Multiple Choice
The decomposition of N2O5(g) to NO2(g) and O2(g) obeys first-order kinetics. Assume the form of the rate law is
Rate ![The decomposition of N<sub>2</sub>O<sub>5</sub>(g) to NO<sub>2</sub>(g) and O<sub>2</sub>(g) obeys first-order kinetics. Assume the form of the rate law is Rate where k = 3.4 × 10<sup>-5</sup> s<sup>-1</sup> at 25°C. -The reaction A → B + C is known to be zero order in A with a rate constant of 3.8× 10<sup>-2</sup> mol/L • s at 25° C. An experiment was run at 25°C where [A]<sub>0</sub> = 1.0 × 10<sup>-3</sup> M. What is the rate after 6.5 minutes? A) 1.0 × 10<sup>-3</sup> mol/L • s B) 3.8 × 10<sup>-2</sup> mol/L • s C) 3.8 × 10<sup>-5</sup> mol/L • s D) 3.7 × 10<sup>-4</sup> mol/L • s E) 1.5 × 10<sup>-11</sup> mol/L • s](https://d2lvgg3v3hfg70.cloudfront.net/TB6422/11eaaf91_9dea_f09a_892c_a9519fd66c83_TB6422_11_TB6422_11_TB6422_11.jpg)
where k = 3.4 × 10-5 s-1 at 25°C.
-The reaction A → B + C is known to be zero order in A with a rate constant of 3.8× 10-2 mol/L • s at 25° C. An experiment was run at 25°C where [A]0 = 1.0 × 10-3 M. What is the rate after 6.5 minutes?
A) 1.0 × 10-3 mol/L • s
B) 3.8 × 10-2 mol/L • s
C) 3.8 × 10-5 mol/L • s
D) 3.7 × 10-4 mol/L • s
E) 1.5 × 10-11 mol/L • s
Correct Answer:
Verified
Correct Answer:
Verified
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