Write a balanced reaction for which the following rate
relationships are true:
Rate = -1/2 delta[N2O5] over delta t = 1/4 delta[NO2] over delta t
= delta]O2] over delta t
a. 2N2O5 yields 4NO2 + O2
b. 4NO2 + O2 yields 2N2O5
c. 2N2O5 yields NO2 + 4O2
d. 1/4 NO2 + O2 yields 1/2 N2)5
e. 1/2 N2O5 yields 1/4 NO2 + O2
Can someone please describe WHY the answer is A? Please show work.
a. 2N2O5 yields 4NO2 + O2
2N2O5 -------> 4NO2 + O2
-1/2[N2O5]/t = +1/4[NO2]/t = +[O2]/t
Ex xA + yB ------> zC
-1/x[A]/t = -1/y [B]/t = +1/z[C]/t
Write a balanced reaction for which the following rate relationships are true: Rate = -1/2 delta[N2O5]...
1 points Save Answe QUESTION 8 Choose the balanced reaction for which the following rate relationships are true. -A[N2O5] A[NO2] 4[NO2] 4[02] rate 2 At 4Δt Δt 2 N 205 - NO 2 + 402 01/21 2015 - / NO 2 + 02 2 N 205 4 NO 2 + O2 4 NO 2 + O2 2 N 205 NO 2 +02 - įN 205
10) Write a balanced reaction for which the following rate relationships are true. 1 Δ[N2] = Δ[02] = 1 Δ[N20] Rate- 2 At
for the following first-order reaction, what would be the rate at 2 Molarity concentration of N2O5 if the rate constant is 4.8×10^-3 s^-1. 2N2O5 (soln)->4NO2 (soln)+O2 (soln)
Consider the rate of decomposition: 2 N2O5(g) → 4NO2(g) + O2(g). The rate of reaction will be dependent on: A. [N2O5] B. [NO2] C. [O2] D. [NO2] and [O2]
3. The rate of decomposition of N2O5 in the reaction 2 N2O5(g) 4 NO2(g) + 5 O2(g) at a particular instant is 4.2 x 10-7 M/s, what is the rate of appearance of NO2?
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...
Just need help with d[N2]/dt please 18.1 Nitrogen pentoxide (N205) gas decomposes according to the reaction 2N2O5 = 4NO2 + O2 At 328 K, the rate of reaction v under certain conditions is 0.75 X 10-4 mol L-75-1. Assuming that none of the interme- diates have appreciable concentrations, what are the values of d[N2O5]/dt, d[N2]/dt, and d[02]/dt?
If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4 NO2(g) + O2(g) → 2 N205(8) at what rate is N2O5 being formed? O 0.048 M/s 0.096 M/S 0.024 M/s 0.012 M/s The rate law for the reaction 2 NO, +O3 -- N2O5 + O, is rate - k[NO][03]. Which one of the following mechanisms is consistent with this rate law? NO2 + NO2-N202 + O2 (slow) N2O2 +O3-N20s (fast) NO2+O3 -NO3 + O2...
please answer these question For the following reaction: 2 N2O5 (g) 4NO2 (g) + O2 (g) the initial rate of formation of O, was found to be 1.25 x 10-4 mol dms-1. What is the initial rate of consumption of N2O5? 2.50 x 10-4 mol dm's-1 1.25 x 10-4 mol dm-35-1 O 3.75 x 10-4 mol dm's-1 05.00 10-4 mol dm3s-1 A second order reaction, A + P has a rate constant k = 0.05 dmº mol-1 3-1 and an...
Please show work I am not getting the correct answers 1. Hydrogen peroxide, H2O2, decomposes spontaneously through the following reaction. 2H2O2(aq) 2H2O(g) + O2(g) The kinetics are second order, and the half‐life is 17.3 min when a 1.75 M solution of H2O2 is made. What is the concentration of the solution after 24.8 min? 2. The decomposition of N2O5 occurs by the following reaction: 2N2O5(g) 4NO2(g) + O2(g) The rate constant is experimentally determined to be 3.4 x 10‐4 s‐1....