O KINETICS AND EQUILIBRIUMUsing a rate lawThe rate of a certain reaction is given by the following rate law:- K[H,[NH,]rate = kUse this information to answer the questions below.What is the reaction order in H,?What is the reaction order in NH3?What is overall reaction order?At a certain concentration of H, and NH, the initial rate ofreaction is 15.0 M/ s. What would the initial rate of thereaction be if the concentration of H, were halved? RoundMyour answer to 3 significant digits.The rate of the reaction is measured to be 0.780 M / s when[H2] = 0.31M and [NH-] = 0.52 M. Calculate the value of thek =rate constant. Round your answer to 2 significant digits.ExplanationCheck2021 M

Answered: Image /qna-images/answer/18f13a6a-8cec-462b-b019-2f654657cd51.jpg

The rate of a certain reaction is given by the following rate law: =<[H,]°[NH,] %3D Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in NH;? What is overall reaction order? At a certain concentration of H, and NH3, the initial rate of reaction is 15.0 M/ s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 0.780 M/s when -2 -1 [H2] = 0.31 M and [NH3] = 0.52 M. Calculate the value of the k =M rate constant. Round your answer to 2 significant digits.

The rate of a certain reaction is given by the following rate law: =<[H,]°[NH,] %3D Use this information to answer the questions below. What is the reaction order in H2? What is the reaction order in NH;? What is overall reaction order? At a certain concentration of H, and NH3, the initial rate of reaction is 15.0 M/ s. What would the initial rate of the reaction be if the concentration of H2 were halved? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 0.780 M/s when -2 -1 [H2] = 0.31 M and [NH3] = 0.52 M. Calculate the value of the k =M rate constant. Round your answer to 2 significant digits.

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 28QAP: Diethylhydrazine reacts with iodine according to the following equation: Â...

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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.
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 rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion present. The rate of decomposition was measured at constant temperature and pressure for various concentrations of H2O2and of KI. The data appear below. Determine the order of reaction for each substance, write the rate law, and evaluate the rate constant. Rate [H2OJ [Kll (mL min-’) (mol L ’) (mol L ’) 0.090 0.15 0.033 0.178 0.30 0.033 0.184 0.15 0.066
Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure shows the increase in nitrosyl chloride concentration under appropriate experimental conditions. The concentration of nitrosyl chloride actually starts at zero, although this fact may be difficult to see in the figure. (a) Write an expression for the rate of reaction in terms of a changing concentration. (b) Calculate the average rate of reaction between 40 and 120 seconds. (c) Calculate the instantaneous rate of reaction after 80 seconds. (d) Calculate the instantaneous rate of consumption of chlorine 60 seconds after the start of the reaction.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
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?
A proposed mechanism for a reaction is C4H9BrC4H9++BrSlowC4H9++H2OC4H9OH2+FastC4H9OH2++H2OC4H9OH+H3O+Fast Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction? What are the intermediates in the proposed mechanism?
For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min at 728C. (a) What is the activation energy of the reaction? (b) What is k at 485C? (c) At what temperature is k, the rate constant, equal to 11.6 L/mol min?
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.