4. 13.67 The following diagrams represent the progress of the reaction AB, where the red spheres represent A molecules and the green spheres represent B mole- cules. Calculate the rate constant of the reaction. t=0 s 1 = 20 s t = 40 s

5. [30 pts] Two short questions on previous topics: A. The following two-step mechanism has been proposed for a certain aqueous reaction Step 1: ClO + ClO → ClO2+ Cl Step 2: ClO2 + CIO→ ClO3 + Cl¯ i. Write down the balanced equation for the overall (net) reaction. ii. Laboratory experiments give the following rate law for the reaction above: Rate = k[CIO¯]² If the two-step mechanism above is correct, which is the slow step? Explain your answer based on the laboratory result. B. Draw Lewis structures for the molecules below, and show the hydrogen-bonding interaction between the two molecules using a (...) symbol. ii. iii. i. CH2=O and H₂O CH3OH and CH3OH HF and HCN Hint: the atoms of HCN are connected in the order written.

a) Consider the combustion of butane, given below: 2 C4H10(g) + 13 O2(g)  8 CO2(g) + 10 H2O(g) If C4H10(g) is decreasing at the rate of 0.340 mol/s, what are the rates of change of O2(g), CO2(g), and H2O(g)?O2(g)/t =  ____ mol/sCO2(g)/t =  ____ mol/sH2O(g)/t =  ____ mol/s(b) The decomposition reaction given below: 2 IF5(g)  1 I2(g) + 5 F2(g) is carried out in a closed reaction vessel. If the partial pressure of IF5(g) is decreasing at the rate of 312 torr/min, what is the rate of change of the total pressure in the vessel?Ptot /t =  ______ torr/min

At a certain temperature the rate of this reaction is first order in N₂O5 with a rate constant of 0.0125 s¯¹: 2N₂O5 (g) → 2N₂O4 (8) + 0₂ (8) Suppose a vessel contains N₂O5 at a concentration of 1.14M. Calculate the concentration of N₂O5 in the vessel 88.0 seconds later. You may assume no of reaction is important. Round your answer to 2 significant digits.

3. (14.24 Brown) For each of the following gas-phase reactions, write the rate expression in term of the appearance of each product and the disappearance of each reactant: a. 2 H₂O(g) → 2H2(g) + O2(g) b. 2SO2(g) + O2(g) → 2 SO3(g) c. 2NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) d. N2(g) + 2H2(g) → N₂H4(g)

Step 1: (slow) Step 2: C0 (fast) = CI The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (03) in the upper atmosphere. Based on the models, which of the following represents a species that acts as a catalyst for the reaction? 88.8

Reaction of nitric oxide gas (NO) and chlorine gas (Cl2) produces a very poisonous gas called nitrosyl chloride (NOCl). The experimental data of the reaction is given below. Use the data to calculate the specific rate constant K and overall order of the reaction. Please show full work!

A chemical engineer is studying the rate of this reaction. H₂CO3(aq) → H₂O (aq) + CO₂ (aq) He fills a reaction vessel with H₂CO3 and measures its concentration as the reaction proceeds. Here's a graph of his data: (W) [O'H] 0.2. 02 Use this graph to answer the following questions: What is the half life of the reaction? Round your answer to 2 significant digits. I Don't Know t (s) Submit 1/2 = 1.5[s 25 M. tv 0 x10 5 Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use 中村区

12. The reaction was run at a higher temperatures. At 37.0 °C, the rate constant was measured to be 0.584 M-¹-¹ and at 120.0 °C, it was 10.641 M¹s. What is Ea (kJ/mol)? Give your answer in the #12 blank with 3 significant figures and units.

Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88