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Factors Affecting the Rate of Chemical Reactions: Collision Theory Explained

This article explores the key factors influencing the rate of chemical reactions, including temperature, concentration, particle size, pressure, and the presence of catalysts. Utilizing Collision Theory, we explain how each factor impacts the frequency and energy of particle collisions. Aspects such as increased surface area and concentration result in higher reaction rates, while the nature of reactants also plays a crucial role. Additionally, we discuss how temperature changes can dramatically alter reaction speeds, emphasizing the importance of these factors in chemical kinetics.

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Factors Affecting the Rate of Chemical Reactions: Collision Theory Explained

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  1. 2 H2 + O2 → 2 H2O +

  2. Identify the factors that could affect the rate of a chemical reaction. • Use the Collision Theory to explain the factors influencing the rate of a reaction. • Explain the effect these factors have on the shape of a kinetic energy distribution curve.

  3. Factors Affecting Reaction Rates • temperature • concentration or pressure of a reactant • surface area (particle size) • presence/absence of a catalyst. • nature of the reactants

  4. Effect of Particle Size (surface area) Rate of reaction increases with increased surface area(crushing, grinding) . More particles involved, more frequent collisions.

  5. Effect of Concentration Rate of reaction increases with increased concentration (mol/L) of particles. Moreparticles with activation energy - more chances of a successful collision.

  6. Effect of Pressure Only affects reaction rates of gaseous reactions. Rate of reaction increases with decreased volume of the container - mimics higher [ ]. Closer particles – more chance of collisions.

  7. Effects of a Temperature Change Rate of reaction increases with increased temperature. MoreKEperparticles – more frequentcollisions and moreEA.

  8. 10°C increase in temp usually doubles reaction rate.

  9. Effect of the Nature of Reactants 1. Comparing reactions with similar compounds: Less bonds to break, faster the reaction. 2 NO(g) + O2(g) → 2 NO2(g) 2 C8H18(g) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)

  10. 2. Comparing reactions with similar bond numbers: Covalent bonds takes longer to break than aqueous. (aq) are already separated into ions, so are instantaneous. H2(g) + I2(g) → 2 HI(g) KNO3(aq) + NaI(aq) → KI(aq) + 2 NaNO3(aq)

  11. KNO3(aq) + NaI(aq)→ KI(aq) + NaNO3(aq) Na+ K+ I- NO3-

  12. 3. Comparing similar compounds and similar bond numbers: (g) faster> (l) > (s) • Stronger IMF to overcome • Less KE per particle • Less collisions • Less Surface area

  13. Effect of Catalysts A catalyst speeds up or starts a reaction by lowering the activation energy. • Does not alter products or ΔH. • Not involved in the overall chemical reaction • Appears unchanged. Enzymes are known as biological catalysts. An inhibitor is the opposite of a catalyst.

  14. Things that increase reaction rate: • increased surface area • increased concentration • increased pressure • increased temperature • fewer bonds, aqueous or gas states • catalyst To decrease reaction rate - do the opposite....

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