Determining the Rate of Reaction When Reacting Magnesium Powder with Hydrochloric Acid Essay

AimTo determine the station of answer forResearch QuestionWhat effect does the ingress of hydrochloric bitter engage on the rove of reaction when combined with magnesium powder? possible actionI hypothesise that the sight of hydrogen gas produced forget annex at a steep, but steady pose as the absorption of hydrochloric social disease increases, until the preoccupation is equal to 1.0 breakwater system dm-3. in that respectfore, the compute of reaction entrust remain constant until this point. I suggest this concentration because the hurtard concentration of hydrochloric acid utilize in general experiments is usually 1 mol dm-3. I so theorize that the ramble of reaction will bit by bit decrease until the incline of the graph (effect of increasing concentration of HCl against the intensiveness of hydrogen produced line graph 1) becomes 0.VariablesType of VariableVariableEn receivedd byDependent Variable* Time Taken* Timed using bring out clock* Volume of Hydr ogen Gas Produced* Experiment repeated terce time & Average takenIndependent Variable (quantitative)* Concentration of HCl(aq)* 8 concentrations were usedControlled Variables* Temperature* Water bath was used* Thermometer set in water bath* Mass of Magnesium* Used a 3 d.p. equalizer* Surface Area of Magnesium* Used powder & made sure mass was the same* Volume of Hydrochloric pane* A burette was used to measure volumeRequirements* water bath (30oC)* 500cm3 conical flask* pencil eraser double backper* delivery tubing* bill cylinder* clamp stand* stop clock* 0.06g magnesium powder* 20cm3 hydrochloric acid* 3 d.p. poise* spatula* weighing boat* burette (x2)* thermometer in water trough* sanctuary gogglesApparatusTechnical Notes1) The magnesium powder should be as pure as possible. It should be stored in a clean and change environment to ensure that no impurities (such as effects of oxidation) prevent the parade of accurate data.2) Eye protection is necessary due to the use of hydrochloric acid tiny bubbles may cause irritation of eyes.3) Rubber, instead of cork, must be used as the material for the bungs. Cork is too porous and will leak.4) No naked flames should be present hydrogen gas is highly flammableMethod1. The solutions were prepared with a calculated combination of hydrochloric acid and water, to produce 8 different concentrations of 20cm3 hydrochloric acid2. The apparatus was set up as shown in the diagram. The trough was half filled with water3. The cadence cylinder was filled with water, and remained full whilst being turned upside-down (as in diagram)4. The magnesium powder was added to the conical flask quickly and the bung was replaced as fast as possible to prevent any gas escaping. The stop clock was started.5. The volume of the gas was then collected in the measuring cylinder, measured and recorded after 30 seconds6. Steps 3-5 was repeated three times with fresh materials, and an honest volume of gas collated was calculated for t hat concentration7. This process (steps 1-6) was repeated for the 7 other concentrations (0.25 2.00M)8. The rate of reaction was then calculated for apiece of the concentrationsObservations* As the magnesium powder reacted with the hydrochloric acid, fizzing on the surface was evidence of a reaction taking place.ConclusionFrom my data and calculations, I determined the rate of reaction (for concentration of HCl 0.25 to 2.00M) to be mingled with 0.24 and 1.14 (respectively) 11.68%.The rate of reaction is affected by a number of factors. change magnitude the concentration of reactants will usually cause the rate of reaction increase. A higher concentration will mean that there is more of the reactant to conflict together and react.By measuring the volume of gas (hydrogen) evolved at each concentration, I was able to calculate the rate of reaction for each of the concentrations.The volume of gas evolved increases as the concentration of HCl (aq) increase, as does the rate of reac tion (the gradient of line graph 1). However, the graph showing the rate of concentration against average volume of gas (i.e. showing the rate of reaction) begins to level off at 1.25M, and not 1.00M, as I hypothesised.This could be associated to one or umpteen of the random or systematic errors, resulting in 11.68% uncertainty for the value of rate of reaction. It could also be that my hypothesis was proved wrong on this account.There is no standard rate of reaction, as it is different for each trial, since the rate of reaction is dependent on concentration. There is not single rate of reaction for this type of experiment.EvaluationVariablePossible ProblemsPreventionTemperature of Hydrochloric AcidIf the temperature increases, it could be the cause of any change in rate of reaction & would mask the effects of the change in concentrationThe flask was placed in a water bath set at 30oC in order to keep it at a constant temperature & eliminate this as an independent variableVolume of Hydrochloric AcidIf the volume varies, it could be trustworthy for an increase or decrease in the rate of reaction & it would not be a reliable experiment20cm3 of hydrochloric acid was used for any experimentMass of Magnesium PowderIf the mass increases, it would alter the rate of reaction & would cause inaccurate results0.06g of magnesium powder was used for any experiment