Scenario: You are an engineer supervising the work on a brownfield remediation project. Just before the close of business, as you are grabbing your coat, you notice one of your coworkers left some stock solutions out on the bench. Thinking you can quickly put them away and then go home, you walk over to do so, but you discover instead that the labels have not been put on the stock containers. There are labels on the counter, in front of the containers, but they have not been printed yet. There are four colorless glass containers, two of which contain a clear, colorless solution. The other two solutions have a dark bluish-green color. Over to the right are a number of containers that had been used recently. These containers contain chemical compounds, in solid form, that are commonly used in your lab. They are: barium nitrate, nickel (II) chloride, potassium nitrite, iron (III) nitrate, lithium sulfate, aluminum nitrate, sodium bromide, lead (II) chloride, calcium nitrate and magnesium fluoride. Can you identify the contents of the containers and put correct labels on the containers? Design a flowchart to show how you would test the solutions to determine what they might be. The flowchart must clearly list the chemicals needed for each test as well as show the expected test results.

One mole of an ideal monatomic gas is expanded from an initial state at 3 bar and 450 K to a final state at 2 bar and 250 K. There are two different paths for this expansion:
path 1: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas, 3 bar, 250 K) → (1 mole ideal gas, 2 bar, 250 K)
path 2: (1 mole ideal gas, 3 bar, 450 K) → (1 mole ideal gas, 2 bar, 450 K) → (1 mole ideal gas, 2 bar, 250 K)

Part A

Specify the paths carefully.

Check all that apply.

Part B

Calculate w for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part C

Calculate q for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part D

Calculate w for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part E

Calculate q for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part F

Calculate ΔU for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part G

Calculate ΔS for the path 1.

Express your answer to three significant figures and include the appropriate units.

Part H

Calculate ΔU for the path 2.

Express your answer to three significant figures and include the appropriate units.

Part I

Calculate ΔS for the path 2.

Express your answer to three significant figures and include the appropriate units.

alkynes can be hydrated in the presence of acid and HgSO4 by electrophilic addition of the molecule of water to the triple bond.The reaction proceedes by way of carbocation intermediate. Hydration of acetylene produces acetaldehyde. Outline the steps that occur in this transformation

You mix 28.0 mL of 0.298 M FeCl₃ with 39.5 mL of 0.423 M NaOH. What mass of Fe(OH)₃ (in grams) will precipitate from this reaction mixture?

One of the reactants (FeCl₃ or NaOH) is present in a stoichiometric excess. What is the molar concentration of the excess reactant remaining in solution after Fe(OH)₃ has been precipitated?

Calculate the freezing point of a solution containing 13.2 gg FeCl3FeCl3 in 159 gg water.

Calculate the boiling point of the solution above.

Calculate the freezing point of a solution containing 5.9 %% KClKCl by mass (in water).

Calculate the boiling point of the solution above.

Calculate the freezing point of a solution containing 0.151m MgF2

Calculate the boiling point of the solution above.

Calculate the mass of butane needed to produce 86.2 gg of carbon dioxide.

Which of the pH indicators from the following table would be most appropriate for the titration of 100 mL of 0.30 M acetic acid (Ka = 1.8 x 10-5 ) with 0.15 M sodium hydroxide?

w

1.              What material is most susceptible to hydrogen embrittlement?   

2.              What processes often generate hydrogen?

3.              What are three ways to prevent or mitigate hydrogen embrittlement?

4.              What is adhesive wear? What are two other terms for adhesive wear?

5.              What type of wear is likely to occur in bearings?

2 Ag+ + Cu --> Cu+2 + 2 Ag
You individually weigh out a piece of Copper Wire and an empty Reaction Tube. You add a measured volume of silver nitrate solution of known concentration to the Reaction Tube and drop in the copper wire.
Weight of copper wire 1.3771 g
Weight of empty Reaction Tube 6.4591 g
Volume of AgNO3 solution used 3.65 mL
Molarity of original AgNO3 solution 0.1536 M

While the silver is being reduced, you make the following spectroscopic measurements. The blank is distilled water. The STANDARD is made by pipetting 1.00 ml of the original standard into a cuvet and adding exactly 5.00 mL of ammonia + distilled water to give a total volume in the cuvet of 6.00 mL.
%T of Blank 99.1 %
Concentration of original Cu Standard 0.0361 M
%T of Cu Standard in cuvet 39.0 %

After the reaction is complete, 2.35 ml of 14 M ammonia is added to the Reaction Tube to give a total of 6.00 mL of blue solution. 1.00 mL is pipetted into the cuvet and 5.00 mL of ammonia and distilled water were added. The %T of this mixed homogeneous solution was measured in the spectrometer.
The mass of the remaining copper wire was measured
The precipitated silver metal in the Reaction Tube was washed with distilled water and dried and the reaction tube with silver crystals was weighed.
%T of Cu ion in Reaction Tube 24.8 %
Mass of Cu Wire after reaction 1.3579 g
Mass of dried Reaction Tube with Silver metal after reaction 6.5240 g
Calculate:
a) Mass of Silver Metal produced ______________ mg
b) Millimoles of Ag + used up ______________ mmol
c) Atomic Weight of Silver based on silver used up ______________ g/mol
d) Mass of Copper Metal lost from wire ______________ mg
e) Atomic Weight of Silver based on copper metal lost ______________ g/mol
f) Absorbance of Cu +2 standard ______________
g) Absorbance of Cu+2 in Reaction Tube ______________
h) Molarity of Cu+2 in Reaction Tube ______________ M
i) Millimole of Cu+2 in Reaction Tube ______________ mmol
j) Atomic Weight of Silver based on Cu+2 produced ______________ g/mol

Ethanol reacts with sodium dichromate in an aqueous hydrochloric acid solution according to the balanced net ionic equation shown below.

3 C₂H₅OH (aq) + 2 Cr₂O₇^2- (aq) + 16 H⁺ (aq) → 3 HC₂H₃O₂ (aq) + 4 Cr³⁺ (aq) + 11 H₂O (l)

This reaction is carried out with 1.00 mL of C₂H₅OH (density 0.816 g/mL, molar mass 46.07 g/mole) reacting with 32.76 mL of a solution that is 0.5775 M in Na₂Cr₂O₇ and 6.000 M in HCl.

What is the limiting reagent?

The mass of CrCl₃ (molar mass 158.36 g/mole) formed? (in grams)

According to The Aldol Addition and Condensation: The Effect of Conditions on Reaction Pathways for 3-Hydroxy-3-(4-nitrophenyl)-1-(2-pyridyl)-1-propanone, Answer this Q/

Q: 112 microliters of 2-acetylpyridine (121.14 g/mol, 1.08 g/mL) was reacted with 145 mg of 4-nitrobenzaldehyde (151.12 g/mol) and 35 mg of sodium carbonate (105.99 g/mol). What is the theoretical yield, in milligrams (mg), of the aldol addition product (254.25 g/mol)? Enter your answer as digits only (no units), using the proper number of significant figures.

1. The densities of crystalline Cl2 and H2S at 160 K are 2.02 and 0.95 g/cm3, respectively. Calculate their molar volumes.

2. The fluorocarbon compound C2Cl3F3 has a normal boiling point of 47.6 ∘C. The specific heats of C2Cl3F3(l) and C2Cl3F3(g) are 0.91 J/g⋅K and 0.67 J/g⋅K, respectively. The heat of vaporization for the compound is 27.49 kJ/mol.

Calculate the heat required to convert 73.0 g of C2Cl3F3 from a liquid at 13.90 ∘C to a gas at 99.80 ∘C.

Express your answer using two significant figures.

Calculate the enthalpy chamge when 75.0g of ethanol goes from 87.0 C to -15.0 C, given the following information for ethanol: c ethanol = 2.44j/g*C, Delta Hfusion=5.02 kj/mol, delta Hvap=38.56 kj/mol.

For a particular redox reaction NO is oxidized to NO3– and Cu2 is reduced to Cu . Complete and balance the equation for this reaction in basic solution. Phases are optional.

NO + Cu²⁺ ----> NO₃^- + Cu⁺

I know how to do it for an acidic solution, please show work for a basic solution. Thanks.