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1 points Save Answe QUESTION 8 Choose the balanced reaction for which the following rate relationships...
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.
10) Write a balanced reaction for which the following rate relationships are true. 1 Δ[N2] = Δ[02] = 1 Δ[N20] Rate- 2 At
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...
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...
For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: O3(g)+2NO2(g)→N2O5(g)+O2(g) Step 1: O3(g)+NO2(g)→NO3(g)+O2(g) slow Step 2: NO3(g)+NO2(g)→N2O5(g) fast View Available Hint(s) For the overall reaction below, which of the following is the correctly written rate law? Overall reaction: Step 1: slow Step 2: fast A.] Rate=k[O3][NO2]2 B.] Rate=k[O3][NO2] C.] Rate=k[NO3][NO2] D.] Rate=k[O3][NO2]2[N2O5][O2]
Question 15 1 pts Given the following balanced equation, determine the rate of reaction with respect to [SO2). 2 SO2(g) + O2(g) +2 SO3(s) Rate A[S02] 24t Rate = 24[S02] At Rate = -2A(SO2] At Rate = -A[S02] 2Δt Rate Δt -2A(SO2] Rate = -2At A[S02] Rate = 2At A[S02]
- When the following reaction is at equilibrium, which of these relationships is always true? Se 2 03(g) = 3 O2(g) -) K[O3)2 = [O213 str(0.5 pt) 3) [03] = [O2] SEP ) Kc[02]2 = [03] ) K[02]3 = [O3)2 S -) [O3)2 = [02]3.
The rate of the following reaction expressed in terms of the appearance of Oz is 4[O2l. 2 Δt 2N2Os → 4NO2 + O2. An equivalent expression for the rate of this reaction is: 010 010 (a) AN205] Δt (b) +14N-Osl 2 At 8 to find stets iw 1910 bora of ol beveiled ai co Bris 01:06 to noticoqmos 5° 2 18 (c) .14N2Os]. At (9): 09:05 10:05 - ) (d) .14NO21 foristsqmstift in Ollo stile srit ei tort 4 Δt...
a Choose the balanced equation for the following half-reaction, which takes place in acidic solution НВFO,(ag) —> Вr (aq) 4 8e7H (aq) + HBr04 (aq) -> Br (aq) + 4H20(1) 8e H (aq)HBrO4 (aq) -> Br (aq)4H20() Se + 7H* (ag) + HBFO, (ag) — 2Br (аq) + 4H20() Зе + 7H* (ад) + HBFO4(ag) — Br (aq) + 4H20() b Choose the balanced equation for the following half-reaction, which takes place in acidic solution NO3 (ag) > NО2(9) 3e2H...
QUESTION 8A Consider the reaction 2 N2O5 --> 4 NO2 + O2. A chemist studying the kinetics of the reaction monitored the concentration of N2O5 as a function of time at 45°C, and obtained the data below. Time (s) [N2O5] (M) 0 0.100 50 0.0707 100 0.0500 200 0.0250 300 0.0125 400 0.00625 What is the order of the reaction? 0 1/2 1 2 QUESTION 8A Use the data from question 8 to determine the value of the rate constant for...