Water Quality lab report

I need help with #4. I think all the previous answers are correct, I'm just not sure how to do #4, both a. and b.

Resarch project ( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering Ocean Acidification add lots of pictures and details

Lab 6: Chemical Reactions Post-Lab Questions Station V: Heating Cu with Atmospheric O₂ Chemical equation: Complete ionic equation: Net ionic equation: General reaction type: Station VI: Reacting CuSO4 Solution with Steel Wool (Fe)

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000 000 ← OCT 18 © Macmillan Learning Chapter 7 HW - General, Organic, and Biological Chemistry for He Solution Resources Hint Penalized Place the following events of breathing in order, starting with inhalation. Drag the correct phrase to each target. Two of the phrases are incorrect and will not be used. The diaphragm lowers during inhalation. ↓ Answer Bank ↓ ↓ The volume of the lungs decreases and air pressure in the lungs increases. The volume of the lungs increases and air pressure in the lungs decreases. Air enters the lungs. Air is forced out of the lungs. The diaphragm rises during exhalation. The volume of the lungs increases and air pressure in the lungs increases. The volume of the lungs decreases and air pressure in the lungs decreases. MacBook Pro ☑ 114 A Σ

DDT (molar mass % 354.49 g/mol) was a widely used insecticide that was banned from use in the United States in 1973. This ban was brought about due to the persistence of DDT in many different ecosystems, leading to high accumulations of the substance in many birds of prey. The insecticide was shown to cause a thinning of egg shells, pushing many birds toward extinction. If a 20-L drum of DDT was spilled into a pond, resulting in a DDT concentration of 8.75 X 10-5 M, how long would it take for the levels of DDT to reach a concentration of 1.41 X 10-7 M (a level that is generally assumed safe in mammals)? Assume the decomposition of DDT is a frst-order process with a half-life of 56.0 days.

Hi, please I really need these two questions to be answered please help me with this I really don't know what to do, I'm so much struggling, please please kindly help me.

At 40^0c, H202 (aq) will decompose according to the foll. reaction: 2 H202 (aq) ----2H20(l) +02 (g) The foll. data were collected for the concentration of h202 at various times. Time.                    [H202] (mol/L) 0.                           1.600 3.10*10^4              0.592 6.20*10^4.            0.219 (a) Calculate the average rate of decomposition in H202 between0 and 3.10 * 10^4 s. use this rate to calculate the average rate of production 02 (g) over the same time period. (b) What are these rates for the time period 3.10*10^4 s. to 6.20 *10^4 s.? Rate of H202 decomposition Rate of O2 Production

Consider the balanced chemical equation. Submit Request Answer H2O2 (aq) + 31 (aq) + 2H+(aq) → I3 (aq) + 2H2O(1) In the first 12.0 s of the reaction, the concentration of I drops from 1.000 M to 0.773 M . Part B You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Predict the rate of change in the concentration of I3 (AI3]/At). Express the rate to three significant figures and include the appropriate units. A[l; ]/At = Value Units

Based on your ICE table (Part 1) and the definition of Ka, set up the expression for Ka in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 1.8 × 10-5 [500.0] [0.200] RESET [5.00] [1.0 × 10-9] [1.0 × 10-9] [1.8 × 10-5] [x + 5.00] [x + 1.0 × 10] [x-1.0 x 10 x + 1.0 × 10-] [x-1.0 × 10-] [x+1.8 × 10] [x-1.8 × 10%] [0] [x-5.00] < PREV 1 2 3 Based on your ICE table (Part 1) and the equilibrium expression, Ka (Part 2), determine the original mass of solid CH3COONa added to create this buffer solution. MNACH3COO g 0 0.360 30 21 43 11 15 36 x 10' 59 x 105 43 x 105 RESET 59 50

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tion 1 of 19 The decomposition of N, O, can be described by the equation 2 N,0, (soln) 4 NO, (soln) + O,(g) Consider the data in the table for the reaction at 45 °C in carbon tetrachloride solution. t(s) [N,O;] (M) 2.194 175 1.965 506 1.596 795 1.331 Given the data, calculate the average rate of reaction for each successive time interval. Question Source: MRG - General Chemistry | Pub | privacy policy |help about us terms of use contact us careers N W prime video

Lactase is an enzyme that breaks down the sugar lactose which is commonly found in dairy products. Some people develop lactose intolerance as they grow older and the amount of lactase enzyme in their gut diminishes. Since the enzyme is commonly found in the gut of humans it can withstand a pH that is very acidic, ranging from a pH of 2-7. A student decided to do an experiment to determine how the pH of a solution affects lactase enzyme activity. Lactase works by breaking lactose into its two component sugars of glucose and galactose.   To conduct the experiment the student prepared a solution of lactose and placed it into 5 different test tubes. A pH buffer solution was then added to each test tube with a pH of 2.0 in the first tube, 4.0 in the second, 6.0 in the third, 8.0 in the fourth, and a 10 pH in the fifth. Next, the enzyme lactase was added in equal amounts to each test tube and allowed to sit for ten minutes white the enzyme reacted with the lactose. At the end of the ten…

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Resarch project( le chatelier's principle ) Be sure to explain the Chemistry involved in this reaction or process and how this reaction relates to Technology, Society and/or the Environment. Some examples include: Haber-Bosch Process Blood Buffering add lots of pictures and details

Initial Concentrations: Exp. 1 Exp. 2 Exp. 3 [NO] 0.210 M 0.210 M 0.420 M दाव 11) () The reaction 2NO(g) +2H₂(g) → N, (g) + 2H₂O(g) was studied at 904°C, and the data in the table were collected. (SHOW CALCULATIONS) [H₂] 0.150 M 0.300 M 0.150 M Ezer b) What is the rate law for the reaction? 1-01-0 Initial Rate 0.0339 M/s 0.0678 M/s 0.136 M/s a) Using the data, determine the order for each reactant. Show any calculations or explain reasoning. c) What is the value of the rate constant, k, for this reaction? -= 12) The reduction half-reaction for the deposit of copper metal is: Cu²+ (aq) +2e → Cu(s) How long will it take to deposit 2.5 g of copper using a current of 3.25 A? (molar mass Cu = 63.5 g/mol, F = 96,500 C/mol) (SHOW CALCULATIONS) 3) (4) Balance the following skeleton oxidation-reduction reaction. The reaction occurs in an acidic solution. (Show all steps and sub steps using the half reaction method) NO+CIO3 → NO3 + HClO₂

Which of the following is not true? 1. When conditions are NOX-limited, the excess of VOCs in the atmosphere quickly oxidize available NO to NO2. 2. Reducing the concentration of NOX may lead to an increase in ozone formation when conditions are VOC- limited. 3. Smog episodes are not initiated during nighttime hours, because the hydroxyl radicals necessary to initiate the reactions are formed due to photodecomposition reactions. 4. Photochemical smog never occurs in areas without significant vehicle traffic and power plant emissions. 4. Metropolitan areas surrounded by wooded areas need to focus their smog reduction on limiting NOX concentrations due to the VOCs produced by surrounding trees.

Using the reaction and data in the table below answer the following series of questions. CH3OH(aq) + HCl(aq) ----> CH3Cl(aq) + H2O(I) Reaction CH3OH conc. HCl conc. Initial Rate (M/s) 1 0.100 M 0.100 M 1.1 x 10-2  2 0.200 M 0.100 M 2.3 x 10-2 3 0.100 M 0.200 M 1.1 x 10-2 *conc = concentration a.  The reaction is                                order in regards to CH3OH. b.  The reaction is                              order in regards to HCl.

What is the role of sodium and chloride ions in this experiment

A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) = H*(aq) + A¯(aq) The equilibrium concentrations of the reactants and products are [HA] = 0.100 M, [H*] = 3.00 × 10-4 M, and [A-] = 3.00 x 10-4 M. Calculate the value of pK, for the acid HA. pKa =

DDT (molar mass = 354.49 g/mol) was a widely used insecticide that was banned from use in the United States in 1973. This ban was brought about due to the persistence of DDT in many different ecosystems, leading to high accumulations of the substance in many birds of prey. The insecticide was shown to cause a thinning of egg shells, pushing many birds towards extinction. If a 20-L drum of DDT was spilled into a pond, resulting in a DDT concentration of 8.9 x10^-5 M, how long would it take for the levels of DDT to reach a concentration of 1.41x10^-7  M (a level that is generally assumed safe in mammals)? Assume the decomposition of DDT is a first-order process with a half-life of 56.0 days.

DDT (molar mass = 354.49 g/mol) was a widely used insecticide that was banned from use in the United States in 1973. This ban was brought about due to the persistence of DDT in many different ecosystems, leading to high accumulations of the substance in many birds of prey. The insecticide was shown to cause a thinning of egg shells, pushing many birds towards extinction. If a 20-L drum of DDT was spilled into a pond, resulting in a DDT concentration of 8.21 x 10-5 M, how long would it take for the levels of DDT to reach a concentration of 1.41 x 10-7 M(a level that is generally assumed safe in mammals)? Assume the decomposition of DDT is a first-order process with a half- life of 56.0 days. Time = days

THIS IS WRONG PLEASE HELP BY GIVING RIGHT ANSWER. THIS IS A CHEMISTRY PROBLEM, NOT A WRITING OR ESSAY ASSIGNMENT!!!!!!!!

9-12 please

please balance equations 13-15