Question Determine the rate law and the value of k for the following reaction using the...

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Determine the rate law and the value of k for the following reaction using the data...

Determine the rate law and the value of k for the following reaction using the data provided. 2 N2O5(g) → 4 NO2(g) + O2(g) [ N2O5]i (M) Initial Rate (M-1s-1) 0.033 1.84 × 10-4 0.066 7.37 × 10-4 0.099 1.66× 10-3 A. Rate = 5.6 × 10-1 M-1/2s-1[N2O5]3/2 B. Rate = 1.7 × 10-1 M-1s-1[N2O5]2 C. Rate = 1.7 × 10-1M1/2s-1[N2O5]1/2 D. Rate = 6.0 × 10-1 M-2s-1[N2O5]3 E. Rate = 5.2 × 10⁻1 s-1[N2O5]
Part A Determine the rate law and the value of k for the following reaction using...

Part A Determine the rate law and the value of k for the following reaction using the data provided: 2NO(g) + O2(g) + 2NO2(9) [NO]; (M) [Ogl (M) Initial Rate (M4 st) 0.030 0.0055 8.55 x 103 0.030 0.0110 1.71 x 10-2 0.0055 3.42 x 10-2 0.060 Rate = 3.1 x 105 M-3 s[NO]2[0212 Rate = 57 M' s'[NO][O21 Rate = 9.4 x 103 M25 *[NO][0212 Rate = 3.8 M-1/2 s [NO](O2) 1/2 Rate = 1.7 x 103 M2 s?[NO]2[02]
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate =...

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...

Determine the rate law and the value of k for the following reaction using the data...

Determine the rate law and the value of k for the following reaction using the data provided. 2 NO(g) + Br2(g) → 2 NOBr(g) [NO]i (M) [Br2]i (M) Initial Rate (Ms-1) 0.030 0.0055 1.81 x 10-2 0.030 0.0110 3.62 x 10-2 0.060 0.0055 7.25 x 10-2 please show step by step.
For the overall reaction below, which of the following is the correctly written rate law? Overall...

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]
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0...

The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0 x 10-5 s-1, what is the reaction rate when the N2O5 concentration is 0.0091 mol L-1? 2.The decomposition of acetaldehyde, CH3CHO, was determined to be a second order reaction with a rate constant of 0.0771 M-1 s-1. If the initial concentration of acetaldehyde is 0.301 M , what will the concentration be after selected reaction times? a. What will the CH3CHO concentration be after...

If molecular oxygen is reacting at a rate of 0.024 M/s in the following reaction; 4...

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...
1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq)...

1) Determine the rate law and the rate constant given the data below. 2 MnO4 (aq) + 5 C103(aq) + 6 H+(ag) Experiment Mn04] 0.10 2 0.25 3 0.10 4 0.10 2 Mn2+ (aq) + 5 C104 (aq) + 3 H20 (1) [C103] [H] Initial Rate(M/s) 0.10 0.10 5.2 x 10-3 0.10 0.10 3.3 x 10-2 0.30 0.10 1.6 x 10-2 0.10 0.20 7.4 x 10-3
A reaction obeys the rate law: rate = k [A]2[B]. At some set of concentrations, the...

A reaction obeys the rate law: rate = k [A]2[B]. At some set of concentrations, the rate is found to be 8.2 x 10-2 M/sec. What will be the rate of reaction if the concentration of A is halved and the concentration of B is doubled? A. 4.1 x 10-2 M/sec B. 8.2 x 10-2 M/sec C. 5.0 x 10-1 M/sec D. 1.6 x 10-1 M/sec

Part A Determine the rate law and the value of k for the following reaction using...

Part A Determine the rate law and the value of k for the following reaction using the data provided. SO82 (aq) + 3 l'(aq) 2 SO42-() + 13 "(aq) [S,08?) (M) (0) (M) Initial Rate (M's) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33 O Rate = 86 M?s" [S,08? Rate = 36 M 's' (S203 2701 Rate = 120 M2 [S208 2 101 Rate - 23 M-1/2" [S2O3 1912 Rate = 195 Mºss,Og 2012 Submit Request Answer