01:160:162 Lecture 2: Chapter 15

• School: Rutgers University
• Department: Chemistry
• Course: 01:160:162
• Professor: Professor Klein- Juneau

Document Summary

The concentration of the reactant particles: 2. ) The structure and orientation of the particles: 3. ) Average rate of reaction: the average rate of reaction is calculated from any two-point interval, example: 2no2(g) -> 2no(g) + o2(g). )00. 50( s mol sl: the negative sign shows us that in a concentration is negative are using up the reactant. the change because we. 5 sl: d e p e n d e n c e o f r a t e o n. ]a[ t: using calculus, we get the equation in the form of a line (y = mx + b). and. If the initial concentration of n2o5 is 1. 65 x 10^-2 mol/l, what is the concentration of n2o5 after 825 seconds? ln[n kt. ]a[ t: using calculus, we get the equation in the form of a line (y = mx + b).