Consider this reaction. 2N0_2(g) + F_2(g) rightarrow 2NO_2F(g) The rate equation
ID: 1071037 • Letter: C
Question
Consider this reaction. 2N0_2(g) + F_2(g) rightarrow 2NO_2F(g) The rate equation for this reaction is: rate = k [NO_2] [F_2] Which mechanism is consistent with the rate law? 2NO_2(g) + F_2(g) rightarrow 2NO_2 F(g) NO_2(g) F_2(g) rightarrow NO_2F(g) + F(g) (fast) NO_2(g) + F(g) rightarrow NO_2F(g) (slow) F_2(g) rightarrow 2F(g) (fast) 2NO_2(g) + 2F(g) rightarrow 2NO_2F(g) (slow) NO_2(g) + F_2(g) rightarrow NO_2F(g) +F(g) (slow) NO_2(g) + F(g) rightarrow NO_2F(g) (fast) The decomposition of hydrogen peroxide is described by the equation: 2H_2O_2(aq) rightarrow 2H_2O(l) + O_2(g) The reaction is first order in H_2O_2. It takes 10.0 hours for the concentration of H_2_O_2 to drop from 0.500 M to 0.250 M. How many hours are required for the concentration of H_2O_2 to drop from 0.400 M to 0.100 M? 38.0 h 24.0 h 20.0 h 12.0 hExplanation / Answer
(8) (D) Because the slow reactions 1 NO2 and 1 F2. So, rate depends on first power of NO2 and first power of F2.
(9) (C) 20 hr.
It follows first order kinetic. It is independent of intial concentration. t1/2 = 0.693 / k .
0.400 to 0.200 and 0.200 to 0.100
total 2 half lives so, 10 hrs + 10 hrs = 20 hrs