Rate increases and increases the frequency of

Rate of reaction is affected by some factors such as concentration of reactant.When the concentration of one or more reactants increase, the higher the number of particles in a unit per volume.The frequency of collisions between the particles increases and increases the frequency of effective collisions.Hence, the rate of reaction increases.

Besides, the rate of reaction also caused by the surface area of reactant.The larger th totak surface area exposed,the higher the rate of reaction.By increasing the total surface area of reactant, there are more collision per unit of time. Temperature is the factor as well.The higher the temperature,the particles of reactants will collide more frequently per unit time and become more energetically due to the collisions..The frequency of collisions between the particles increase and hence it increase the frequency of effective collisions.

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Therefore, the rate of reaction is increases.(Jessie & David,n.d.) Arrhenius equation was originally formulated by J.J. Hood on the basis of studies of the variation of rate constants of some reactions with temperature. The Swedish chemist Svante Arrhenius, for whom the equation is named, showed that the relationship is applicable to almost all kinds of reactions.

The Arrhenius equation is a mathematical expression that expressed the effect of temperature on the velocity of a chemical reaction.It is the basis of all predictive expressions used for calculating reaction-rate constants. In the Arrhenius equation, k is the reaction-rate constant, A and E are numerical constants characteristic of the reacting substances, R is the thermodynamic gas constant, and T is the absolute temperature which is in the unit of Kelvin. The equation is commonly given in the form of an exponential function,k = Aexp(?E/RT),and it predicts that a small increase in reaction temperature will produce a marked increase in the magnitude of the reaction-rate constant.

(Encyclopedia Britannica, 2017)The Arrhenius equation,k=Ae?Ea/RT(1)can be written in a non-exponential form that is often more convenient to use and to interpret graphically. Taking the logarithms of both sides and separating the exponential and pre-exponential terms yieldslnk=ln(Ae?Ea/RT)=lnA+ln(e?Ea/RT)(2)(2)ln?k=ln?(Ae?Ea/RT)=ln?A+ln?(e?Ea/RT)lnk=lnA+?EaRT=(?EaR)(1T)+lnA(3)(3)ln?k=ln?A+?EaRT=(?EaR)(1T)+ln?Awhich is the equation of a straight line whose slope is –Ea?/R–Ea?/R. This affords a simple way of determining the activation energy from values of k observed at different temperatures, by plotting lnkln?k as a function of 1/T1/T.(Chemistry Libretext,2017)


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