This preview shows pages 1–2. Sign up to view the full content.
This preview has intentionally blurred sections. Sign up to view the full version.View Full Document
Unformatted text preview: with k = 0.810 M-1 s-1 at 10 o C. We start with 4.00 X 10-3 M NOBr in a flask at 10 o C. How many seconds does it take to use up 1.50 X 10-3 M of NOBr? 2 NOBr(g) N 2 (g) + O 2 (g) + Br 2 (g) Compounds A and B react to form C and D in a reaction that was found to be second order in A. The rate constant at 30 o C is 0.622 liters per mole per minute. What is the t 1/2 of A when 4.10 X 10-2 M A is mixed with excess B? A + B C + D Temperature and Rates The rate constant is tripled when T increases from 298K to 308K. Find E a . Mechanisms NO 2 + CO NO + CO 2 by experiment: Rate = k[NO 2 ] 2 2 NO + Br 2 2 NOBr Rate = k[NO] 2 [Br 2 ] 3 rd order (1) NO + Br 2 NOBr 2 (fast) k 1 /k-1 (2) NOBr 2 + NO 2 NOBr (slow) k 2 2 NO + Br 2 2 NOBr...
View Full Document
- Winter '07