reaction rates
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By Carolyn Stevens and Alyce Casey. Reaction rates. Collision Theory. The collision theory is the process where the reacting particles collide, with enough energy to break the bonds and reconstruct them to form a new product. - PowerPoint PPT PresentationTRANSCRIPT
By Carolyn Stevens and Alyce Casey
The collision theory is the process where the reacting particles collide, with enough energy to break the bonds and reconstruct them to form a new product.
Activated Complex – the partial bonding that occurs in the brief moment between bond disruption and bond formation
Activation Energy – the minimum amount of energy required in order for an effective collision to occur
Energy of Reaction (ΔH)
Activation Energy
Nature of the Reactantsweak bond → increases collision efficiency → faster reaction
Surface Area (only affects solids)
crushing → increases surface area → increases collision frequency → faster reaction
Concentration (only affects liquids and gases)
increased pressure (gases only) → increases concentration → more particles → increases collision frequency → faster reaction
Temperature (endothermic and exothermic)
increased temperature → higher Ek → faster particles → increases collision frequency → faster reaction
Catalyst (creates an alternate path for the reaction without being changed)
catalyst → lower energy barrier → increases collision frequency → faster reaction
t[product]
t[reactant]
RreactΔ
Δ
Δ
Δ
In the decomposition reaction2 N2O5(g) → 4 NO2(g) + O2(g)
that takes place in 1.5L of pure carbon tetrachloride solution, 0.04 moles of O2 are produced over 5.7 minutes.
Calculate (a) the rate of production of O2 gas and (b) the loss of N2O5 (g).
2Omin / L / moles0047.0min 5.7*L 1.5
moles 0.04
Δ
Δ
t[reactant]
Rreact
Answer to part (a):
Answer to part (b):
(0.047 mol/L/min)(2) = 0.0094 mol/L/min N2O5
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