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Half Life Of Second Order Reaction. 1 0.9 [ a] ∘ = k 2 t 10 % + 1 [ a] ∘. 2 [ a] 0 = 1 [ a] 0 + 2 k t 1 / 2.
Difference between order and molecularity of a reaction 2310 from www.slideshare.net
Minus 1 / [ a] 0 from each side. 2 [ a] 0 = 1 [ a] 0 + 2 k t 1 / 2. By definition, the half life of any reaction is the amount of time it takes to consume half of the starting material.
Difference between order and molecularity of a reaction 2310
T 1 / 2 = 1 2 k [ a] 0. T 1 / 2 = 1 2 k [ a] 0. T 1 / 2 = 1 k [ a] 0. For a 1st order reaction (half life is constant.) for a second order reaction (half life increases with decreasing concentration.) for a zero order reaction a products , rate = k:
