28.9 g per day of a certain industrial waste chemical P arrives at a treatment plant settling pond with a volume of 1000. m³. P is destroyed by sunlight, and once in the pond it has a half-life of 33. h. Calculate the equilibrium concentration of P in the pond. Round your answer to 2 significant digits. B00 g 0- m X S

28.9 g per day of a certain industrial waste chemical P arrives at a treatment plant settling pond with a volume of 1000. m³. P is destroyed by sunlight, and once in the pond it has a half-life of 33. h. Calculate the equilibrium concentration of P in the pond. Round your answer to 2 significant digits. B00 g 0- m X S

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 99QAP: The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for...

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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.
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for the forward reaction at 700C of 138 L/moI s and an activation energy of 165 kJ/moI. (a) Calculate the activation energy of the reverse reaction given that H f for HI is 26.48 kJ/moI and H f for I2(g) is 62.44 kJ/mol. (b) Calculate the rate constant for the reverse reaction at 700C. (Assume A in the equation k=AeE a /RT is the same for both forward and reverse reactions.) (c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
Substances that poison a catalyst pose a major concern for many engineering designs, including those for catalytic converters. One design option is to add materials that react with potential poisons before they reach the catalyst. Among the commonly encountered catalyst poisons are silicon and phosphorus, which typically form phosphate or silicate ions in the oxidizing environment of an engine. Group 2 elements are added to the catalyst to react with these contaminants before they reach the working portion of the catalytic converter. If estimates show that a catalytic converter will be exposed to 625 g of silicon during its lifetime, what mass of beryllium would need to be included in the design?
The rate constant for the radioactive decay of 14C is 1.21104 year-1. The products of the decay are nitrogen atoms and electrons (beta particles): C614N714+e rate =k[C614] What is the instantaneous rate of production of N atoms in a sample with a carbon-14 content of 6.5109M?
You probably know that on exposure to air silver tarnishes and iron rusts; but gold, stainless steel, and chromium do not change. Explain these facts, using the concept of stability.
Consider the following reaction: CH3X+YCH3Y+X At 25C, the following two experiments were run, yielding the following data: Experiment 1: [Y]0 = 3.0 M [CH3X] (mol/L) Time(h) 7.08 103 1.0 4.52 103 1.5 2.23 103 2.3 4.76 104 4.0 8.44 l05 5.7 2.75 l05 7.0 Experiment 2: [Y]0 = 4.5 M [CH3X] (mol/L) Time(h) 4.50 103 0 1.70 103 1.0 4.19 104 2.5 1.11 104 4.0 2.81 l05 5.5 Experiments also were run at 85C. The value of the rate constant at 85C was found to be 7.88 108 (with the time in units of hours), where [CH3X]0 = 1.0 102 M and [Y]0 = 3.0 M. a. Determine the rate law and the value of k for this reaction at 25C. b. Determine the half-life at 85C. c. Determine Ea for the reaction. d. Given that the C8X bond energy is known to be about 325 kJ/mol, suggest a mechanism that explains the results in parts a and c.
Consider this scenario and answer the following questions: Chlorine atoms resulting from decomposition of chloro?uoromethanes, such as CCI2F2, catalyze the decomposition of ozone in the atmosphere. One simplified mechanism for the decomposition is: O3sunlightO2+O O3+CIO2+CIO CIO+OCI+O2 (a) Explain why chlorine atoms are catalysts in the gas-phase transformation: 2O33O2 (b) Nitric oxide is also involved in the decomposition of ozone by the mechanism: O3sunlightO2+O O3+NONO2+O2 NO2+ONO+O2 Is NO a catalyst for the decomposition? Explain your answer.
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Scientists can determine the age of ancient objects by the method of radiocarbon dating. The bombardment of the upper atmosphere by cosmic rays converts nitrogen to a radioactive isotope of carbon, 14C, with a half-life of about 5,730 years. Vegetation absorbs carbon dioxide through the atmosphere, and animal life assimilates 14C through food chains. When a plant or animal dies, it stops replacing its carbon, and the amount of 14C present begins to decrease through radioactive decay. Therefore, the level of radioactivity must also decay exponentially. a) Dinosaur fossils are too old to be reliably dated using carbon-14. Suppose we had a 67 million year old dinosaur fossil. What percent of the living dinosaur's 14C would be remaining today? (Round your answer to five decimal places.) b) Suppose the minimum detectable amount is 0.7%. What is the maximum age (in years) of a fossil that we could date using 14C? (Round your answer to the nearest year.)