NO is an atmospheric pollutant that destroys ozone in the stratosphere. Here is the accepted mechanism: O3+ NO + NO2 + O2 (slow) NO2 +O + NO + O2 (fast) O3 +0 → 202 X Incorrect. Identify any catalyst in the mechanism. If none, enter none. Edit none eTextbook and Media Correct. Identify any intermediate in the mechanism. If none, enter none. NO,

For the following chemical Konction there are possible Reaction mechanisms as Shown STEP I Step 2 NET 2 co + Cl₂ → 2 Coll STEP 1 Step 2 REACTION MECHANISM I со - CO + Cl₂ ⇒ Coll + el C(Slow) (Fast) со coel اح tee Three MECHANISM I Cl₂ → 2 l (Slow) llz 2 ll + 10 + 2 coll (Fast)

3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640

A certain reaction is second order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4] Initial rate of reaction 2.41 M 0.733 M 19.0 M/s 0.501 M 0.733 M Mls 0.873 M 2.02 M Mls dlo Ar

Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data

The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.

10. The data below are for the reaction: 2 NO₂ (g) + F₂ (g) → 2 NO₂F (g) [NO₂] (M) 0.100 0.200 0.200 0.400 0.200 [F₂] (M) 0.100 0.100 0.200 0.400 0.400 Initial rate (M/s) 0.026 0.051 0.103 0.411 see part c a. Write the rate law for this reaction. b. Determine the rate constant for this reaction. Pay attention to units. c. Predict the initial rate of the reaction when [NO₂] = 0.200 M and [F₂] = 0.400 M. d. The mechanism of the reaction is suggested as two steps: NO₂+ F2 → NO₂F + F (fast) NO₂+ F→→ NO₂F (slow) Is your rate law consistent with this mechanism? Explain your answer, making any changes necessary to create consistency.

The rate of disappearance of HBr in the gas phase reaction 2HBr (g) is 0.301 M s-¹ at 150°C. The rate of appearance of Br₂ is 1.66 0.151 H2(g) + Br2 (g) 0.0906 0.602 0.549 M s-¹.

DUE NOW. Please answer it correctly. Thanks!