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

A kinetic study of the answer between sedimentary atomic number 11 thiosulphate and hydrochloric acidAim To carry protrude a complete kinetic study of the reaction betweenaqueous sodium thiosulphate and hydrochloric acidEquation Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + S(s) + SO2(g) + H2O(l) affair ATo deduce the stage of the reaction with respect to the concentrationsof sodium thiosulphate and hydrochloric acid the experiment will becarried out at constant temperature and the time musical interval between the sum total of HCl and the obscuring of the ink bad-tempered on white paper bythe solid yellow sulphur precipitate will be mensurable for a constantvolume of beginning 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 bed be determined by the compute theamount of sulphur produced in the time recorded. This is given by the equationRate = Amount of sulphur clockThe amount of sulphur needed to mingled the cross is assumed to be thesame in each reaction so in that locationfore,Rate = 1 clippingThen, the data will be laid in a table to determine the piece ofconcentration on the rate of reaction and hence the order of bothreactants brush off 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 calculateenergizin g 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 the deepen in amount (or concentration) of a particular reactant orproduct over the time taken for this change.M both factors mask 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 settlement, 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 hydrochloric acidEquation Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + S(s) + SO 2(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 ca n 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 for this change.Many factors affect the rate of a reaction, one o f 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