0.0798% 1. Calculate the mass of hydrochloric acid (HCl) heated. Assume that density of HCl is the same as water:1.00g/cm3 Solution: mHCl = DHCl. VHCl mHCl = 1.00g/cm3. 100cm3 mHCl = 100g 1. Calculate the temperature change, ΔT, of the HCl.

1. ## Chemistry Investigation to find the Empirical Formula of Magnesium Oxide

Calculations Formulae Sample Formulae Sample Result Finding the mass of Mg Finding the mass of O Mg Mass of MgO Moles of Mg 3.414x 10-3 Finding moles of O 1.938x10-3 Average (do this last) 37.238 + 38.038 + 34.256 + 33.613 + 33.971 + 39.322 + 32.844/7 = 35.6117g Percentage

2. ## Discovering the formula of MgO

Apparatus and chemicals: 1. Crucible with lid 2. Bunsen burner 3. Tripod 4. Tongs 5. Balance 6. Pipe clay triangle 7. Beaker 8. Magnesium ribbon Hazards-Safety: 1. Inhalation of magnesium oxide fumes can cause metal fume fever therefore ensure that the room is well ventilated. • Over 160,000 pieces
of student written work
• Annotated by
experienced teachers
• Ideas and feedback to 