ir this yellow highlighted line is really confuse me and I c n t understand that line ease you on pen paper tell me in simple

Question

ir this yellow highlighted line is really confuse me and I c n t understand that line ease you on pen paper tell me in simple way Fraction of molecules 10 Energy of activation This area shows fraction of molecules reacting at t This area shows fraction of additional molecules which react at 10 Kinetic energy Fig 4 9 Distribution curve showing temperature dependence of rate of a reaction temperature is raised the maximum of the curve moves to the higher energy value Fig 4 9 and the curve broadens out i e spreads to the right such that there is a greater proportion of molecules with much higher energies The area under the curve must be constant since total probability must be one at all times We can mark the position of E on Maxwell Boltzmann distribution curve Fig 4 9 Increasing the temperature of the substance increases the fraction of molecules which collide with energies greater than E It is clear from the diagram that in the curve at t 10 the area showing the fraction of molecules having energy equal to or greater than activation energy gets doubled leading to doubling the rate of a reaction In the Arrhenius equation 4 18 the factor e Ea RT the fraction of molecules that have kinetic energy greater than E corresponds to Taking natural logarithm of both sides of equation 4 18 E In k In A RT 4 19 The plot of In k vs 1 T gives a straight line according to the equation 4 19 as shown in Fig 4 10

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