Consider the reaction PO + DONG → PODONG, determine the reaction order for each component and the rate constant. The reaction rates of various PODONG formations are given below. Runs [PO], M [DONG], M Rate, x 104 M/s 1 0.40 1.20 1.97 2 0.80 1.20 7.89 3 0.40 0.40 0.073 4 1.20 0.80 5.23 What is the rate law of the reaction?

Consider the reaction PO + DONG → PODONG, determine the reaction order for each component and the rate constant. The reaction rates of various PODONG formations are given below. Runs [PO], M [DONG], M Rate, x 104 M/s 1 0.40 1.20 1.97 2 0.80 1.20 7.89 3 0.40 0.40 0.073 4 1.20 0.80 5.23 What is the rate law of the reaction?

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

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

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Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
First order: [A]o In———- = kt [A]t t1/2= .693/k
Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecules'. Convert 3.5 x 1027 cm3 molecule1 s to L mol-1 sl. Round vour answer to 2 decimal nlaces.
[References) Use the References to access important values if needed for this question. In a study of the gas phase decomposition of dimethyl ether at 500 °C CH;OCH;(g)- →CH4(g) + H2(g) + CO(g) the concentration of CH,OCH, was followed as a function of time. It was found that a graph of In[CH,OCH] versus time in seconds gave a straight line with a slope of -6.28x10s and a y-intercept of -3.50 Based on this plot, the reaction i Đ order in CH,OCH, and the rate constant for the reaction is zero first second Submit Answer Try Another Version 2 item attempts remaining (Previous 12 étv ll MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ #3 $ & * 4 6. 7 8 W E R Y { S G J K く C V ...- ~の * 00 ラエ B
I#12 please. C would be The equation for a second order with 1/A. woykd not the answe mr for A v T be reverse and answet B . This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl
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4) The rate of the following rxn depends only on NO₂: NO₂ + CO NO + CO₂. The following data was collected from a kinetics experiment: Time (s) 0 1200. 3000. 4500. 9000. 18000. [NO₂] (mol/L) 0.500 0.444 0.381 0.340 0.250 -0.174 1 I a. Order with respect to NO₂: the best R2 value in order to find the rate of the reaction) (Ans: 2nd order-r' value of 0.999) b. Rate law for this reaction: (Hint: [NO₂]. Ln[NO₂] and 1/[NO₂] and find (Ans: rate= K[NO₂] ²) c. [NO₂] at 2.7 x 104 s after the start of the rxn: 2nd order reaction rate law) (Hint: use the integrated
IV. Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of cm3 molecule-1 s-1. Convert 3.5 x 1027 cm3 molecule-1 s-1 to L mol-1 s-1. Round your answer to 2 decimal places
Q4. lodide ions are oxidised to iodine by hydrogen peroxide in acidic conditions. H₂O₂(aq) + 2H+(aq) + 21-(aq) → 1₂(aq) + 2H₂O(1) The rate equation for this reaction can be written as rate = k [H₂O₂] [1] [H*]c In an experiment to determine the order with respect to H*(aq), a reaction mixture is made containing H*(aq) with a concentration of 0.500 mol dm-³ A large excess of both H₂O2 and 1 is used in this reaction mixture so that the rate equation can be simplified to rate = k₁ [H*]c (a) Explain why the use of a large excess of H₂O2 and I means that the rate of reaction at a fixed temperature depends only on the concentration of H+(aq). (b) Samples of the reaction mixture are removed at timed intervals and titrated with alkali to determine the concentration of H*(aq). State and explain what must be done to each sample before it is titrated with alkali.
NH4+ {aq) + NO2(aq) -> N2(g) +2H2O{l} Data Initial [NH4+] Initial [NO2-] rate 1 0.0100 0.200 5.4 x10-7 2 0.0200 0.200 10.8x10-7 3 0.0400 0.200 21.5x10-7 4 0.200 0.0202 10.8x10-7 5 0.200 0.0404 21.6x10-7 6 0.200 0.0808 43.3x10-7 Find x,y,k