The following data were obtained for the reaction 2C102 (aq) + 20H (ag) → Cl03 (aq) + C1O2¯ (ag) + H,0(1) A[CIO2] At where Rate (CIO,lo (mol L) I_HO) (mol/L) Initial Rate (molL s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 × 10¬1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH]* b Determine the value of the rate constant. Rate constant = 2.30x1 / L² /mol? · s © What would be the initial rate for an experiment with [C1O2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·s

The following data were obtained for the reaction 2C102 (aq) + 20H (ag) → Cl03 (aq) + C1O2¯ (ag) + H,0(1) A[CIO2] At where Rate (CIO,lo (mol L) I_HO) (mol/L) Initial Rate (molL s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 × 10¬1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH]* b Determine the value of the rate constant. Rate constant = 2.30x1 / L² /mol? · s © What would be the initial rate for an experiment with [C1O2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·s

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.42PAE: Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small...

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Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?
Nitric oxide reacts with hydrogen to release large amounts of chemiluminescence with the characteristics of the highly cytotoxic species. The following data were measured for the reaction of nitric oxide with hydrogen: Data number 1 2 3 2 NO(g) + 2 H₂(g) → N₂(g) + 2 H₂O(g) [NO] (M) 0.1 0.1 0.2 [H₂] (M) 0.1 0.2 0.1 Based on the data, (a) Determine the rate law for this reaction. (b) Calculate the rate constant. (c) Calculate the rate when [NO] = 0.050 M and [H₂] = 0.150 M Initial rate (M/S) 1.23 x 10-³ 2.46 x 10-³ 4.92 x 10-³
7) For the reaction CO(g) + 3 H2(g) = H2O(g) + CH4(g), Kc = 190 at 1000 K. If a vessel is filled with these gases such that the initial concentrations are [CO] = 0.036 M, [H2] = 0.045, [H2O] = 0.020, 7) %3D %3D %3D and [CH4] = 0.031, in which direction will a reaction occur and why? A) it is at equilibrium because Q = 190 B) toward products because Q = 4.1 C) toward reactants because Q = 0.24 D) toward products because Q = 0.38 %3D %3D %3D %3D E) toward reactants because Q = 61 %3D
Consider the following gas phase reaction at constant volume: 2CH2N2(g) −→ 2N2(g) + C2H4(g) i) Given that the initial pressure is p0 calculate the total pressure after three quarters of the CH2N2(g) has reacted. ii) Derive an equation which shows how the total pressure varies as a function of the fraction, α, of the CH2N2(g) that has reacted. iii) Sketch a graph which shows how the pressure varies as a function of α
(a) Explain the meaning of the sentence:“The velocity laws of reactions are empirical” (b) It can be determined that the velocity law of a generic reaction A +B→Pév = k[A]x[B]y. Plot on a graph the variation of [A] and [P] with time, and explain why v= d[P]/dt = -d[A]/dt. (c) Explain the meaning of the terms k, x and y, in the velocity law, presented in item b: (d) Explain what it means in practice for a velocity law to be of zero order. Plot ,A as a function of t, for the zero-order reaction A→Products. (e) Explain what elementary reactions are and how they can be classified.
Suppose the formation of tert-butanol proceeds by the following mechanism: step elementary reaction rate constant CBr(aq) (CH), С"(аg) + Br (ag) c* k 1 2 (CH3),C"(aq) + OH (aq) → (CH,),COH(aq) k2 3 3 Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for 0 k = the reverse of the two elementary reactions in the mechanism.
1a) The decomposition of ethanol at some constant temperature (above 500°C), over a copper surface, C2H5OH(g)--> CH3CHO(g) + H2(g) was studied by monitoring the total pressure with time.The following data were obtained: t (s) Ptotal (torr) 0 120 45 131 139 154 233 177 376 212 380 213 What will be the total pressure at t = 462 s? 1b) What is the rate constant (k)?(Include appropriate units.)
(a) The decomposition of a gas phase reactant, A, into gaseous products, P and Q, proceeds according to the reaction stoichiometry: A (g) P (g) + Q (g) and has been studied by measurement of the pressure increase in a constant volume system. Starting with an initial pressure of 112 torr of pure A at 713 K, the following total pressures, were measured at the times stated: Time (min) Pressure (Torr) | 136 15 30 45 60 75 155 170 181 191 (i) Give a suitable expression for the integrated rate equation by which the tabulated data can be analysed to confirm that the reaction exhibits first order kinetics. (ii) Calculate the rate constant and the half life of the reaction. (ii) If the activation energy of the reaction is given by 120 kJ mol, determine the rate constant and half life at a temperature of 1100 K.
Here is the correct statement for Qc and Kc for a certain reaction. Qc value is determined by the concentrations of reactants and products at a particular moment rather than by the temperature, but Kc value stays the same at a certain temperature regardless of the concentrations. For the following reaction at 20oC, the Qc value at a particular time is equal to 3.5 x 10‒5 3A(aq) + B(aq) ⟶ 2C(aq) + D(aq) Kc = 5.5 x 10‒5 If the reaction temperature is suddenly increased to 40oC without affecting the concentration of each component in the system, which of the following is a correct prediction about Qc and Kc at this particular time at 40oC? Q ≠ 3.5 x 10‒5, K = 5.5 x 10‒5 Q ≠ 3.5 x 10‒5, K ≠ 5.5 x 10‒5 Q = 3.5 x 10‒5, K ≠ 5.5 x 10‒5
Write down the kinetic equation for a simple reaction in a homogeneous medium 2A + B = 2C. Indicate the general and in relati on to all reactants reaction orders
The reaction between fluorine and chlorine dioxide, F2(g) + ClO2(g) → 2FClO2(g) Proceeds according to the following rate Law: r=k⋅PF2⋅PClO2 where k= 0.0489 bar-1 s-1. In an isolation experiment, the initial partial pressures are: PF2(t=0) = 0.04687 bar and PClO2(t=0) = 3.606 bar. Note: Ukeff means units of keff . You need to use a string with no spaces. For example enter gm3 as g*m^{-3} or g/m^3 . (a) Calculate the effective rate constant keff= Ukeff= (b) Compute the pressure of fluorine in bar after 55.8 s. PF2(t=55.8s)= bar (c) How long will it take for the pressure of fluorine to drop to 0.01318 bar? t = s
In a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)V½ H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.72×103 M1s1and a y-intercept of 0.667 M1. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M1s1