This question was created from VVS Module 6 Summative Assessment.pdf

Question This question was created from VVS Module 6 Summative Assessment.pdf https://www..com/file/43143716/VVS-Module-6-Summative-Assessmentpdf/ how would this be done for cuso4 and k2cr2o7 ATTACHMENT PREVIEW Download attachment 43143716-334196.jpeg System 4 Answer [11 Marks) Fully Labelled Diagram Oxidation Half- Reduction Half- reaction Net Cell Reaction Cell Notation Empirical Anode: Evidence Cathode: Theoretical Standard Cell Potential Observed Cell Potential

Use the reaction 2CO(g) O2(g) 2CO2(g) for the following

Question Use the reaction 2CO(g) O2(g)  2CO2(g) for the following questions. (7 points)       i. Write the equilibrium constant for the reaction. (1 point)       ii. What does Le Châtelier’s principle predict would happen to the equilibrium conditions if CO2 were added to the system? (1 point)       iii. What would happen to the equilibrium if the pressure were increased? (1 point)       iv. A gas mixture contains 4.8  10-4 M CO and 3.5  10-2 M O2, and Keq = 3.58  10-4. What would the equilibrium concentration of CO2 be at these conditions? (2 points)       v. If at another temperature the Keq = 8.28  1010, would the reaction favor product formation or reactants? Explain your answer. (2 points)

Question 2: Acids and Bases (10 points) style=”color:#000000;”> a. Arrhenius

Question Question 2: Acids and Bases (10 points) style=”color:#000000;”> a. Arrhenius acid-base reaction (3 points)       i. Complete the following acid-base reaction. What does it mean that HI is a strong acid and CsOH is a strong base? (2 points)HI CsOH        ii. How does HI fit the definition of an Arrhenius acid, and how does CsOH fit the definition of an Arrhenius base? (1 point) b. Brønsted-Lowry acid-base reaction (3 points)       i. Identify the conjugate acid-base pairs in the following reaction. Indicate what each substance is in each pair. (2 points)H2CO3  PO43-  HCO3-  HPO42-       ii. How do the acid-base conjugate pairs fit the definition of Brønsted-Lowry acids and Brønsted-Lowry bases? (1 point) c. Lewis acid-base reaction (3 points)       i. What is the Lewis acid and what is the Lewis base in the reaction BF3  N(CH3)3  F3BN(CH3)? (2 points)       ii. Explain why the above chemical equation represents a Lewis acid-base reaction. (1 point) d. Which of the following bases is the weakest? Explain your answer. (1 point)(CH3)2NH, Kb = 5.1  10-4  ClO-, Kb = 2.9  10-7  SO42-, Kb = 8.3  10-13

The existing recommendations from the National Institute of Occupational Safety

Question The existing recommendations from the National Institute of Occupational Safety and Health (NIOSH) and the American Conference of Governmental Industrial Hygienists (ACGIH) are now as much as 100 times lower on some contaminants, but OSHA cannot enforce NIOSH or ACGIH levels if OSHA has its own published PEL. What do you think OSHA should do?

Question 3: pH and pOH (5 points) style=”color:#000000;”> a. What

Question Question 3: pH and pOH (5 points) style=”color:#000000;”> a. What is the difference in pH between an acidic solution and a basic solution? (1 point) b. A solution has a hydrogen ion concentration of 6.8  10-3 M. (2 points)       i. What is the pH of the solution? Show your work. (1 point)       ii. What is the pOH of the solution? Show your work. (1 point) c. A weak base ionizes according to the reaction B H2O  BH   OH-. What would adding more BH do to the pOH? Explain your answer based on the Kb of the base. (2 points)

Question 4: Acid-Base Reactions (8 points) a. What is formed

Question Question 4: Acid-Base Reactions (8 points) a. What is formed in the reaction between a strong acid and a strong base? What is this type of acid-base reaction called? (2 points) b. What kind of experiment determines an unknown concentration of an acidic solution by adding a measured amount of a basic solution? (2 points) c. Antacids such as Rolaids and Tums are used to relieve heartburn and sour stomach. Products like these commonly contain substances such as Mg(OH)2, Al(OH)3, and CaCO3. (4 points)       i. What is it about these substances that soothe a burning stomach? How do they work? (2 points)       ii. Many antacids also have the ability to buffer the stomach acid. What would be the purpose of a buffer in an antacid? (2 points)

Question 5: Reaction Rate (16 points) style=”color:#000000;”> a. A high

Question Question 5: Reaction Rate (16 points) style=”color:#000000;”> a. A high school student went to a pharmacy to get some medicine. The pharmacist put the medicine in a dark brown bottle and told the student to keep it out of direct sunlight. Why? (2 points) b. The rate of a reaction 2NO(g) O2(g) 2NO2(g) is given by the rate law Rate = k[NO]2[O2], where the rate constant k = Ae-Ea/RT. Use these equations to answer the following questions. (2 points)      i. How would the rate of the reaction change if the concentration of NO were halved? (1 point)       ii. How does the rate law include the effect of temperature on reaction rate? (1 point) c. One step in the industrial production of hydrogen gas involves reacting CO with steam according to the reaction CO(g) H2O(g) 2 CO2(g) H2(g). Heat is produced in this reaction, which is represented by the following diagram. Use the equation and diagram to answer the following questions. (12 points)      i. What would increasing the temperature do to the reaction rate? Explain your answer. (2 points)       ii. What would increasing the temperature do to the hydrogen yield? Explain your answer. (2 points)       iii. How would increasing the pressure affect the reaction rate? Explain your answer. (2 points)       iv. What would increasing the pressure do to the hydrogen yield? Explain your answer. (2 points)       v. This reaction is run using an iron catalyst. What would adding iron to the reaction do to the energy diagram? Explain your answer and draw the change on the energy diagram. (2 points)       vi. How does the catalyst accomplish its effect on the energy diagram of a reaction? What does the change do to the reaction rate? (2 points)

1. The normal melting and boiling points of a substance

Question 1.     The normal melting and boiling points of a substance are -163°C and -128°C respectively. Its triple point is at 125 K and 0.37 atm. Its critical point is at 150 K and 1.45 atm. a.      Sketch the phase diagram for the substance, showing the four points given and indicating the area in which each phase is stable (i.e. solid, liquid, gas regions).b. As it is heated, will the substance sublime or melt under a pressure of 0.20 atm?

1. What is the final temperature of water given an

Question 1.    What is the final temperature of water given an initial temperature of 28 ˚C, a mass of 5 g, and heat (q) of 184 J (Specific Heat of water = 4.184 )?2.    What is the specific heat of a metal with a mass of 14.0 g, heat of 2.45 kJ and a change in temperature of 3.2 ?

Please refer to the periodic table link below to pick one

Please refer to the periodic table link below to pick one of the transition element and talk about the element’s physical, chemical properties, preparation, discovery, and industrial application of that element. Your essay should be no more than 200 words.

Question 1:Part A: Calculate % mass of a solution made

Question Question 1:Part A: Calculate % mass of a solution made by dissolving 20 grams of NaOH in 100 grams of H2O.a. 5.0% 16.7% c. 20.0% d. 40.0%Provide A Rationale For Your Answer:Use the diagram for parts b, c, and d:Part B: 43. At what temperature will 50 g of KCl dissolve in 100 g of water?a. 50 °C b. 65 °C c. 80 °C d. 100 °CProvide A Rationale For Your Answer:Part C: 44. How much KNO3 will dissolve in 200 g of water at 50 °C?a. 40 g b. 80 g c. 100 g d. 160 gProvide A Rationale For Your Answer:Part D: 45. How much more NaNO3 will dissolve in 100 g of H2O if the temp rises from 10°C to 35°C?a. 11 g b. 20 g c. 56 g d. 93 gProvide A Rationale For Your Answer: ATTACHMENT PREVIEW Download attachment 1565220368743.png

I just need the answers please

Question

I just need the answers please

ATTACHMENT PREVIEW Download attachment 21586448-334096.jpeg Copyright @ 2015 Apex Learning Inc. Use of this material is subject to Apex Learning’s Terms of Use . Any unauthorized copying, reuse, or redistribution is prohibited. Apex Learning @ and the Apex Learning Logo are registered trademarks of

I need to know the concentrations as well as the

Question I need to know the concentrations as well as the moles. alt=”6B8DB013-DB80-4D9D-B15F-56DF9F6AEE84.jpeg” /> Attachment 1 Attachment 2 ATTACHMENT PREVIEW Download attachment 6B8DB013-DB80-4D9D-B15F-56DF9F6AEE84.jpeg Procedure, Part III: Spectrophotometric Analysis of Nickel Reread Experiment 1 in this manual for instructions on the use of a pipet. Read the section on Beer’s Law and the use of the spectrophotometer in Experiment 10 for information on how to perform the spectrophotometric analysis. Experiment 10 also contains information on using a volu- metric flask. Preparation of Standard Nickel Solutions In this part of the procedure, you will create a set of three solutions of known concentration in NiCl2.6 H2O and measure their absorbance. You will use this data to graphically determine the concentration of nickel in the unknown solution. See the Introduction to this experiment for further explanation. Obtain a clean, rinsed 50 mL volumetric flask and a clean, dry 150 mL beaker. Weigh the beaker on the analytical balance and record the mass to 0.001 g on the data sheet. Add approximately 1.1 g of NiCl2.6 H2O, and record the mass of the beaker and its contents exactly. Dissolve the crystals completely in about 30 mL of 0.5 M H2SO4, with stirring. Transfer the solution to the 50 mL volumetric flask using your stirring rod to avoid losing any solution. Wash the beaker three times with 3 mL portions of 0.5 M H2SO4, transferring the washings quantitatively to the flask. Dilute the solution in the flask exactly to the mark with 0.5 M H2SO4, stopper, and mix thoroughly by inverting the flask several times. Calculate [Ni2 ] of nickel in this stock solution. The stock solution will serve as one standard solution; you will need to create two others, so that you can measure how absorption changes as a function of concentration. Prepare the two additional standards diluted as follows: Pipet 10.0 mL of the stock solution into a clean, rinsed 25 mL volumetric flask and dilute to the mark with 0.5 M H2SO4 (invert twice to mix thoroughly). Then pipet 20.0 mL of stock solution into a second 25 mL volumetric flask and dilute with acid (mix). Calculate [Ni2 ] in each of these diluted standard solutions. Preparation of the Complex Compound Solution Place approximately 0.6 g of your complex compound in a pre-weighed 150 mL beaker, and record the mass of your complex as exactly as possible. Dissolve in roughly 30 mL of H2SO, and transfer to a 50 mL volumetric flask. Rinse with H,SO, and dilute the solution to exactly 50 mL, as described above for the preparation of the stock solution. Spectrophotometric Measurements Obtain two cuvettes (see directions for how to handle these). One will be a reference blank for the spectrophotometer and the other will contain the solution to be measured. Fill the blank cuvette to its fill line with 0.5 M H2SO4. Fill the other cuvette to the fill line with one of the stock solutions; you should use the same blank in all of your measurements, so do not discard this solution until the experiment is complete. Make a measurement with the spectropho tometer (the wavelength should be 395 nm) and record the absorbance. Empty the stock solution int the waste container, then rinse the cuvette with distilled water and dry it. Then measure the abso bance with each of the other two standard solutions. Finally, measure the absorbance of the solution containing your synthesized compound.Read more ATTACHMENT PREVIEW Download attachment C8DE9F0F-9005-43F4-B52D-35C2859835EF.jpeg Analysis of Nickel Sample Preparation: Mass of beaker and NiCl,.6 HO 66 .426 9 Mass of beaker 65 . 325 g Mass of NiCl2.6 H20 1. 1 235 Mass of beaker and compound 69. 620 Mass of beaker 68. 970 Mass of compound 0 , 634 Spectrophotometric Measurements: Absorbance Concentration (mol/L) Stock Solution 0. 589 mm 0. 5 mol /L First diluted solution 2. 228 mm Second diluted solution 0.464 mm Complex compound solution 0. 358 am Estimated concentration of synthesized compound in solution based on Beer’s Law plot: Hand-drawn: mol/L Computer-generated (optional): mol/L (Circle the value above that you are using for your calculations below.) Moles of nickel in sample (total): Moles of nickel per gram of sample: Mass of nickel per gram of sample: Percentage by mass of nickel in sample: R THIS EXPERIMENT.

i have an experiment where students construct atoms i have

Question i have an experiment where students construct atoms i have to :1- Critically evaluate whether it has been well designed and is consistent with research-based theory on effective science education pedagogy as discussed in your texts and readings. Incorporate references to the literature to support your arguments (you must use the APA referencing style as per the School of Education referencing guide. References are not included in the word count).2- Modifications – How would you modify this activity to improve organisational or pedagogical outcomes? If you believe the activity requires no modification, justify your position.3- Organisation and logistics – How will you communicate the instructions to students (e.g. board, OHP, PowerPoint slides, handouts). How will you ensure they understand what is required? How will you group students to maximise their participation and achievement of outcomes? How would you ensure that students record the activity and results in an effective way?

1. Write the formula of the conjugate base for acid

Question 1. Write the formula of the conjugate base for acid H2CO3.Express your answer as an ion.2. Calculate the [OH−] of each aqueous solution with the following [H3O ]:stomach acid, 4.5×10−2MExpress your answer using two significant figures.urine, 6.0×10−6MExpress your answer using two significant figures.orange juice, 2.2×10−4MExpress your answer using two significant figures.bile, 7.0×10−9MExpress your answer using two significant figures.3.what is the balanced equation for the neutralization of each of the following. H2SO4(aq) and KOH(aq)Express your answer as a chemical equation. Identify all of the phases in your answer.HCl(aq) and Al(OH)3(s)Express your answer as a chemical equation. Identify all of the phases in your answer.H2SO3(aq) and Mg(OH)2(s)4. What is the chemical formula for the base cobalt(III) hydroxide?Express your answer as a chemical formula.The formula for the selenate ion is SeO42−. Predict the formula for selenic acid.5. How many moles of Ba(OH)2 are present in 125 mL of 0.600 M Ba(OH)2?Express your answer with the appropriate units.

1. Explain the expected relative conductivity of 0.10 mol/L samples

Question 1.            Explain the expected relative conductivity of 0.10 mol/L samples of hydrobromic acid, benzoic acid, and hydrocyanic acid.a.          Using the five-step method, predict the predominant Bronsted-Lowry acid base reaction when solutions of ammonium chloride and sodium hydrogen carbonate are combined.  a.            Predict whether the equilibrium will favour the formation of the reactants or products. Support and explain your answer.

A 4.50 g of hydrogen gas is produced when a

Question A 4.50 g of hydrogen gas is produced when a sample of magnesium ­metal is reacted with an excess of hydrochloric acid solution according to the reaction below. How many moles of the magnesium metal were reacted?.Mg(s) 2HCl(aq) —-> MgCl2(aq) H2(g) 

write balanced chemical equations for the aerobic respiration reaction of

Question write balanced chemical equations for the aerobic respiration reaction of sucrose, showing how it reacts with oxygen to produce energy?

1. A 100 mL sample of hydrazoic acid, HN3(aq) with

Question 1.   A 100 mL sample of hydrazoic acid, HN3(aq) with a concentration 0.25 mol/L has a pH of 2.78. Calculate the Ka for hydrazoic acid. Remember, when calculating the Ka, do not round off any of the numbers until the very end of the calculation!.2.     Calculate the pH of a 0.025 mol/L solution of magnesium hydroxide.3.     Calculate the pH of a 0.025 mol/L solution of sodium nitrite.4.   Hydrazine, N2H4(aq), is used in the preparation of polymers, pharmaceuticals and rocket fuel. Hydrazine has alkaline properties similar to ammonia and will act as a weak base. Given that a 100 mL sample of 0.10 mol/L hydrazine solution has a pH of 10.55 at 25.0 oC, write the formula for the conjugate acid and calculate the Ka of the conjugate acid. Formula for the conjugate acid of hydrazine: Calculate the Ka of the conjugate acid:

Use redox theory to explain the corrosion of iron and

Question Use redox theory to explain the corrosion of iron and briefly describe 2 ways to prevent or slow therust forming process.

Electrochemistry review question. ATTACHMENT PREVIEW Download attachment Question.png 13. Balance

Question Electrochemistry review question. ATTACHMENT PREVIEW Download attachment Question.png 13. Balance the following redox reaction by the oxidation number method, be sure to show your steps: CuO NH; –

The post This question was created from VVS Module 6 Summative Assessment.pdf appeared first on Smashing Essays.

Looking for a Similar Assignment? Order now and Get 10% Discount! Use Coupon Code "Newclient"