The combustion of ammonia is shown below:4NH:(g) + 50:(g) → 4NO(g) + 6H20(g)Write an equation that relates the rates of consumption of the reactants and the rates offormation of the products.At 298 °C, the rate of reaction (v) is 2.7 x 10 mol L-'s. Find the rate change of NH3,O2, NO and H20.(ii)

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Answered: The combustion of ammonia is shown…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Given the following values of the enthalpy (DH) and activation energy (Ea) of four different reactions, identify an exothermic reaction that would exhibit the fastest rate at 298 K. (Assume that all reactants have the same initial concentration and the same Arrhenius frequency factor A in k = Ae-Ea/RT). (A) DH = +45 kJ/mol; Ea = 75 kJ/mol; (B) DH = +35 kJ/mol; Ea = 65 kJ/mol; (C) DH = -35 kJ/mol; Ea = 75 kJ/mol; (D) DH = -45 kJ/mol; Ea = 65 kJ/mol;
5.) For the reaction X + Y ↓ Z; the reaction rate is found to depend only upon the concentration of X. A plot of 1/[X] verses time gives a straight line. What is the rate law for this reaction?
1. Consider the reaction for the production of urea used in synthesizing fertilizers: Answer the following. + 2NH30) CO2 (9) CO(NH,)2() + H200) During the analysis, a student found that the rate of ammonia consumption is 5.45 x 103 What was the rate (a) CO, was reacting? (b) CO(NH,), was being formed? (c) H,0 was being produced?
The oxidation of ammonia produces nitrogen and water via the following reaction: 4NH3(g) + 302(g) → 2N2(g) + 6H₂O(A) Suppose the rate of formation of H₂O(A) is 3.0 mol/(Ls). Which of the following statements is true? The rate of consumption of NH3 is 2.0 mol/(L. s). The rate of consumption of O₂ is 2.0 mol/(L. s). The rate of formation of N₂ is 1.3 mol/(Ls). The rate of formation of N₂ is 2.0 mol/(Ls). The rate of consumption of NH3 is 0.50 mol/(L. s).
The reaction C,H¿(g) 2C,H,(g) has an activation energy of 262 kJ/mol. At 600.0 K, the rate constant, k, is 6.1 x 10-8 s-!. What is the value of the rate constant at 770.0 K? k = * TOOLS х10
18. Which of these reactions appear to involve a catalyst? In those cases where a catalyst is present, tell whether it is homogeneous or heterogeneous. a) CH,COOCH,(aq) + H,O(() CH,COOH(aq) + CH,OH(aq) Rate = k[CH,COOCH,[H,O"] b) H;(g) +1(g) - Rate = k[H,][I,] +2 HI(g) %3D
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
The reaction described by the equation O3 (g) + NO(g) 0,(g) + NO,(g) has, at 310 K, the rate law rate of reaction = k[O¸][NO] k = 3.0 x 106 M-1-s-! Given that [O,] = 8.0 x 10-4 M and [NO] = 3.0 x 10-3 M at t = :0, calculate the rate of the reaction at t = 0. rate: M/s What is the overall order of this reaction? 3
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(a) Consider the combustion of ammonia, given below: 4 NH3(g) + 5 O2(g) --------> 4 NO(g) + 6 H2O(g) If NH3(g) is decreasing at the rate of 0.130 mol/s, what are the rates of change of O2(g), NO(g), and H2O(g)?O2(g)/t = _____ mol/s
While developing a catalytic process to make ethylene gly-col from synthesis gas (CO +H₂), a chemical engineer finds therate is fourth order in gas pressure. The uncertainty in the pres-sure reading is 5%. When the catalyst is modified, the rate increases by 10%. If you were the company patent attorney,would you file for a patent on this catalyst modification? Explain.
Consider the following reaction in aqueous solution: 5Br-(aq) +BrO3-(aq) +6H+(aq)→ 3Br2(aq) + 3H2O(l) If the rate of disappearance of Br–(aq) at a particular moment during the reaction is 2.5 x 10–4 mol L–1 s–1, what is the rate of appearance of Br2(aq) at that moment? Question 2 options: a) 2.1 x 10–4 mol L–1 s–1 b) 1.5 x 10–4 mol L–1 s–1 c) 7.2 x 10–4 mol L–1 s–1 d) 9.4 x 10–4 mol L–1 s–1

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