(a)
Interpretation:
The half-lives of decomposition of
Concept Introduction:
The half-life of the particular
(b)
Interpretation:
The time taken by
Concept Introduction:
According to the integrated rate law for the first order reaction, the concentration of reactant is the exponential function of time. The two equations that represent the integrated rate law for the first order kinetics is shown below.
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CHEM PRINCIPLES LL W/ACHIEVE ONE-SEM
- 36. The gas-phase reaction H+ D2 → HD + D is the exchange of isotopes of hydrogen of atomic mass 1 (H) and 2 (D, deuterium). The following data were obtained for the rate constant k of this reaction: Temperature (K) k (L mol-1 s-1) 299 1.56 x 104 327 3.77 x 104 346 7.6 x 104 440 106 549 1.07 × 105 745 8.7 x 107arrow_forwardA second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants? The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C. Evaluate the Arrhenius parameters of the reaction. A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmº mol2 s¹. Calculate the time required for the concentration of A to change from 0.077 mol dm3 to 0.021 mol dm³.arrow_forwardAcetone is one of the most important solvents in organicchemistry, used to dissolve everything from fats and waxes toairplane glue and nail polish. At high temperatures, it decom-poses in a first-order process to methane and ketene(CH2=C=O). At 600C, the rate constant is 8.7x10^-3s⁻¹.(a) What is the half-life of the reaction?(b) How long does it take for 40.% of a sample of acetone todecompose?(c) How long does it take for 90.% of a sample of acetone todecompose?arrow_forward
- E17C.1(b) The equilibrium constant for the binding of a drug molecule to a protein was measured as 200. In a separate experiment, the rate constant for the binding process, which is second order overall, was found to be 1.5 x 10 dm mol s. What is the rate constant for the first-order dissociation of the drug molecule from the protein- drug complex?arrow_forward(a) Describe the term “integrated rate law” and briefly explain how it can be used tographically obtain the order of a reaction. (4)(b) Define the term “half-life of a substance” and briefly explain how it be used todetermine the order of the reaction and the rate constant for a first-order reaction. (4)arrow_forwardBenzoyl peroxide (C14H10O4) is widely used in acne treatments. It degrades by 1st-order kinetics and has a half-life of 9.8×103 days at 25 °C.(a) What is the rate constant for this reaction at 25 °C? (b) How many years will it take for 10% of the benzoyl peroxide to degrade?arrow_forward
- Assume that the formation of nitrogen dioxide: 2NO(g) + O2(g) 2NO2(g) is an elementary reaction. (a) Write the rate law for this reaction. (b) A sample of air at a certain temperature is contaminated with 2.0 ppm of NO by volume. Under these conditions, can the rate law be simplified? If so, write the simplified rate law. (c) Under the conditions described in part (b), the half-life of the reaction has been estimated to be 6.4 × 103 min. What would the half-life be if the initial concentration of NO were 10 ppm?arrow_forward(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.arrow_forwardThe reaction between ethyl iodide and hydroxide ion inethanol (C2H5OH) solution, C2H5(1alc) + OH- (1alc)----->C2H5OH(l) + I - (alc) , has an activation energy of86.8 kJ>mol and a frequency factor of 2.10 x 1011 M-1 s-1.(a) Predict the rate constant for the reaction at 35 °C. (b) Asolution of KOH in ethanol is made up by dissolving 0.335g KOH in ethanol to form 250.0 mL of solution. Similarly,1.453 g of C2H5I is dissolved in ethanol to form 250.0mL of solution. Equal volumes of the two solutions aremixed. Assuming the reaction is first order in each reactant,what is the initial rate at 35 °C? (c) Which reagent inthe reaction is limiting, assuming the reaction proceeds tocompletion? (d) Assuming the frequency factor and activationenergy do not change as a function of temperature,calculate the rate constant for the reaction at 50 °C.arrow_forward
- 20B.2(b) The rate constant for the first-order decomposition of a compound A in the reaction 2 A→P is krr=3.56×10−7 s−1 at 25 °C. What is the half-life of A? What will be the pressure, initially 33.0 kPa after (i) 50 s, (ii) 20 min after initiation of the reaction?arrow_forwardSome reactions proceed through a chain mechanism involving radicals, which are highly reactive species with one or more unpaired electrons. The radicals are produced in initiation steps, through either thermal or photodissociation. Reactions in which the radical centre is transferred are called propagation steps. The radicals are lost in termination steps. Consider the following chain mechanism:(1) AH → A + H·(2) A → B· + C(3) AH + B· → A + D(4) A + B· → P(a) Identify the initiation, propagation, and termination steps.(b) Use the steady-state approximation to deduce that the decompositionof AH is f irst-order in AH.arrow_forward(iv) The activation energy, Ea, and pre-exponential factor, A, for the decomposition of N2O5: N2O5→ 2 NO2 + ½ O2 are: E = 102.2 kJ mol-1 and A = 2.81 x 1013 s-1. (a) Using these data calculate the rate constant of the reaction at 300 K. (b) Assuming the reaction is first order calculate the rate of the reaction, at 300 K, when the concentration of N2O5 is 0.015 mol L-1.arrow_forward
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