The catalyzed reaction: 2SO2 + O2 – 2SO3 is thought to occur by the following mechanism Step 1: 2NO + O2 → 2NO2 slow Step 2: 2NO2 + 2SO2 → 2NO + 2SO3 fast
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Identify the intermediate |
answer 1 |
Write the rate law for the reaction. |
answer 2 |
Identify the catalyst. |
answer 3 |
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- Methanoic acid, HCOOH(aq) , is a monoprotic acid that can be synthesized by the reaction between CO and NH3 in the presence of hydronium ions. A proposed mechanism for the reaction consists of the three elementary steps shown below.Step 1: CH3 OH + CO → HCO2CH3 slowStep 2: HCO2CH3 + NH3 → HCONH2 + CH3 OH fast Step 3: HCONH2 + H3 O+ → HCOOH + NH4 + fast Overall reaction: CO + NH3 + H3 O+ → HCOOH + NH4 + ΔHrxn = −81 kJ/molrxn(a) Write the chemical formula of a species that behaves as a catalyst in the mechanism.(b) According to the proposed mechanism, if additional NH3 is added to the reaction mixture, will the rate of the overall reaction increase, decrease, or remain the same? Justify your answer.Methanoic acid, HCOOH(aq) , is a monoprotic acid that can be synthesized by the reaction between CO and NH3 in the presence of hydronium ions. A proposed mechanism for the reaction consists of the three elementary steps shown below.Step 1: CH3 OH + CO → HCO2CH3 slowStep 2: HCO2CH3 + NH3 → HCONH2 + CH3 OH fast Step 3: HCONH2 + H3 O+ → HCOOH + NH4 + fast Overall reaction: CO + NH3 + H3 O+ → HCOOH + NH4 + ΔHrxn = −81 kJ/molrxn1. The following data were collected from the alkaline hydrolysis reaction of t-butylbromide to t-butyl alcohol as: (CH3)3CBr à alkaline hydrolysis à (CH3)3COH a. At concentration 0.5 M the rate was 0.005 (mol/L.s) b. At concentration 1.5 M the rate was 0.015 (mol/L.s) If you know that: Rate2 / Rate1 = ([A2] / [A1])m Find out the followings: a. The reaction order b. The reaction constant c. The half-life of the reaction.
- The active ingredient in an over the counter pain killer analgesic decomposes with a rate constant, k = 9.05 × 10−4 day−1. How many days does it take for 15% of the original ingredient to decompose?The following reaction mechanism was proposed for this reaction: (1) To2 → 2To [slow] (2) 2To + O2 → 2ToO [fast] (3) 2ToO + To2 → 2To2O [fast] What would be the molecularity of step? Would this be a possible mechanism for this reaction? ExplainA compound decomposes by a first-order process. If 28 % of the compound decomposes in 60 minutes, the half-life of the compound is ________minutes. A. 127 B. 28 C. -18 D. 33 E. -5
- Overall Reaction: A2 + BC4 → AB + AC4 The proposed mechanism is as follows: A2 ⇋ 2A (fast) A + BC4 → AB + AC3 (slow) A + AC3 ⇋ AC4 (fast) What is the rate law?What is the molecularity of the rate limiting step for the mechanism below? Step 1: H2O2 (aq) + I–(aq) → H2O(l) + OI–(aq) (slow)Step 2: H2O2 (aq) + OI–(aq) → H2O(l) + O2 (g) + I–(aq) (fast)If the rate constant in a first-order degradation reaction of a drug product is 0.462/year, what is the shelf-life of the drug product in months?
- 11. Propose a mechanism for the chemical reaction below. Which step in your mechanism is rate-determining?1) If the reaction order of reactant A is 1, and the reaction order of reactant B is 2, what is the overall reaction order? 2) How is the value of the rate constant determined? 3) How does the value of the rate constant effect the reaction rate?Consider the following reaction: X_Y + Z >2X + D, The proposed mechanism of this reaction is below: Step 1: X2Y = 2x + Y (fast) Step 2: Y + Z>D (slow) Based on the mechanism, what is the overall order of this reaction.