The reaction: NO2(8) ---> NO(g) + 1/2O2(e) is second order and it takes 46 seconds for...
1a. The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) → 2 NO2(g) The reaction is second order with respect to NO(g) and first order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.6 x 102 M–2 s–1. When the initial concentrations of NO and O2 are 0.02 M and 0.015 M, respectively, the rate of the reaction is ___ M/s. 1b. The rate constant of a first-order decomposition reaction is 0.014...
The rate constant for the second-order reaction: 2N02(g)-→ 2NO(g) + O2(g) is 0.54/M s at 300°C 2 M to 0.28 Mn (a) How long (in seconds) would it take for the concentration of NO2 to decrease from 0.6 (b) Calculate the half-lives at these two concentrations.
The thermal decomposition of NO2: 2 NO2(g) → 2 NO(g) + O2(g) takes place in two steps: (1) 2 NO2(g) → NO3(g) + NO(g) (slow) (2) NO3 → NO(g) + O2(g) (fast) Which of the following statements is true? a. Rate = k [NO2] b. The reaction is second order in NO2. c. The reaction is first order in O2. d. Increasing [NO2] has no effect on reaction rate. e. All the above.
Question 9 10 poin The following decomposition reaction of NO2 is a second order reaction with a rate constant of 0.255 M-1-1 NO2(g) NO(g) +0 (8) If the reaction begins with 0.010 M of NO2, what would be the concentration of NO2 after 200 seconds? a. 0.0066 M 6.0.0204 M OC. 0.0196 M O d. 0.0071 M Moving to the next question prevents changes to this answer. Question MacBook 80 F3 DII F8 11 DOO F4 F10 F9 F5 F6...
The rate constant for this second-order reaction is 0.940 M1s-1 at 300 °G A products How long (in seconds) would it take for the concentration of A to decrease from 0.670 M to 0.290 M? Number
The rate constant for the second order reaction is 0.200 How long in seconds would it take for the concentration of A to decrease from 0.830 M to 0.240 M
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
12. Use Hess's Law to find AH for this reaction. (5) NO2(g) +2H2(g) ---> 2H2O(e) + NHs(g) Given the following two equations: 2NH3(g) -->N2(g) + 3H2(g) AHo +92 kJ 2N2(g)+ 2H2O(l) ---> NO2(g) + 2H2(g) AH° = +170 kJ
The decomposition of nitrogen dioxide occurs according to the equation below: NO2 (g)------>NO( g)+1/2 O2 (g) The reaction is second order with respect to NO2. The specific rate constant for this reaction is 3.04M-1min-1. How long does it take for the concentration of NO2 to decrease from 2.00M to 1.25M?
The rate constant for this second-order reaction is 0.400 M-'.5' at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.770 M to 0.360 M? R. T U T O P F G H J K L NM <