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

Stoichiometry Lab Report. Aim: To determine what solid product is produced in the decomposition of NaHCO3, based on the pre-calculated mass of the solid products versus the mass found in the experiment.

Extracts from this document...

Introduction

Chemistry Lab Report Dr. Terbush Lotje Mulder Stoichiometry Lab Report Aim: To determine what solid product is produced in the decomposition of NaHCO3, based on the pre-calculated mass of the solid products versus the mass found in the experiment. Hypothesis: I think that the solid product produced from the decomposition of baking soda will be Na2CO3 because out of the three possible products it weighs the most. The two bi-products H2O and CO2 weigh almost nothing and therefore subtract almost nothing from the weight of the reactant. Theory: In this experiment, two branches in chemistry are involved: chemical decomposition as well as stoichiometry. Decomposition is the separation of a chemical compound into two or more elements or other compounds. It can be defined as the opposite of chemical synthesis. In this experiment we are using thermal decomposition because we are using extreme environmental conditions like heat to limit the stability that the chemical compound ordinarily has. The reaction is usually endothermic because it is absorbing heat because heat is required to break the chemical bonds in the compound in order to undergo decomposition. ...read more.

Middle

Materials: - tripod - Bunsen burner - clay triangle - crucible with lid - 2.0 grams of baking soda for each trial - stopwatch or timer Diagram: Procedure: 1. Set up a tripod and a Bunsen burner. Place a clay triangle on the tripod. 2. Clean the empty crucible and then measure the mass of it and record the mass in the data table. 3. Measure the 2.0 grams of baking soda in the crucible and record this in the data table. 4. Measure the total mass of the crucible and the baking soda. Record this measurement in the data table. 5. Heat the crucible for 10 minutes. During the heating process, break up the clumps that form with a stirring rod. 6. Once the crucible has cooled to room temperature, measure the mass of the crucible and the remaining solid material. Record this measurement in the data table. Data Table (+/- .001 g) Mass of crucible Mass of baking soda Mass of crucible and baking soda Mass of crucible and solid product Mass of solid product 9.615 g 2.000 g 11.615 g 10. ...read more.

Conclusion

This may have caused the reaction to change due to impurities interfering with the decomposition. Second of all, we didn't stir throughout the 10 minutes. This means that any clumps in the baking soda would not have reacted completely. Also if it is less hot towards the outer layer of the baking soda, the chemical bonds may not have been broken down as well as the baking soda towards the bottom of the crucible. Third of all, we did not measure the weight of the crucible with the final product when it was completely cooled off. The reaction may not have been fully done until all the heat was used; however because we didn't wait, the results may have been affected. Improvement: Based on the evaluation you can see that it is imperative to follow the procedure exactly as it is. If not, you are risking faulty data. If I were to repeat this experiment again for a third time, I'd make sure I clean the crucible to the best of my ability. I'd also make sure to stir throughout the ten minutes as well as measure the final weight after it cooled off. ?? ?? ?? ?? ...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. THE CATALYTIC DECOMPOSITION OF HYDROGEN PEROXIDE

    To make this clearer, it means that catalysts only help to overcome activation energy in order to conserve the rest of the energy for the reaction. The more energy there is left the faster the reaction will be. This would explain why adding more catalyst causes an increase in the rate of decomposition.

  2. Enthalpy of Combustion Lab Report

    2. Once the time period of one and a half minutes has elapsed, the cap of the spirit flame was placed over the wick of the spirit lamp with precision and safety. 3. Before starting the experiment, one made a double check about all the equipment being used in the experiment and whether the equipment is efficient or not.

  1. IB chemistry revision notes

    --> Iron (II) chloride. --> Potassium dichromate (VI) Ag Sc Ti V Cr Mn Fe Co Ni Cu Zn 1+ 3+ 3+ 2+ 2+ 2+ 2+ 2+ 2+ 1+ 2+ 3+ 4+ 3+ 3+ 4+ 3+ 3+ 4+ 4+ 6+ 6+ 6+ 3+ 5+ 7+ 8+ Redox Titrations and 1.

  2. Combustion of alcohols lab report

    My graph shows one straight-line (Literature values), and another somewhat straight-line (experimental values), and this shows that the more carbon atoms there are in a compound, the heat of combustion goes up. This is probably because the molecular length of the compound increases, increasing the surface area, thus allowing more

  1. acid base lab report

    Phenolphthalein, the acid-base indicator that was used in this titration, has a color change range of pH range of 8.2 to 9.8 (see Table 1) and produced an endpoint colour change with Trial at a pH of 10.1. This indicator is unsuitable since it does not cover the range of the equivalence point which is 7.0.

  2. To determine the molecular mass of an unknown alkali metal carbonate, X2CO3.

    The 50cm3 beaker was placed on the digital balance and the balance was calibrated to 0. 2. Using the metal spoon, slowly and carefully, 1.5g of substance Z was weighed out into the 50cm3 beaker. 3. Distilled water was added to completely dissolve the solid mass of substance Z. 4.

  1. Period 3 Chlorides. Aim: To study the chlorides of period 3 elements and ...

    2) Wikipedia, the free online encyclopaedia. Aluminium Chloride. 4 November 2007. 17 November 2007 <http://en.wikipedia.org/wiki/Aluminium_chloride>. 3) Wikipedia, the free online encyclopaedia. Magnesium Chloride. 15 November 2007. 17 November 2007 <http://en.wikipedia.org/wiki/Magnesium_chloride>. 4) AUS-e-TUTE. Trends Across Period 3 of the Periodic Table. 18 November 2007. 17 November 2007 <http://www.ausetute.com.au/trendpd3.html>. Conclusion: After following the necessary procedure, taking the correct measurements and

  2. The aim of this experiment is to examine the enthalpy of combustion of the ...

    = ρ (H2O) * V (H2O) = 1.0 g cm-3 * 40.0 cm3 = 40.0 g The change in temperature is found in the following way : ΔT (H2O) = Tmin – Tmax = 24.0 °C – 85.0°C = 61°C ΔT (H2O)

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