CHEMISTRY.pptx
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This document discusses the temperature dependence of reaction rates. It notes that increasing temperature causes an exponential increase in the reaction rate constant based on the Arrhenius equation. The Arrhenius equation quantitatively relates the reaction rate constant to temperature, the activation energy, and a frequency factor. Specifically, a higher temperature results in a higher percentage of reactant molecules possessing kinetic energy exceeding the activation energy threshold, thereby increasing the reaction rate.
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Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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- 1. Name: Kumar Ashutosh Class: 12 ‘B’ Roll no: 3322 Subject: Chemistry Topic: Temperature dependence of rate of reaction Submitted to: Kapishwar Ji Parmeshwari Devi Dhanuka Sarswati Vidya Mandir
- 2. RATE OF REACTION: The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. Reactant concentration, the physical state of the reactants, and surface area, temperature, and the presence of a catalyst are the four main factors that affect reaction rate. We will discuss the about the factor of effect of temperature on rate of reaction
- 3. Temperature dependence of the rate of a reaction Activation energy comes into play. A reaction occurs when the reactant molecules clash with each other, according to collision theory. The threshold energy is the smallest amount of energy that colliding molecules must have in order for their collision to be effective. The activation energy is the lowest additional amount of energy absorbed by the reactant molecules in order for their energy to equal the threshold value. Threshold energy = Activation energy + Energy possessed.
- 4. Arrhenius equation The Arrhenius equation can quantitatively explain the temperature dependency of the rate of a chemical process. k = Ae-Ea/RT The Arrhenius factor, also known as the frequency factor or pre-exponential factor, is represented by A. Ea is the activation energy in joules/mole, and R is the gas constant. The fraction of molecules with kinetic energy larger than Ea is represented by the factor e-Ea/RT.
- 5. As a result of the Arrhenius equation, it has been discovered that increasing the temperature or decreasing the activation energy causes an increase in the reaction rate and an exponential increase in the rate constant. Taking both sides of the equation’s natural logarithm ln k = -(Ea/RT) + ln A A straight line with slope is drawn when ln k vs 1/T is plotted = -(Ea/R) and intercept = ln A At temperature T1, equation ln k1 = Ea/RT1 + ln A At temperature T2, equation ln k2 = Ea/RT2 + ln A For a given reaction, A is constant. The values of rate constants for temperatures T1 and T2 are k1 and k2, respectively. Subtracting equation form, ln k2 – ln k1 = (Ea/RT1) – (Ea/RT2) ln (k2/k1) = Ea/R ((1/T1)-(1/T2)) log k2/k1 = (Ea/2.303R) × ((1/T1)-(1/T2)) log k2/k1 = (Ea/2.303R) × ((T2-T1)/(T1T2))
- 6. Graphical description of effect of temperature Plotting a fraction of molecules with particular kinetic energy versus kinetic energy for two distinct temperatures T1 and T2 illustrates this. The number of molecules having those levels of kinetic energy is proportional to the area under the curve. At T1 and T2, the entire area is the same. The fraction of molecules with kinetic energy greater than Ea at T1 and T2 are represented by the areas (a) and (b). This means that when the temperature rises, the percentage of molecules having energies greater than Ea rises. As a result, the velocity of the reaction quickens.
- 7. .