The reaction
2NOBr → 2NO + Br2
exhibits the rate law
Rate = k[NOBr]2 ![The reaction 2NOBr → 2NO + Br<sub>2</sub><sub> </sub>exhibits the rate law Rate = k[NOBr]<sup>2</sup> where k = 1.0 × 10<sup>-5</sup> M<sup>-1</sup> • s<sup>-1</sup> at 25° C. This reaction is run where the initial concentration of NOBr ([NOBr]<sub>0</sub>) is 1.00 × 10<sup>-1</sup> M. -The [NO] after 1.00 h has passed is A) 9.7 × 10<sup>-3</sup> M B) 9.9 × 10<sup>-3</sup> M C) 1.0 × 10<sup>-3</sup> M D) 3.5 × 10<sup>-4</sup> M E) none of these](https://d2lvgg3v3hfg70.cloudfront.net/TB6422/11eaaf91_9deb_65cc_892c_478d3d53b46d_TB6422_11_TB6422_11.jpg)
where k = 1.0 × 10-5 M-1 • s-1 at 25° C. This reaction is run where the initial concentration of NOBr ([NOBr]0) is 1.00 × 10-1 M.
-The [NO] after 1.00 h has passed is
A) 9.7 × 10-3 M
B) 9.9 × 10-3 M
C) 1.0 × 10-3 M
D) 3.5 × 10-4 M
E) none of these
Correct Answer:
Verified
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