Answer Q13, 14, 15 What is the overal order of the reaction?11.A) 0C) 3In a study of the rate of reactionX(aq) + Y(aq) > Z(aq), solutioncontaining different initial concentrations ofX and Y were allowed to react. The time takenfor concentration of Z to reach a certain levelwas measured. The results are shown below7.B) 1D) 2The graph below shows the variation of enerovagainst reaction path for an exathermic reactionTimeInitial [X]mollInitial [Y]mollEnergytaken s0.10.11610.10.280Reactant540.10.20.30.1390.30.118PodutThe right expression for the rate of reaction interms of concentration of X and Y iaA) Rate = K[X][Y]B) Rate = K[X] [YPC) Rate = K [XF MD) Rate = K (X] IYPReaction path12. Which of the letters A to C represents theactivation energy for the reaction?Questions 13 and 14Z, the rate isFor the reaction X + 2Yquadrupled when (X] is doubled and [Y] is keptconstant. It is doubled when [Y] is doubled and[XI in kept constant.Questions a and 9The preparation of ethylbromide fromelhanol is thought to proceed by thefollowing mechanism8.13. The right rate expression for the reaction isA) Rate = K[Y]XB) Rate = K [YP [X]C) Rate = K[YTIXID) Rate = K[XTY) CH CH-OH-H'Fast>CH,CH,-OH step Iii) CH,-CH-OH +Br S CH,-CH-OH step Ii) CH,-CH,-OH: CH,CH,Br +H,O; step II14. What will be the effect on the rate of thereaction when [X] is halved while [Y] in keptconstant?BrWhich step(s) is the rate determining step?A) Steps I and IIC) Steps II and IIA) Rate of reaction is halvedB) Rate of reaction is multiplied by a quarterC) Rate of reaction is squaredD) Rate of reaction is quadrupled.B) Steps Il onlyD) Step I only9.State the order of the reactionA) 2C) 0B) 1D) none of the above.15. The table below gives some data concerninga reaction belween two compounds A and B.Questions 10 and 11Concentration ofRate ofThe rate of the reactionA and B (moldm)ReactionCH Br + OHdirectly proportional to the concentration ofbromo methane and hydroxyl ln.-> CH OH + Br isB121536102410. An expression for the rate of the reaction is;A) Rate = K (CH, Br (OH]B) Rate = K [CH Br]" [OH]C) Rate = K [CH,Br [OH)D) Rate = K [CH Br [OH]The partial order of the reaction with respect tocompound A isA) 3C) 2B) 1D) 0160

Here I have answered all the question using rate law

Questions 13 and 14 For the reaction X + 2Y Z, the rate is quadrupled when [X] is doubled and [Y] is kept constant. It is doubled when [Y] is doubled and IX] in kept constant. 13. The right rate expression for the reaction is A) Rate = K [Y] [X] B) Rate = K [YP [X] C) Rate = K[YFIXI D) Rate = K[XFIY] 14. What will be the effect on the rate of the reaction when [X] is halved while [Y] in kept constant? A) Rate of reaction is halved B) Rate of reaction is multiplied by a quarter C) Rate of reaction is squared D) Rate of reaction is quadrupled. 15. The table below gives some data concerming a reaction belween two compounds A and B. Concentration of Rate of A and B (moldm) Reaction 12 15 36 10 24 The partial order of the reaction with respect to compound A is A) 3 C) 2 B) 1 D) 0 A5

Questions 13 and 14 For the reaction X + 2Y Z, the rate is quadrupled when [X] is doubled and [Y] is kept constant. It is doubled when [Y] is doubled and IX] in kept constant. 13. The right rate expression for the reaction is A) Rate = K [Y] [X] B) Rate = K [YP [X] C) Rate = K[YFIXI D) Rate = K[XFIY] 14. What will be the effect on the rate of the reaction when [X] is halved while [Y] in kept constant? A) Rate of reaction is halved B) Rate of reaction is multiplied by a quarter C) Rate of reaction is squared D) Rate of reaction is quadrupled. 15. The table below gives some data concerming a reaction belween two compounds A and B. Concentration of Rate of A and B (moldm) Reaction 12 15 36 10 24 The partial order of the reaction with respect to compound A is A) 3 C) 2 B) 1 D) 0 A5

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 13.24QE

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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?
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.
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.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?
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?
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.
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?