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

Chemistry IA design format

Extracts from this document...

Introduction

Contents Page Number Areas 1 Title 2 Contents 3 1.0.1, 1.0.2, 1.0.3 4 1.1.1 5 1.1.2, 1.1.3 6 1.1.4,1.2.1 7 1.2.2 8 Bibliography 1.0.0- Introduction 1.0.1- Focus Question- If the mass of magnesium reacted with hydrochloric acid is changed will the temperature of the solution increase and the total mass decrease. 1.0.2- Hypothesis- If the mass of magnesium that is reacted with hydrochloric acid is changed the temperature of the solution will increase and the total mass will decrease. 1.0.3- Theory- The reaction between magnesium and hydrochloric reaction is written as follows, Mg(s)+ 2HCL (aq)------ (MgCl2(aq)+H2 (g) (Ng, 2008, pg 1). This reaction goes through two distinct changes that both have an effect on the energy change in the reaction. Enthalpy refers to changes in energy in a compound (Assut, 2008, pg 1). Two distinct changes can occur. An endothermic change occurs when the energy being absorbed is grater then the energy being released whereas and exothermic change is when the energy being released is greater than the energy being absorbed. ...read more.

Middle

In a mass of a substance there is a certain amount of material that can be reacted. By increasing mass the amount of substance that may be reacted increases. Therefore if mass increased the amount that of substance reacted will increase as well providing there is enough of the reactant. This will in turn increase the energy change. Also if more of the substance reacts with the reactant more of the reactant will be used up. This means that if the magnesium is increased there will be more reaction with hydrochloric acid; this means that more hydrogen will be released as gas and the total mass of the solution will decrease. Henceforth the change in heat should be greater if their entire solution is lighter as more of the hydrochloric acid has been reacted and hydrogen lost as a gas. How the reaction works (Figure 1) Mg(s)+ 2HCL (aq)------ (MgCl2(aq)+H2 (g) 1.1.0- Controlling variables 1.1.1- Variables (Table 1) Variable Type of variable Method for control Mass of magnesium Independent Mass will change for each sample, sample range will be 2g, 4g, 6g, 8g and 10g Heat change Dependent This will be calculated by subtracting the final heat of the solution by the initial heat of the solution. ...read more.

Conclusion

Apparatus 1 Pair of rubber gloves Apparatus 1 Measuring cylinder 50mls Apparatus 1 1.1.4- Safety aspects (table 3) Aspect Risk MSDS reference Control Hydrogen gas giving off reaction Extremely flammable Risk of explosion if heated under confinement. R22 R44 S16 S60 Keep area well ventilated Hydrochloric acid Harmful if swallowed Toxic by inhalation Causes severe burns Risk of serious damage to eyes R22 R23 R25 S01 S27 S23 S17 S25 S35 S26 S45 S38 S60 S51 S63 S09 S40 S07 Magnesium Highly flammable Contact with water liberates extremely flammable gas (hydrogen) Spontaneously flammable in air. R11 R15 R17 S30 S22 S24 S29 S51 S09 S26 S60 1.2.0- Method for the collection of data 1.2.1- Protocol diagram (Figure 2) 1.2.2- Procedure 1- Record weight of empty calorimeter 2- Fill calorimeter with 40mls of hydrochloric acid 3- Measure weight and subtract this weight by weight of calorimeter and weight of the magnesium sample and record. 4- Heat sample to 25 degrees Celsius with hotplate 5- Immediately insert 2 grams of magnesium strips 6- Once reaction has been fully completed (No more magnesium or no more hydrochloric acid) record the final temperature. ...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. A comparison of various proprieary antacids

    The volume of 25cm3 to which the antacid is added also has an error. The pipette has an error label of �0.06 cm3 Pipette error= 0.06/ 25 cm3 x 100= 0.24 % Therefore initial moles of HCl= 0.0125 moles � 0.24% Errors in titrating the remaining NaOH with hydrochloric acid

  2. Hesss Law Lab, use Hesss law to find the enthalpy change of combustion of ...

    RU ( c) = 0 ( table value ) So percentage uncertainty for RU(Q)=RU(m)+ RU(?T) RU(Q) = 2+ 12.5 = +/- 14.5 % Now, the absolute uncertainty for MgO's mass is, AU(m(MgO))=+/-0.01 g Then RU(m(MgO))= (AU(m(Mg))/ m(Mg))*100% RU(m(MgO)) = (0.01/0.40)*100 = 1/0.40 = � 2.5 % As AU(M(Mg))=0 because this value is given and not calculated by us so, RU(n)

  1. IB IA: Determination of Heat of Neutralization

    The experimental value for the enthalpy change for neutralization is less than the theoretical value of standard enthalpy change for neutralization. 5. This is due to the fact that some heat is lost to the surrounding and the heat absorbed by the polystyrene cup is not included in the calculation.

  2. IB chemistry revision notes

    Charge Found in atom Proton 1 +1 Nucleus Nucleons Neutron 1 0 Nucleus Electron 1/1840 -1 Shells * Almost all the mass of the atom is concentrated in the nucleus which has a very small radius.

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

    8. Less flame. 9. No flame but it glows. 10. Less sparks and less glow. 11.Little smoke. 12.No smoke(white fluid material and residue on lid). 13. No further reaction. Raw Data: Initial mass of crucible with lid ( in grams) + 0.0001= 27.6400g Mass of magnesium inside crucible with the lid ( in grams)

  2. Acids/Bases Design Lab. How does a change in the pH value of a solution ...

    The temperature of the hydrochloric acid solution should be at room temperature, as should the zinc metal strips being used in the investigation. The zinc metal strips, once exposed to the room temperature air, will adjust themselves to conform to the atmospheric temperature, and can do so as the investigator is setting up their materials.

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

    Using the burette, 15cm3 of 2M HCl was withdrawn into the calorimeter and was allowed to sit for a minute or two so that its temperature reaches the ambient temperature. In the duration of these few minutes, Magnesium Oxide was prepared for reaction using the following step.

  2. Paper Chromatography on Amino Acids IA

    The entire experiment was only completed once which means only one chromatogram was produced. Therefore, an average could not be deduced. Repeat the experiment once or twice more as it then allows for an average to be calculated. An average will give a better sense of an overall Rf value and will be able to reduce errors in the experiment.

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