1) A reagent used in organic synthesis, decomposes in acidic solution by following a first-order kinetic, producing B and CO2(g). A(aq) → B(aq) + CO2(g) If the half-life of this decomposition reaction is 143.5 min, (a) What is the time required for the 65% decomposition of A(aq)? (b) How many liters of CO2(g), measured at 24.5 °C and 747 mmHg, are produced when 10.0 g sample decomposes for 575 min? (A = 102.09 g/mol; R=0.082 L atm/mol K). %3D

1) A reagent used in organic synthesis, decomposes in acidic solution by following a first-order kinetic, producing B and CO2(g). A(aq) → B(aq) + CO2(g) If the half-life of this decomposition reaction is 143.5 min, (a) What is the time required for the 65% decomposition of A(aq)? (b) How many liters of CO2(g), measured at 24.5 °C and 747 mmHg, are produced when 10.0 g sample decomposes for 575 min? (A = 102.09 g/mol; R=0.082 L atm/mol K). %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
Be sure to answer all parts. The reaction 2A →B is second order with a rate constant of 51.0/M· min at 24°C. (a) Starting with [A]0 = 8.90 ×10−3 M, how long will it take for [A]t = 3.40 ×10−3 M? (b) Calculate the half-life of the reaction.
A decomposition reaction has a rate constant of 0.0012 yr⁻¹.(a) What is the half-life of the reaction? (b) How long does ittake for [reactant] to reach 12.5% of its original value?
The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2 are reddish-brown. 2NOBr(g) →2NO(g) + Br2(g) Use the data below to make the following determinations: (a) the average rate of decomposition of NOBr over the entire experiment. (b) the average rate of decomposition of NOBr between 2.00 and 4.00 seconds. Time (s) [NOBr] (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 The rates of decomposition of NOBr are (a) mol L−1 s−1 (b) mol L−1 s−1
4) The decomposition of phosphorus pentachloride (PCIS) into phosphorus trichloride (PCI3) and chlorine gas (Cl2) is a first order process with a rate constant of 0.0842 s at a certain temperature. If 40.4 s after the reaction begins, the concentration of PCIs is 0.0203 M, what was the initial concentration of PCI3? (A) 6.76 x 104 M (B) 0.609 M (C) 3.42 M (D) (E) 0.495 M ES 0.820 Mt (D)
Be sure to answer all parts. The reaction 2A → B is second order in A with a rate constant of 33.5 M−1 · s−1 at 25 ° C. (a) Starting with [A]0 = 0.00801 M, how long will it take for the concentration of A to drop to 0.00180 M? s (b) Calculate the half-life of the reaction for [A]0 = 0.00801 M. s (c) Calculate the half-life of the reaction for [A]0 = 0.00289 M.
In the first-order decomposition of dinitrogen pentoxide at 335 K,N2O5(g) → 2 NO2(g) + ½ O2(g)if we start with a 2.50-g sample of N2O5 at 335 K and have 1.50 g remaining after 109 s, (a) What is the value of the rate constant k? (b) What is the half-life of the reaction? (c) What mass of N2O5 will remain after 5.0 min?
The first order rate constant for the decomposition of N2Os to NO2 and O2 at 70 °C is 6.82 x 10-3 s. Suppose we start with 0.300 mol of N,O5(g) in a 0.5 dm container. 5. (a) How many moles of N2O5 will remain after 1.5 minutes? (b) How many minutes will it take for the concentration of N2O5 to decrease by 0.4 M? (c) What is the half-life of N2O5 at 70 °C? (d) How long will it take for [N2O5] to decrease to 20 % of its original value?
6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?
2 the first-order decomposition of dinitrogen pentoxide at 335 K, N2O5(g) → 2 NO2(g) + ½ O2(g) if we start with a 2.50-g sample of N2O5 at 335 K and have 1.50 g remaining after 109 s, (a) What is the value of the rate constant k? Select one: a. k = 2.83×10–3 s–1 b. k = 8.69×10–3 s–1 c. k = 1.69×10–3 s–1 d. k = 4.69×10–3 s–1
The thermal decomposition of phosphine into phosphorus and hydrogen is a first order reaction with a half-life of 35.0 s at 680 °C. 4 PH3 (g) → P4 (g) + 6 H2 (g) a) Write the rate law for this reaction. b) How much time (in minutes) is required for 97% of a phosphine sample to decompose at 680 °C? c) If the activation barrier is 3.05 x 105 J/mol, what is the half-life for this reaction at 710 °C?
(a) The decomposition of A into products has a value of K as 4.5 × 103 s-1 at 10°C and energy of activation 60 kj mol-1. At what temperature would K be 1.5 × 104 s-1?(b) (i) If half life period of a first order reaction is x and 3/4,th life period of the same reaction is y, how are x and y related to each other?(ii) In some cases it is found that a large number of colliding molecules have energy more than threshold energy, yet the reaction is slow. Why?