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

omenTo determine the outrank of reception forResearch enquireWhat effect does the niggardness of hydrochloric blistering have on the appreciate of reaction when combined with magnesium demolish?HypothesisI hypothesise that the passel of heat content sport produced will increase at a steep, but steady measure as the assiduity of hydrochloric acrimonious increases, until the concentration is equal to 1.0 mol dm-3. Therefore, the roam of reaction will remain constant until this point. I suggest this concentration be originator the surviveard concentration of hydrochloric biting utilise in general experiments is usually 1 mol dm-3. I then theorize that the set out of reaction will gradually falling off until the slope of the graph (effect of increasing concentration of HCl against the pot of hydrogen produced line graph 1) becomes 0. unsettledsType of VariableVariableEnsured byDependent Variable* era Taken* Timed using bear time* Volume of Hydrogen Gas Produced* Experiment iterate three time & Average taken freelancer Variable (quantitative)* Concentration of HCl(aq)* 8 concentrations were employControlled Variables* Temperature* piddle john was used* Thermometer placed in urine bath* Mass of magnesium* Used a 3 d.p. balance* Surface Area of Magnesium* Used powder & made sure survey was the same* Volume of Hydrochloric Acid* A burette was used to measure volumeRequirements* water bath (30oC)* 500cm3 conical flaskfulful* rubber stopper* speech communication tubing* measuring cylinder* clamp stand* stop clock* 0.06g magnesium powder* 20cm3 hydrochloric acid* 3 d.p. balance* spatula* weighing boat* burette (x2)* thermometer in water sewer* safety lookApparatusTechnical Notes1) The magnesium powder should be as pure as possible. It should be stored in a clean and dry environment to stop that no impurities (such as effects of oxidation) prevent the appealingness of accurate data.2) Eye protection is necessary imputable to the use of hydrochloric acid tiny bubbles may lawsuit irritation of eyes.3) Rubber, instead of cork, must be used as the material for the bungs. Cork is too holey and will leak.4) No naked flames should be exhibit hydrogen splatter is extremely flammablemethod acting1. The solutions were prepared with a mensural combination of hydrochloric acid and water, to produce 8 different concentrations of 20cm3 hydrochloric acid2. The frame-up was set up as shown in the diagram. The trough was half filled with water3. The measuring cylinder was filled with water, and remained full whilst being turned turned (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 each feature escaping. The stop clock was started.5. The volume of the gas was then calm in the measuring cylinder, measured and recorded after(prenominal) 30 seconds6. Steps 3-5 was repeated three multiplication with fresh materials, and an average vol ume of gas collated was calculated for that concentration7. This process (steps 1-6) was repeated for the 7 new(prenominal) concentrations (0.25 2.00M)8. The rate of reaction was then calculated for separately 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 between 0.24 and 1.14 (respectively) 11.68%.The rate of reaction is affected by a bend of factors. Increasing the concentration of reactants will usually suffice the rate of reaction increase. A higher concentration will mean that there is more of the reactant to bump around 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 concentratio n of HCl (aq) increase, as does the rate of reaction (the gradient of line graph 1). However, the graph screening 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 genius or many of the random or dictatorial errors, resulting in 11.68% uncertainty for the value of rate of reaction. It could withal 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 qualified on concentration. There is not single rate of reaction for this type of experiment.EvaluationVariable doable ProblemsPreventionTemperature of Hydrochloric AcidIf the temperature increases, it could be the cause of any change in rate of reaction & would screen the effects of the change in concentrationThe flask was placed in a water bath set at 30oC in order to restrain it at a constant temperature & eliminate this as an independent variableVolume of Hydrochloric AcidIf the volume varies, it could be responsible for an increase or decrease in the rate of reaction & it would not be a reliable experiment20cm3 of hydrochloric acid was used for all experimentMass of Magnesium millIf the mass increases, it would alter the rate of reaction & would cause inaccurate results0.06g of magnesium powder was used for every experiment