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4 X = 1 O 1 2 3 4 Rate [Br 03] 0.001 0.002 0.001 0.001 bc be be bc bc 3 Brz reaction: 0.00 5 0.005 0.001 0.001 [Br] 0.005 Y 0.001 = K [B₁03] [Br]² 2° = 1 2'=2 2² = 4 23=8 24=16 + 3 H₂O = 2.50e-4 1.00€-3 0.5% = 0.25 y = 2 [H+] 0.100 0.100 0.100 0.200 New Rate lx old rate 2x old rate 4x old rate 8x old rate 16x old rate 0.112 0.2 0.5² = 1 Z O = 1 Rate m/s • Unimolecular: I molecule, always 1st order • Bimolecular: collision of 2 molecules, always 2nd order • Termolecular: Collision of 3 molecules (rare) 2.50e-4 5.00e-4 1.00 e-3 1.00 e-3 - Elementary Reaction processes that occur in a single event/step - Molecularity of a reaction: # of molecules that are reactants in an elemento Step - A chemical equation is the net statment of rxn chanses -Reaction Mechanism: complete reaction process • Multistep Mechanism: Sequence of elementary Steps • Must add up to net • Intermediate product of I step used as a reactant in another step - Ex/ 2 NO₂ → NO₂ + NO NO₂ + CO → NO₂ + CO₂ NO₂+ CO NO + CO₂ - Rate - Determing Step: slowest step in a multistep reaction that determines rate law Example: What is the rate determining step? Write the balanced equation for the overall reaction. 2 NO + 2 H₂ → N₂ + 2 H₂O Step 1: NO+NON₂Q₂ (fast) Step 2: N₂Q₂+H₂-N₂O+H₂O (slow) Step 3: N₂Q+H₂→N₂+H₂O (fast) Step 2 Are there any intermediates? If so, state what they are. N₂0 and N₂O₂ -Effective Collisions: particles must collide with proper orientation & energy in order to react - PE Diagrams PF enery needed to breakf bonds Reactants Activation Enersy (Activation complex. Time energy released Products - The PE diagram is reversed when reaction is reversed - Activation Energy: min amt of energy to start a chemical rxn - Transition State: point where particles have collided and are abt to form products - Activated Complex: assembly of atoms in an excited state btwn reactants and products