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Unformatted text preview: CHAPTER 16 Reaction Rate : should always be positive-(change in concentration of A/change in time) [A]/[t] Rate Law: - Must be determined experimentally- Can NOT get from the coefficients!- = K[A] m [B] n units of mol/Ls or Ms-1 o k depends on reaction temperature, pressure and presence of a catalyst First order reactions: ln([A] t /[A] ) = - kt Second order reactions: 1/[A] t = kt + 1/[A] Zero order reactions: [A] t = [A] kt Arrhenius Equation: K = Ae-Ea/RT ln(K 2 /K 1 ) = - (Ea/R)(1/T 2 1/T 1 ) CHAPTER 17: If temperature is increased: equilibrium shifts AWAY from heat!- In an endothermic reaction, equilibrium shifts right, products INCREASE!- In an exothermic reaction, equilibrium shifts left, products DECREASE! If temperature is decreased: equilibrium shifts TOWARDS heat!...
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This note was uploaded on 04/07/2011 for the course BIOL 104 taught by Professor Bray-speth during the Spring '11 term at Saint Louis.
- Spring '11