#8. Kinetics

#8. Kinetics - -4 to 3.959x10-4 . So when the reactant is...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
Technical Abstract When the concentration of H 2 O 2 (hydrogen peroxide) and KI (potassium iodide) was decreased, the rate constant was increased but the rate was decreased. However, when the temperature was decreased, the rate constant and the rate both were decreased. When the concentration of H 2 O 2 was decreased from 0.7M to 0.35M, the initial rate was changed from 1.7x10 -5 M/s to 5.71x10 -6 M/s and the rate constant was changed from 3.469x10 -4 to 4.661x10 -4 . When the concentration of KI was decreased from 0.1M to 0.05M, the initial rate was decreased from 1.7x10 -5 M/s to 9.7x10 -6 M/s and the rate constant was increased from 3.469x10
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: -4 to 3.959x10-4 . So when the reactant is increased, the rate of decomposition gets faster. And the rate is faster at higher temperature. The mechanism for this reaction is H 2 O 2 + I- IO-+ H 2 O and H 2 O 2 + IO- I-+ H 2 O + O 2 . The rate determining step is first step. It is slowest step in the mechanism and rate=k[H 2 O 2 ] x [KI] y is the ideal(theoretical) rate law when the first step is the rate determining step. Its reactants are H 2 O 2 and KI (or I) while the reactants of the second step are H 2 O 2 and IO which is an intermediate (something will disappear)....
View Full Document

Ask a homework question - tutors are online