{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}

lecture 14 - chem

lecture 14 - chem - General Analytical Chemistry II...

Info iconThis preview shows pages 1–6. Sign up to view the full content.

View Full Document Right Arrow Icon
General & Analytical Chemistry II 1011-216 Winter 2008/2009 Lecture 14
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
General & Analytical Chemistry II Concentration vs. Time Rate = k[N 2 O 5 ] m Is often referred to as the differential rate law. If we sum the rate over successive time intervals we get [N 2 O 5 ] vs. t For a 1 st -order reaction the integrated rate law l n [N 2 O 5 ] = l n [N 2 O 5 ] o - kt l n(.1) = -2.3 [N 2 O 5 ] o = 0.1 mol/L
Background image of page 2
General & Analytical Chemistry II Zero-Order Reactions For A products - [A]/ t = k For zero-order reactions the rate is constant. Zero-order reactions are observed for many surface reactions. Integrated Rate Law [A] = [A] o – kt Unit of k mol/L.s t 1/2 = [A] o /2k
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
General & Analytical Chemistry II 1 st - Order Reactions For A products - [A]/ t = k[A] A graph of rate vs. concentration will have a slope of k. Radioactive decay follows 1 st - order kinetics. Integrated rate law: l n [N 2 O 5 ] = l n [N 2 O 5 ] o – kt Units of k (1/s) = s -1 t 1/2 = l n(2)/k l n(.1) = -2.3 [N 2 O 5 ] o = 0.1 mol/L
Background image of page 4
General & Analytical Chemistry II 2 nd - Order Reactions For A products - [A]/
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full Document Right Arrow Icon
Image of page 6
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}