help on these two plz The gas phase decomposition of hydrogen peroxide at 400 °CH₂O₂(g) → H₂O(g) + ½/2O₂(g)is second order inH₂O₂ with a rate constant of 0.6501M-sIf the initial concentration ofH₂O₂ is 0.221 M, the concentration ofH₂O₂ will beM after 21.5 seconds have passed. Determine half-life, order, and k from concentration-time data.The following data were collected for the gas phase decomposition of sulfuryl chloride at 600 K.SO₂Cl₂(g) SO₂(g) + Cl₂(g)[SO₂Cl₂], M 4.43x10-3time, min 02.22x10-3 1.11x10-3186.00372.005.55x10-4558.00(a) What is the half-life for the reaction when [SO₂Cl₂] = 4.43x10-3 M?(b) What is the half-life for the reaction when [SO₂Cl₂] = 2.22x10-³ M?(c) Is the reaction first order?If so, what is the rate constant for the reaction? (If not first order leave blank).minminmin ¹

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The gas phase decomposition of hydrogen peroxide at 400 °C H₂O₂(g) → H₂O(g) + O₂(g) is second order in H₂O₂ with a rate constant of 0.650 1 M-s If the initial concentration of H₂O₂ is 0.221 M, the concentration of H₂O₂ will be M after 21.5 seconds have passed.

The gas phase decomposition of hydrogen peroxide at 400 °C H₂O₂(g) → H₂O(g) + O₂(g) is second order in H₂O₂ with a rate constant of 0.650 1 M-s If the initial concentration of H₂O₂ is 0.221 M, the concentration of H₂O₂ will be M after 21.5 seconds have passed.

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 11.48PAE: 11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol...

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11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
At 620. K butadiene dimerizes at a moderate rate. The following data were obtained in an experiment involving this reaction: t(s) [C4H6] (mol/L) 0 0.01000 1000.. 0.00629 2000. 0.00459 3000. 0.00361 a. Determine the order of the reaction in butadiene. b. In how many seconds is the dimerization 1.0% complete? c. In how many seconds is the dimerization 10.0% complete? d. What is the half-life for the reaction if the initial concentration of butadiene is 0.0200 M? e. Use the results from this problem and Exercise 45 to calculate the activation energy for the dimerization of butadiene.
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
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)?
Would the slope of a ln(k) versus 1/T plot (with temperature in kelvin) for a catalyzed reaction be more or less negative than the slope of the ln(k) versus 1/T plot for the uncatalyzed reaction? Explain. Assume both rate laws are first-order overall.
The decomposition of sulfuryl chloride, SO2Cl2, to sulfur dioxide and chlorine gases is a first-order reaction. The following kinetic data for the decomposition at a certain temperature are given below: (a) Plot the data to show that the reaction is first-order. (b) From the graph, determine k. (c) What is the half-life of the decomposition? (d) Using k from (b), find the time it takes to decrease the concentration to 0.00427 M. (e) What is the rate of decomposition [ SO2Cl2 ]=0.0153M?
11.51 Peroxyacetyl nitrate (PAN) has the chemical formula CtHjNOj and is an important lung irritant in photochemical smog. An experiment to determine the decomposition kinetics of PAN gave the data below. Determine the order of reaction and calculate the rate constant for the decomposition of PAN. Time, t (min) Partial Pressure of PAN (torr) 0.0 2.00 X 10~’ 10.0 1.61 X 10~} 20.0 1.30 X 10_J 30.0 1.04 X 10"’ 40.0 8.41 X 10-4 50.0 6.77 x 10-4 60.0 5.45 X 10-4
What is the half-life of benzene diazonium chloride decomposition at 20C? See Problem 13.100 for data.
Many biochemical reactions are catalyzed by acids. A typical mechanism consistent with the experimental results (in which HA is the acid and X is the reactant) is Step 1: Step 2: Step 3: Derive the rate law from this mechanism. Determine the order of reaction with respect to HA. Determine how doubling the concentration of HA would affect the rate of the reaction.
For a reaction involving the decomposition of a hypothetical substance Y, these data are obtained: Determine the order of the reaction. Write the rate law for the decomposition of Y. Calculate k for the experiment above.