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2 H 2 + O 2 → 2 H 2 O

2 H 2 + O 2 → 2 H 2 O. +. 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.

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2 H 2 + O 2 → 2 H 2 O

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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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