Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂ (g) NO(g) +0(g) k₁ 2 O(g) +NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₂ « k₂. That is, the first step is much slower than the second. - Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. e rate = k 2

Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂ (g) NO(g) +0(g) k₁ 2 O(g) +NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₂ « k₂. That is, the first step is much slower than the second. - Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. e rate = k 2

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...

See similar textbooks

Similar questions

The following equation represents a reversible decomposition: CaCO3(s)CaO(s)+CO2(g) Under what conditions will decomposition in a closed container proceed to completion so that no CaCO3 remains?
Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the decomposition of ammonium carbonate (NH4)2CO3(s)2NH3(g)+CO(g)+H2O(g) is endothermic. Would the smell of ammonia increase or decrease as the temperature is increased?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
Which reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?
For the following reaction C(s)+2H2(g)CH4(g) K=0.26 at 1000C (3 significant figures). What is the equilibrium constant at 750C (3 significant figures)?
In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research associated with biofuels is the identification and development of suitable catalysts to increase the rate at which fuels can be produced. Do a web search to find an article describing biofuel catalysts. Then, write one or two sentences describing the reactions being catalyzed, and identify the catalyst as homogeneous or heterogeneous.
The reaction for the decomposition of ammonia into its elements ist 2 NH (a) Na (a) +3 Ha (a) [H.)= 0.414M, If the concentrations at a certain time are: [N] 0.0105 M [NH) = 0.505M what will be the associated value of the reaction quotient (a)? (A) (B) (C) 0.00148 0.00292 0.00861 (D) (E) 0.0105 342
For the reaction N2(g) + 3 H2(g) 2 NH3(g) at 25.0°C, the Kc of the reaction is 5.4 ✕ 105. Use the given concentrations to determine the following. [N2] = 0.0024 M [H2] = 0.0047 M [NH3] = 0.20 M (a) Determine Q at this time. (Omit units.)(b) Determine which direction the reaction will proceed in order to reach equilibrium.
Consider the elementary reactions and their rate constants. kf = 4.99 × 10–2s-1 k, = 3.67 × 10-' s-' A(g) + B(g) → C(g) + D(g) C(g) + D(g) A(g) + B(g) What is the equilibrium constant (K) of the following generic reaction? A(g) + B(g) = C(g) + D(g) Ke = Which statement correctly describes the partial pressures of the reactants and products at equilibrium? The partial pressures of the reactants are greater than the partial pressures of the products at equilibrium. The partial pressures of the products are greater than the partial pressures of the reactants at equilibrium. The partial pressures of the reactants and products are equal at equilibrium.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H, (g) + 2NO (g) → N,0 (g)+ H,0 (g) k1 H, (g) + N,0 (g) → N2 (g) + H20 (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k|| Note: your answer should not contain the concentrations of any intermediates.
Balance the following equations and express the rate of the following reactions in terms of the change in concentration of the reactants pr products. NH3 (g) + O2 à NO (g) + H2O (g)