Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2-(aq)-> N2(g) + 2H2O(1) Rate data for this reaction, measured at a certain temperature, are shown in the attached table. Use your rate law, and the rate and concentrations for any of the experiments, to calculate the rate constant (k) for the reaction in /Ms. Type your response Expt. [NH4+] (M) [NO₂ ] (M) Rate (M s-1) 1 0.150 0.220 7.00 x 10-6 2 0.600 0.220 2.80 x 10-5 3 0.600 0.110 1.40 x 10-5

Ammonium ion reacts slowly with nitrite ion: NH4+ (aq) + NO2-(aq)-> N2(g) + 2H2O(1) Rate data for this reaction, measured at a certain temperature, are shown in the attached table. Use your rate law, and the rate and concentrations for any of the experiments, to calculate the rate constant (k) for the reaction in /Ms. Type your response Expt. [NH4+] (M) [NO₂ ] (M) Rate (M s-1) 1 0.150 0.220 7.00 x 10-6 2 0.600 0.220 2.80 x 10-5 3 0.600 0.110 1.40 x 10-5

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 33QRT: For the reaction of phenyl acetate with water the concentration as a function of time was given in...

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The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2: Step 1: Slow NO2(g) + NO2(g) NO(g) + NO3(g) Step 2: Fast NO3(g) + CO(g) NO2(g) + CO2(g) (a) Show that the elementary steps add up to give the overall, stoichiometric equation. (b) What is the molecularity of each step? (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? (d) Identify any intermediates in tins reaction.
One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
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For the reaction of phenyl acetate with water the concentration as a function of time was given in Question 11. Assume that the concentration of water does not change during the reaction. Analyze the data from Question 11 to determine (a) the rate law. (b) the order of the reaction with respect to phenyl acetate. (c) the rate constant. (d) the rate of reaction when the concentration of phenyl acetate is 0.10 mol/L (assuming that the concentration of water is the same as in the experiments in the table in Question 11).
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?