(a)
Interpretation:
The order of the reaction should be determined using given data.
Concept introduction:
The rate law/rate equation for a
(b)
Interpretation:
The rate constant of reaction should be determined using given data.
Concept introduction:
For second order reaction:
Where, k is rate constant, t is time, [A]t is concentration of A at time t and [A]o is the concentration of A at initial time that is at t = 0.
(c)
Interpretation:
Time at which [C4H6] is equal to 0.00423 M should be determined.
Concept introduction:
In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.
(d)
Interpretation:
Time at which [C4H6] is equal to 0.005 M should be determined.
Concept introduction:
In a second order reaction, the rate is linearly proportional to the concentration squared of the reactant.
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General Chemistry: Principles and Modern Applications (11th Edition)
- The composition of a liquid phase reaction 2 A → B was followed spectrophotometrically with the following results:t/min 0 10 20 30 40 ∞[B]/(mol dm-3 ) 0 0.372 0.426 0.448 0.460 0.500Determine the order of the reaction and its rate constantarrow_forwardThe first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.arrow_forwardSecond-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecule1 s1. Convert 3.5 x 1027 cm3 molecule 1 s-1 to L mol-1 s1. 1 Round your answer to 2 decimal places.arrow_forward
- Show that the initial rate law predicted by the reaction mechanism 6-12a-c, with the first step rate-limiting, is rate = 2k,[Cl,]. Assume that the Cl - produced in step (3) can be neglected initially.arrow_forwardII.2- Saponification of ethyl ethanoate, a second-order kinetic? Data: R = 8.314 J mol·l K-' The kinetic study of the saponification reaction of ethyl ethanoate by caustic soda (sodium hydroxide NaOH): CH;COOCH2CH3 + OH- → CH3CO2¯ + CH3CH2OH was achieved at 298 K for initial concentrations a in ester and hydroxide that are identical. Experimental results, for different values of a, are reported in the following table: a (mol L·l) 0.1 7.5 × 10-2 5 × 10-2 4 x 10-2 t1/2 (s) 6.66 ×105 8.89 ×105 1.33 ×106 1.66 ×106 Using a value of Ea = 61.5 kJ mol·l for the activation energy of this reaction in the considered temperature domain, calculate the value of the time that is necessary for the concentration in ethanol CH3CH2OH to reach 5 × 10-³ mol L-' at T = 308 K.arrow_forwardThe protein catalase catalyzes the reaction 2H,0,(aq) – 2 H,0O(0) + 0,(g) and has a Michaelis–Menten constant of KM = 25 mM and a turnover number of 4.0 × 107 s-1. The total enzyme concentration is 0.016 µM and the initial substrate concentration is 6.58 µM. Catalase has a single active site. Calculate the value of Rmax (often written as Vmax ) for this enzyme. Rmax mM-s- Calculate the initial rate, R (often written as Vo), of this reaction. R = mM-s-arrow_forward
- Derive an expression for the time dependence of the degree of polymerization for the stepwise polymerization of a hydroxyacid HO−R−COOH for which the rate law is d[A]/dt = −kr[A]2[OH], where A denotes the carboxylic acid group.arrow_forwardThe mechanism for the reaction described by nust. A common d(a stronger whch ont of ice prhct NO,(g) + CO(g) → CO,(g) + NO(g) coor on be c is suggested to be (1) 2NO,(g) –→ NO,(g) + NO(g) k1 -> k2 (2) NO,(g) + CO(g) → NO,(g) + CO,(g) d[CO2] k[NO2]? %3D The experimental rate law for the production of [CO2] = k1 [NO2J² or dt d[NO3] 0 ), is this a valid mechanism? i.e show Assuming that [NO3] is governed by a steady state ( dt that using elementary reactions 1 and 2, the experimental rate law can found. (Hint write out all the ways d[NO3] = ? d[C02] = ? ) %3| and %3D dt that [NO3] and [CO2] are created and destroyed, dt owing clecre cel at 25 C NiC C)Cu a062 0.62 V 0.00 V 4. 460 Varrow_forwardCalculate the rate of the reaction (k) of ∙OH (105 molecules cm-3) with atmospheric CO (150 ppb) at 28°C, given that the rate constant for the process is 5 × 10-13 exp (-300 / temp) molecule-1 cm3 s-1.arrow_forward
- (b) The reaction between H2O2 and lodide; H,0, + 21 + 2H*→ 2H,0 + 12 Proceeds by two parallel mechanism and led to a rate laws, k, [H,0][I] and = k, [H,0][][#*] %3D dt dt The change in observed rate constants with ionic strength for both the mechanisms is given in the following table. k (M's) 0.69 k2 (M's') Sr. no. Ionic strength (1) 19.0 0.00 0.0207 0.66 15.0 3 0.0525 0.67 12.0 4 0.0925 0.68 11.3 0.69 0.1575 0.2025 9.7 0.71 9.2 With the help of this data and corresponding plots, comment on which mechanism between these two would follow Primary salt effect more prominently. rhich tyne of complex mechanism T-jumparrow_forward5 Why is it important to be able to calculate steady-state variables such as temperature, pressure, concentration?arrow_forwardGiven the transition state diagram(s) below, identify the mechanism(s) of catalysis. Mg2+ Mg2+ H OH H-C-H HOH H H - (M₂C)N= H H-C-H HO -H H- HO -H OH-O -O-H- H-N(CH₂) CH₂OH H H₂C H H LN (CH2) H OH HOH:N (0³H)² CH₂OH H₂C tarrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,