{"id":1286,"date":"2020-06-23T15:09:09","date_gmt":"2020-06-23T19:09:09","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chbe220\/?post_type=part&p=1286"},"modified":"2020-07-30T15:50:46","modified_gmt":"2020-07-30T19:50:46","slug":"chapter-2-reaction-chemistry","status":"publish","type":"part","link":"https:\/\/pressbooks.bccampus.ca\/chbe220\/part\/chapter-2-reaction-chemistry\/","title":{"raw":"Reaction Chemistry","rendered":"Reaction Chemistry"},"content":{"raw":"

Introduction<\/h2>\r\nIn a chemical process, the rate of production is limited by the rate of reaction in the reactors. This chapter introduces methods to predict the rate of reaction and concentration of components. The reactions are analyzed using rate law, reaction equilibrium and reaction mechanisms. By learning this chapter, we can gain knowledge to select the optimal conditions for maximum production rate and model the productivity of our process.\r\n
\r\n

Learning Objectives<\/p>\r\n\r\n<\/header>\r\n

\r\n\r\nBy the end of this chapter, you should be able to:\r\n\r\nCalculate<\/strong> the reaction rate for the reaction and rate of formation of compounds\r\nCalculate<\/strong> the reaction\u00a0extent\r\nDetermine<\/strong> reaction order and rate constant from kinetic data\r\nAnalyze<\/strong> equilibrium reaction equations\r\nExplain <\/strong>the effect of temperature on reaction rates\r\nAnalyze<\/strong> elementary reactions, reaction molecularity\r\nSelect<\/strong> the rate-determining step given the consecutive reactions and overall rate law of the reaction\r\nDerive<\/strong> the rate law of a reaction using steady-state approximations to pre-equilibria assumptions\r\nUnderstand<\/strong> kinetic and thermodynamic control\r\n\r\n<\/div>\r\n<\/div>\r\n \r\n\r\nAs you are going through this chapter, some important terms for you to take note of:\r\n
    \r\n \t
  • Reaction rate<\/li>\r\n \t
  • stoichiometric coefficient<\/li>\r\n \t
  • molarity<\/li>\r\n \t
  • partial pressure<\/li>\r\n \t
  • reaction rate law<\/li>\r\n \t
  • rate constant<\/li>\r\n \t
  • reaction order in a substance<\/li>\r\n \t
  • overall order<\/li>\r\n \t
  • isolation method<\/li>\r\n \t
  • method of initial rates<\/li>\r\n \t
  • linearize the equation<\/li>\r\n \t
  • integrated rate law<\/li>\r\n \t
  • zeroth\/first\/second-order rate laws<\/li>\r\n \t
  • half-life<\/li>\r\n \t
  • equilibrium constants<\/li>\r\n \t
  • Arrhenius equation<\/li>\r\n \t
  • frequency factor<\/li>\r\n \t
  • activation energy<\/li>\r\n \t
  • catalysts<\/li>\r\n \t
  • reaction mechanism<\/li>\r\n \t
  • elementary reactions<\/li>\r\n \t
  • intermediates<\/li>\r\n \t
  • molecularity<\/li>\r\n \t
  • unimolecular reaction<\/li>\r\n \t
  • bimolecular reaction<\/li>\r\n \t
  • consecutive elementary reactions<\/li>\r\n \t
  • steady-state approximation<\/li>\r\n \t
  • rate-determining step<\/li>\r\n \t
  • pre-equilibria<\/li>\r\n \t
  • kinetic control<\/li>\r\n \t
  • thermodynamic control<\/li>\r\n<\/ul>\r\n ","rendered":"

    Introduction<\/h2>\n

    In a chemical process, the rate of production is limited by the rate of reaction in the reactors. This chapter introduces methods to predict the rate of reaction and concentration of components. The reactions are analyzed using rate law, reaction equilibrium and reaction mechanisms. By learning this chapter, we can gain knowledge to select the optimal conditions for maximum production rate and model the productivity of our process.<\/p>\n

    \n
    \n

    Learning Objectives<\/p>\n<\/header>\n

    \n

    By the end of this chapter, you should be able to:<\/p>\n

    Calculate<\/strong> the reaction rate for the reaction and rate of formation of compounds
    \nCalculate<\/strong> the reaction\u00a0extent
    \nDetermine<\/strong> reaction order and rate constant from kinetic data
    \nAnalyze<\/strong> equilibrium reaction equations
    \nExplain <\/strong>the effect of temperature on reaction rates
    \nAnalyze<\/strong> elementary reactions, reaction molecularity
    \nSelect<\/strong> the rate-determining step given the consecutive reactions and overall rate law of the reaction
    \nDerive<\/strong> the rate law of a reaction using steady-state approximations to pre-equilibria assumptions
    \nUnderstand<\/strong> kinetic and thermodynamic control<\/p>\n<\/div>\n<\/div>\n

     <\/p>\n

    As you are going through this chapter, some important terms for you to take note of:<\/p>\n

      \n
    • Reaction rate<\/li>\n
    • stoichiometric coefficient<\/li>\n
    • molarity<\/li>\n
    • partial pressure<\/li>\n
    • reaction rate law<\/li>\n
    • rate constant<\/li>\n
    • reaction order in a substance<\/li>\n
    • overall order<\/li>\n
    • isolation method<\/li>\n
    • method of initial rates<\/li>\n
    • linearize the equation<\/li>\n
    • integrated rate law<\/li>\n
    • zeroth\/first\/second-order rate laws<\/li>\n
    • half-life<\/li>\n
    • equilibrium constants<\/li>\n
    • Arrhenius equation<\/li>\n
    • frequency factor<\/li>\n
    • activation energy<\/li>\n
    • catalysts<\/li>\n
    • reaction mechanism<\/li>\n
    • elementary reactions<\/li>\n
    • intermediates<\/li>\n
    • molecularity<\/li>\n
    • unimolecular reaction<\/li>\n
    • bimolecular reaction<\/li>\n
    • consecutive elementary reactions<\/li>\n
    • steady-state approximation<\/li>\n
    • rate-determining step<\/li>\n
    • pre-equilibria<\/li>\n
    • kinetic control<\/li>\n
    • thermodynamic control<\/li>\n<\/ul>\n

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