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Rate of Rreaction Between Sodium Thiosulfate and Dilute Hydrochloric Acid

            Investigating the rate of reaction between sodium thiosulfate and dilute hydrochloric acid.
            
            
             Sodium thiosulphate + Hydrochloric acid  Sodium Chloride + Sulfur Dioxide + Sulfur + Water .
             Balanced Symbol Equation for this reaction is:.
             Na2S2O3 (aq) + 2HCL (aq)2NaCl (aq)+SO2 (g)+H2O (l) .
             Collision Theory .
             The rate of a reaction is all about collision theory. The collision theory is "the theory that reactions happen when molecules collide." The theory helps to explain the factors that affect the rates of chemical change. "[1] But not all collisions between molecules lead to a reaction. Collisions are only successful when the molecules possess the minimum energy which can break the bonds between atoms to create new molecules. This is called the activation energy. The Rate of a reaction should increase if the number of successful collision per second also increases. .
             These are the factors that affect the rate of reaction for this particular reaction: .
             Temperature of the reactants: As the temperature increases the kinetic energy of the molecules also increases, meaning that there will be more random, frequent, harder, and more successful and fruitful collisions between the particles. At low temperatures or when you decrease the temperature, the rate of reaction decreases because the molecules have less kinetic energy; therefore they move around slower so collisions become weaker and more infrequent. .
             When the temperature is increased it increases the energy of the particles meaning that they are greater than or equal to the activation energy, so at lower temperature the number of particles with the energy required to match the activation energy is less. As a result this means that the reaction is not as fast or successful. Concentrations of reactants in solution: In reactions which involve liquids, increasing the concentration of the solution increase the rate of reaction. This is because there is a greater chance of the molecules colliding frequently, resulting in a faster reaction.


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