Nitrogen dioxide reacts with carbon monoxide by the overall equation NO:(9) + CO(g) → NO(9) + CO2 (9) At a particular temperature, the reaction is second order in NO, and zero order in CO. The rate constant is 0.515 L/(mol - s). How much heat energy evolves per second initially from 7.25 Lof reaction mixture containing 2.40 x 102 M NO,? NO: (9) + NO(g) + co(g) -110.5 kJ/mol + CO2(9) -393.5 kJ/mol AH; = 33.10 kl/mol. 90.29 kJ/mol Assume the enthalpy change is constant with temperature. Energy = kJ/s

Nitrogen dioxide reacts with carbon monoxide by the overall equation NO:(9) + CO(g) → NO(9) + CO2 (9) At a particular temperature, the reaction is second order in NO, and zero order in CO. The rate constant is 0.515 L/(mol - s). How much heat energy evolves per second initially from 7.25 Lof reaction mixture containing 2.40 x 102 M NO,? NO: (9) + NO(g) + co(g) -110.5 kJ/mol + CO2(9) -393.5 kJ/mol AH; = 33.10 kl/mol. 90.29 kJ/mol Assume the enthalpy change is constant with temperature. Energy = kJ/s

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.68QE

See similar textbooks

Similar questions

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)?
Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.
During polymerization, the system usually becomes more ordered as monomers link together. Could an endothermic polymerization reaction ever occur spontaneously? Explain.
The combustion of carbohydrates and the combustion of fats are both exothermic processes,yet the combustion of carbohydrates is a faster process.How can this be?
What is the rate law for the reaction? Show work and explain.
Calculate the rate constant,k, for the reaction about. Show work and include units Rate= k[No]^2[H2]^1
The thermal decomposition of ozone in the gas phase is thought to proceed via the reactive intermediate, oxygen atom; overall: 2 O_3 --> 3 O_2. Mechanism: O_3 --> O_2 + O k_1 O + O_2 --> O_3 k_2 O + O_3 --> 2 O_2 k_3 Apply the steady-state approximation and obtain an expression for the rate of loss of ozone, d[O_3]/dt. You may assume that [O_2] is large and unchanging. (show all work)
33. The four hydrocarbons of lowest molar mass are methane, ethane, propane, and butane. All are used extensively as fuels in our economy. Calculate the thermal energy transferred to the surroundings per gram (the fuel value) of each of these four and rank them by this quantity. 19. Why are homogeneous catalysts harder to separate from products and leftover reactants than are heterogeneous reactants? PS. If you will just answer 1 question because of the HONOR CODE please answer the number 33 question. But If youre willing to help me in this subject please also answer the 2 questions. Thank you.
The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1
Below are the proposed elementary steps and enthalpies for the mechanism of burning coal, C(s). (1, fast) C(s) + H2O(g) ⇌ CO(g) + H2(g) ΔH1 = 100 kJ/mol (2, slow) CO(g) + H2O(g) ⟶ CO2(g) + H2(g) ΔH2 = –300 kJ/mol (3, fast) 2 H2(g) + O2(g) ⇌ 2 H2O(g) ΔH3 = –200 kJ/mol a. Write the net reaction. Identify each of the molecules as either a reactant, product, intermediate, or catalyst. b. Write the rate law for the reaction corresponding to the mechanism above Need step-by-step solution Answer: (a) Net reaction: C(s) + O2(g) ⟶ CO2(g) (b) Intermediates: CO(g), H2(g), Catalyst: H2O (c) Rate = (K1K2/K-1)sqrtK3/sqrtk -3[H2O][O2]1/2
In the presence of O2, NO reacts with sulfur-containing proteins to form S-nitrosothiols, such as C6H13SNO. This compound decomposes to form a disulfide and NO:2C6HSNO(aq)------>2NO(g)+C12H26S2(aq) The following data were collected for the decomposition reaction at 100°C. Time (s) [C6H13SNO] (aq) 0 1.08 x 10-3 10 7.77 x 10-4 20 5.46 x 10-4 30 3.79 x 10-4 Calculate the value of the first-order rate constant for the reaction.