The following reaction is first order with respect to fe^+3with a rate constant
ID: 899519 • Letter: T
Question
The following reaction is first order with respect to fe^+3with a rate constant of 3.0 time 10^-5 2.3 time 10^3sec 2.3 time 10^4sec 2.3 time 10^3 none the overall order for a reaction having the following rate law r= k[A]^1[b]^1/2 is 1 1/2 3/2 -3/2 For the reaction: 2NO_2 right arrow O3right arrow N2o5,+ O_2, .the following mechanism O3+ NO_2 NO3 + O_2. k1slow NO3 + NO_2 N2O5k2. Fast Therefore the Rate Law should be K = k2[NO3][NO_2] R =k2 [O3][NO_2]R = kt[o3][N02lR =k[N02] ^2[O3]1 A reaction was found to be third-order In "A". Increasing the concentration of A y factor of 3 will cause the reaction rate to A. remain constant Increase by a factor of 27 increase by a factor of 9D. triple The equilibrium expression Kc depends on the of the reaction. A mechanism stoichiometry rate pressure The equilibrium expression Kc = [H_2]2[02]1/[H_20]2 describes the next reaction 2H_2(g) + 02(g) U 2H_20(g) H_20(g) H_2(g) + 1/202(g) H_20(g) 0 2H(g) + 0(g) 2H_20(g) U 2H_2(g) + 02(g)Explanation / Answer
5. B. 2.3 x 104 sec (t1/2 = 0.693 / k)
6. D. 3/2 (1+1/2 = 3/2)
7. C. R= k1 [O3] [NO2]
8. B
9. D Since, Kc = Kp (RT)Delta n
10. D
11. B (Reverse the reaction, take square root and change the sign since the rxn is reversed)
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