9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N₂O, and water. 2NO+H₂)------- NO + H₂O In a series of experiments, the following initial rates of disappearance of NO were obtained: Show work Initial Concentrations Initial Rate of Reaction [NO] [H₂] Exp. 1 3.2 X 10 M 1.1 X 10 M 1.3 X 10 M/s Exp. 2 6.4 X 10³ M 1.1 X 10 M 5.2 X 10 M/S Exp. 3 3.2 X 10 M 2.2 X 10 M 2.6 X 10³ M/s Find the rate law expression. Place a check mark in the box below the rate law graph that represents the rate law with respect to H₂. Rate VV Find the value of the rate constant. Attempt only if you can solve all parts with clear handwriting I'll upvote your answer What would the rate be if I initially add 6.4 X 10 M of NO and 4.4 X 10 M of H₂?

9. Nitric oxide, NO, reacts with hydrogen to give nitrous oxide, N₂O, and water. 2NO+H₂)------- NO + H₂O In a series of experiments, the following initial rates of disappearance of NO were obtained: Show work Initial Concentrations Initial Rate of Reaction [NO] [H₂] Exp. 1 3.2 X 10 M 1.1 X 10 M 1.3 X 10 M/s Exp. 2 6.4 X 10³ M 1.1 X 10 M 5.2 X 10 M/S Exp. 3 3.2 X 10 M 2.2 X 10 M 2.6 X 10³ M/s Find the rate law expression. Place a check mark in the box below the rate law graph that represents the rate law with respect to H₂. Rate VV Find the value of the rate constant. Attempt only if you can solve all parts with clear handwriting I'll upvote your answer What would the rate be if I initially add 6.4 X 10 M of NO and 4.4 X 10 M of H₂?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 30QAP

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Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
Diethylhydrazine reacts with iodine according to the following equation: Â (C2H5)2(NH)2(l)+I2(aq)(C2H5)2N2+2HI(aq)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) What is the order of the reaction with respect to diethylhydrazine, iodine, and overall? (b) Write the rate expression of the reaction. (c) Calculate k for the reaction. (d) What must [(C2H5)2] be so that the rate of the reaction is 5.00104mol/Lh when [ I2 ]=0.500M?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
For the reaction QW+X, the following data were obtained at 30 C: [Q]initial (M) 0.170 0.212 0.357 Rate(mol/L/s) 6.68103 1.04102 2.94102 (a) What is the order of the reaction with respect to [Q], and what is the rate equation? (b) What is the rate constant?
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.
In the nuclear industry, chlorine trifluoride is used to prepare uranium hexafluoride, a volatile compound of uranium used in the separation of uranium isotopes. Chlorine trifluoride is prepared by the reaction CI2(g)+3F2(g)2CIF3(g). Write the equation that relates the rate expressions for this reaction in terms of the disappearance of Cl2 and F2 and the formation of CIF3.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
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.
For the reaction AB+C, the following data were obtained at 30 C: [A] (M) 0.230 0.356 0.557 Rate (moI/L/s) 4.17104 9.99104 2.44103 (a) What is the order of the reaction with respect to [A], and what is the rate equation? (b) What is the rate constant?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?