Two lakes are connected to each other as shown in the figure below. Each lake has a volume of 106 m³ and an initial concentration of 10 g/m³. Lake 1 receives an inflow of 105 m³/day and a concentration of 100 g/m³. In addition to the Lake 1 outflow, Lake 2 receives an inflow of 1x105 m³/day with a concentration of 100 g/m³. The chemical undergoes first-order decay with a rate constant of 0.1 /day. (i) Calculate the steady-state concentrations (in g/m³) in the effluent from the lakes. (Include the mass balance equations in your solution.)

Two lakes are connected to each other as shown in the figure below. Each lake has a volume of 106 m³ and an initial concentration of 10 g/m³. Lake 1 receives an inflow of 105 m³/day and a concentration of 100 g/m³. In addition to the Lake 1 outflow, Lake 2 receives an inflow of 1x105 m³/day with a concentration of 100 g/m³. The chemical undergoes first-order decay with a rate constant of 0.1 /day. (i) Calculate the steady-state concentrations (in g/m³) in the effluent from the lakes. (Include the mass balance equations in your solution.)

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...

See similar textbooks

Similar questions

Americium-241 is used in smoke detectors. It has a first order rate constant for radioactive decay of k= 1.6 x 10¹ yr. By contrast, phophorus-32, which is used for the analysis of metabolic pathways, has a rate constant for radioactive decay of k = 0.050 day-1 ▾ How much of a 2.50 mg sample of americium remains after 3 half-lives? Express your answer in milligrams to two significant figures. ▾ TTL = ▾ Part E Submit TIL = How much of a 1.51 mg sample of phophorus remains after 3 half-lives? Express your answer in milligrams to two significant figures. Templates Symbols Undo redo Peser keyboard shortcuts help Templates Symbols Undo redo es keyboard shortcuts Help n Submit Part F TTL= Request Answer How much of a 1.00 mg sample of americium remains after 4 days? Express your answer in milligrams to two significant figures. Part G Submit Request Answer Templates Symbols Undo redo Teset keyboard shortcuts Help n ** Previous Answers Request Answer How much of a 1.35 mg sample of phophorus…
1. The radioactive isotope 32P has a half-life of 14.3 days. If a sample contains 0.884 g of 32P, what mass of the isotope will remain after 22 days? 2. Use the integrated first-order rate law to calculate the mass of 32P remaining after 22 days.
0.1 M of a material has a decomposition rate constant (k) of 2.46×105 M-1 s-1. What equation would you use to calculate the half-life of decomposition?
Geologists can estimate the age of rocks by their uranium-238 content. The decay of U-238 is first-order with a half-life of 4.5 billion years (4.5×109 yrs). A rock contains 49.4% of the initial amount of U-238 from when it was formed. How old is the rock? Please explain full math and formulas used
23. A reaction proceeds by a series of elementary steps as shown below. The activation energy and heat of reaction are shown for each step. Step No. Elementary Step Activation Energy Enthalpy of Reaction 1 АВ — А + %2B, 12 kJ 35 kJ 2 C + B2 → CB, 2.5 kJ -29 kJ 3 АС — А + С 7.5 kJ 21 kJ a) What is the overall equation for this reaction? Show your work. b) What is the heat of reaction for the overall equation? Show your work. c) Which step is the rate determining step and why? d) Using the space provided below, draw and label a potential energy diagram to represent the overall equation in (a). I
A tree killed by being buried under volcanic ash was found to have a ratio of carbon-14 atoms to carbon-12 atoms of 5.7 × 10-14. The rate constant of the C-14 → C-12 decay is k = 1.21 x 10-4 yr-1 and the ratio of carbon-14 to carbon-12 is 1.2 x 10-12 in a contemporary sample. How long ago did the eruption occur? t = yr
Radioactive iodine-131, used in radiotherapy to treat cancer, has a first-order half life of 8.0 days. A sample of iodine-131 is injected directly into a tumor. How long will it take for 15% of the iodine-131 to remain in the tumor? First order: Ln{[A]0/[A]} = kt Half life = 0.693/k
Iodine-131 is a radioactive isotope that is used to diagnose and treat some forms of thyroid cancer. Iodine-131 decays to xenon-131, according to the equation below. iodine-131→xenon-131+electron The decay is first order with a rate constant of 0.138 d−1. All radioactive decay is first order. How many days will it take for 67.0% of the iodine-131 in a 0.400 M solution of this substance to decay to xenon-131? 8.03 days 2.90 days 4.86 days 0.0239 day
Two gases X and Y are found in the atmosphere in only trace amounts because they decompose quickly. When exposed to ultraviolet light the half-life of X is 15. min, while that of Y is 2.50 h. Suppose an atmospheric scientist studying these decompositions fills a transparent 10.0 L flask with X and Y and exposes the flask to UV light. Initially, the partial pressure of X is 5.0 times greater than the partial pressure of Y. As both gases decompose, will the partial pressure of X ever fall below the partial pressure of Y? If you said yes, calculate the time it takes the partial pressure of X to fall below the partial pressure of Y. Round your answer to 2 significant digits. O yes O no min 0 0 14
In a patient, the fraction of radioactive iodine 131I (Iodine) remaining after 32 days was found to be 1/16. Using this information and your knowledge of the rate law, show that the half-life of radioactive iodine is 8.0 days.
Consider the radioisotope ⁴¹Ca (half life = 1.03 × 10⁵ years). What is the first-order rate constant for ⁴¹Ca?
Fallout from nuclear weapons tests in the atmosphere is mainly 90Sr and 137Cs , which have 28.6- and 32.2-y half-lives, respectively. Atmospheric tests were terminated in most countries in 1963, although China only did so in 1980. It has been found that environmental activities of these two isotopes are decreasing faster than their half-lives. Why might this be?