3.1.9 Rate equations

• The rate of reaction is the change in concentration of a reactant or product in a unit of time
• The overall order of a reaction is the sum of all the individual orders
• Zero order reaction

  Reaction is zero order with respect to A

  This means the rate of reaction is constant and independent of the concentration of A

  A) rate

  B) Concentration

  C) Time

  D) Concentration

  
• First Order raction

  Eg. Rate = K[A]^1

  > Reaction is first order wit respect to A

  > If the concentration of A is doubled then the rate doubles.

  A) Rate

  B) Concentration

  C) Concentration

  D) time

  
• Scond Order reaction

  Rate = K [A]^2

  • The reaction is second order with respect to A
  • If the concentration of A is doubled (2^2) then the rate goes up 4 times

  second order reaction

  Rate = K[A][B] can't draw cause there are 2 reactants

  • the reaction is first order w.r.t A
  • The overall Order of the reaction is (I+1) = second order

  A) rate

  B) Concentration

  C) Concentration

  D) Time

  
• The constant of proportionality in a rate equation, value of which is dependent on temperature and activation energy of the reaction

  • The rate constant, exponentially increases with temperature
  • The rate also exponentially increases with temperature
• > The Arrhenius equation Shows the effect that changing temperature. or the activation energy has on the rate constant.

  k = rate constant

  A = Arrhenius constant

  Ea = activation energy

  T = temperature in kelvin

  R = gas constant

  $k=$$Ae^{{\frac {-E_{a}}{RT}}}$

  lnk = y axis

  1/T = x axis

  -Ea/R = m / gradient

  lnA = c

  
  

  $lnk =$$-Ea/RT +$$lnA$