Part A In the gas phase, the reaction between O2 and NO produces NO2. Define the reaction rate in terms of the disappearance of O2, and use the steady-state approximation to determine the rate law predicted by this mechanism. O2 + 2NO NO2 The reaction is proposed to occur via the following mechanism: Drag the appropriate labels to their respective targets. 2NO N2O2 O2 + N2O2 2NO2

9. The reaction 3C A + 2B occurs in one step in the gas phase. In each blank below, write the exponent of the concentration in the FORWARD rate law or write none if that concentration does not appear in the rate law.   [A] ........... [B] .......... [C] ...........

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A. Consider the following proposed mechanism for the production of chlorine dixoide from chlorine and ozone. Draw a reaction coordinate diagram for this reaction. Label reactants, products, transition states, intermediates, and activation energy on your sketch. Assume the reaction is endothermic. NOTE: CI is chlorine, not Carbon lodide Overall: Cl₂ (g) + 203 (g) → 2 CIO₂ (g) + O₂ (g) Step 1: Cl₂ (g) → 2 Cl (g) fast Step 2: Cl (g) + Os (g) CIO₂ +O fast Step 3: O (g) + O3 (g) → 202 (g) fast Step 4: Cl (g) + O2 (g) → CIO2 (g) slow

for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction

Consider the overall reaction 2A + B ⇌ 2C(g) with proposed mechanism for this reaction: A + B ⇌ C + D (slow) A+D ⇌ C (fast)What is the rate law for this proposed mechanism?

The mechanism for the reaction described by NO₂(g) + CO(g) → CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) NO₂(g) + NO(g) k₂ (2) NO3(g) + CO(g) → NO₂(g) + CO₂(g) Assuming that [NO] is governed by steady-state conditions, derive the rate law for the production of CO₂ (g). rate of CO₂ (g) production =