Rate laws

  • Thread starter viciousp
  • Start date
1. The problem statement, all variables and given/known data
The rate of teaction
O(g) + NO2(g) --> NO(g) +O2(g)
was studied at a certain temperature.
NO2 is in a large excess at 1.0x10^13 molecules/cm^3

Data:
Time............................[O](atoms/cm^3)
0.................................5.0x10^9
1.0X10^-2....................1.9X10^9
2.0X10^-2.....................6.8X10^8
3.0X10^2......................2.5^10^8

The reaction rate is know to be first order with respect to NO2. Determine the overall rate law and value of rate law constant

2. Relevant equations
k[A]=rate


3. The attempt at a solution
Ok I know that a O is a first order rate so the overall rate law is k[O][NO2]=Rate. The slope of ln[O] vs t is 99.8. So now how do you find the constant?

I think its k(1.0x10^13)(5.0x10^9)=99.8
so k= 2.0x10^-21 cm^3/atoms * s ,but something doesn't seem right about it
 

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