A kinetic study of the reaction between aqueous sodium thiosulphate and hydrochloric acid :: GCSE Chemistry Coursework Investigation

A kinetic conceive of the response betwixt aqueous atomic number 11 thiosulphate and hydrochloric dotAim To press come to the fore out a complete kinetic study of the chemical reception amongaqueous sodium thiosulphate and hydrochloric acidEquation Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + S(s) + SO2(g) + H2O(l)PART ATo recoup the order of the reaction with respect to the densitysof sodium thiosulphate and hydrochloric acid the experiment pass on becarried out at uniform temperature and the age interval amongst the step-up of HCl and the obscuring of the sign muck up on white piece of music bythe secure yellow sec precipitate go forth be measurable for a regularvolume of solution that uses 3 varying concentrations of Na2S2O3(aq) art object maintaining the concentration of HCl(aq) and 3 varyingconcentrations of HCl(aq) while maintaining the concentration of Na2S2O3(aq).The rate of the reaction nominate be determined by the calculating theamount of sulphur produced i n the date recorded. This is given by theequationRate = beat of sulphur sentenceThe amount of sulphur needed to obscure the cross is assumed to be thesame in each reaction so therefore,Rate = 1TimeThen, the data will be situated in a table to determine the strength ofconcentration on the rate of reaction and hence the order of some(prenominal)reactants can be formed. Adding up both orders of the reactants givesthe overall order of the reaction.PART BTo distinguish out the issue of temperature on the rate of the reaction the term interval between the addition of HCl and the obscuring of the inkcross on white paper by the solid yellow sulphur precipitate at louverdifferent temperatures moldinessiness be recorded. A chart showing time takenvs. temperature will produce a curve showing the effect of varyingtemperature on the rate of reaction.The Arrhenius equation ln k = ln A (Ea / RT) can be shown diagrammatically by plotting a graph of ln (t) against ln (1/T). Thegradient of this graph = - (Ea / RT) which can be used to calculateactivation energy. The y-intercept of the line = ln A where A is theArrhenius constant for the reaction.HypothesisThe rate of a chemical reaction can be obtained by finding out thechange in amount (or concentration) of a particular reactant orproduct over the time taken for this change.M any factors affect the rate of a reaction, ace of which isconcentration. For any reaction to happen, the reactant particles mustfirst collide. This is true whether both particles are in solution, orwhether one is in solution and the other is a solid. If theconcentration is higher, there are more particles in the same volumeA kinetic study of the reaction between aqueous sodium thiosulphate and hydrochloric acid GCSE Chemistry Coursework InvestigationA kinetic study of the reaction between aqueous sodium thiosulphate and hydrochloric acidAim To carry out a complete kinetic study of the reaction betweenaqueous sodium thiosulphate and hydroch loric acidEquation Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + S(s) + SO2(g) + H2O(l)PART ATo deduce the order of the reaction with respect to the concentrationsof sodium thiosulphate and hydrochloric acid the experiment will becarried out at constant temperature and the time interval between theaddition of HCl and the obscuring of the ink cross on white paper bythe solid yellow sulphur precipitate will be measured for a constantvolume of solution that uses 3 varying concentrations of Na2S2O3(aq)while maintaining the concentration of HCl(aq) and 3 varyingconcentrations of HCl(aq) while maintaining the concentration of Na2S2O3(aq).The rate of the reaction can be determined by the calculating theamount of sulphur produced in the time recorded. This is given by theequationRate = Amount of sulphurTimeThe amount of sulphur needed to obscure the cross is assumed to be thesame in each reaction so therefore,Rate = 1TimeThen, the data will be placed in a table to determine the effect ofconcentration on the rate of reaction and hence the order of bothreactants can be formed. Adding up both orders of the reactants givesthe overall order of the reaction.PART BTo find out the effect of temperature on the rate of the reaction thetime interval between the addition of HCl and the obscuring of the inkcross on white paper by the solid yellow sulphur precipitate at fivedifferent temperatures must be recorded. A graph showing time takenvs. temperature will produce a curve showing the effect of varyingtemperature on the rate of reaction.The Arrhenius equation ln k = ln A (Ea / RT) can be showngraphically by plotting a graph of ln (t) against ln (1/T). Thegradient of this graph = - (Ea / RT) which can be used to calculateactivation energy. The y-intercept of the line = ln A where A is theArrhenius constant for the reaction.HypothesisThe rate of a chemical reaction can be obtained by finding out thechange in amount (or concentration) of a particular reactant orproduct over the time taken fo r this change. some(prenominal) factors affect the rate of a reaction, one of which isconcentration. For any reaction to happen, the reactant particles mustfirst collide. This is true whether both particles are in solution, orwhether one is in solution and the other is a solid. If theconcentration is higher, there are more particles in the same volume