A fictional company has been producing propene oxide, C3H6O, from propene, C3H6, with a 96.0%yield. The process requires the use of a compound called m-chloroperoxybenzoic acid, C7H5O3Cl, which can be abbreviated as mCPBA. The entire reaction takes place in the solvent dichloromethane, CH2Cl2:

C3H6+C7H5O3ClCH2Cl2−−−⟶96.0% yieldC3H6O+C7H5O2Cl

The initial propene concentration in the solvent is 21.0 g/L.

Consider the prices of the following substances.

Also consider that the cost of waste disposal is $5.00 per kilogram of propene oxide produced.

Part A

A relatively simple way of estimating profit is to consider the the difference between the cost (the total spent on materials and waste disposal) and the earnings (the price at which the product can be sold).

Calculate the profit from producing 67.00 kg of propene oxide.

Express your answer numerically in dollars using three significant figures.

#1. Which following statement statements is WRONG for Benzocaine?

A. It is an aromatic carboxylic ester.

B. Benzocaine is acidic in nature.

C. It is basic in nature.

D. Benzocaine is used to reduce the pain or discomfort caused by sore throat, teething pain, rectal irritation, hemorrhoids etc.

E. It does not show any side effects if you take more than the dose.

F. It is a colorless trapezial crystal.

#2: Why is sulfuric acid added in an Esterification reaction? (synthesis of benzocaine)

a. It neutralizes base produced in the reaction.

b. It pushes the reaction to completion by dehydrating the product.

c. It is used as a polar protic solvent

d. It activates the carbonyl of p-aminobenzoic acid making it more reactive.

e. A low pH is needed for the reaction to occur

#3. How many different types of proton (By looking H1 NMR spectrum) present in the Benzocaine?

#4. In the IR spectrum of Benzocaine, which peaks are representing C-O stretching bands?

Determine the amount of silver in a saturated solution of silver iodide. Sketch a graph showing how the concentration of silver would change if increasing amounts of potassium nitrate were added. Note, you should label the axes of the sketch but you do not need to include numbers. Note that appendix 10 contains Ksp values.

Moles of Reactant to Moles of Product: Use mole ratio from balanced chemical equation.

1.Ammonia burns in oxygen according to the following equation:

4 NH₃ + 3 O₂  → 2 N₂ + 6 H₂O

How many moles of nitrogen gas are generated by the complete reaction of 8.23 moles of ammonia? Express your answer to two decimal places.

mol N₂

2.

Moles of Product to Moles of Reactant: Use mole ratio from balanced chemical equation.

The commercial process used to make nitric acid is as follows:

3 NO₂(g) + H₂O(l)  → 2 HNO₃(aq) + NO(g)

How many moles of nitrogen dioxide are required to produce 7.19 moles of nitric acid? Express your answer to two decimal places.

mol NO₂

3.

Moles of Reactant to Mass of another Reactant: Balance equation. Use mole ratio, then convert to grams.

Balance the chemical equation showing the reaction of sulfuric acid with calcium phosphate to produce phosphoric acid and calcium sulfate:

Ca₃(PO₄)₂(s) +   H₂SO₄(aq)  →   CaSO₄(s) +   H₃PO₄(aq)

What mass of calcium phosphate is needed to completely reacted with 6.665 moles of sulfuric acid? Express your answer to two decimal places.

g Ca₃(PO₄)₂

4.

Moles of Product to Mass of Each Reactant: Perform a separate calculation for each reactant. Use mole ratio, then convert to grams.

If 0.63 moles of carbon monoxide gas are produced by the following reaction, how many grams of silicon dioxide and of carbon were reacted (assume just enough of each)? Express your answer to two decimal places.

SiO₂(s) + 2 C(s)  → Si(l) + 2 CO(g)

Mass of SiO₂ needed:  g

Mass of C needed:  g

5.

Moles of Reactant to Mass of Reactant: Identify the iodide ions and ozone in the balanced chemical equation. Use mole ratio, then convert to grams.

A method used by the EPA for determining the ozone concentration in the air is to pass an air sample through a bubbler containing iodide ions. The iodide ions remove the ozone according to the following reaction:

O₃(g) + 2 I^-(aq) + H₂O(l)  → O₂(g) + I₂(aq) + 2 OH^-(aq)

How many grams of ozone can be removed from the air sample if 5.11 moles of iodide ions are present in the bubbler? Express your answer to two decimal places.

g

A student was given buffer solutions to calibrate the pH electrode that were labeled incorrectly. The pH's of both buffer solutions were actually lower than the pH's shown on the labels. Explain how such an error would affect the experimental result for the K_a of acetic acid.

2.The solubility of silver chromate (Ag2CrO4) is 2.22 x 10-3 g/100 mL.

a) What is the Ksp? Include the chemical equation and Ksp expression. MW (Ag2CrO4): 332 g/mol

b) What happens to the solubility of Ag2CrO4 in the presence of ammonia?

c) If 0.050 moles of silver nitrate are added, what is the solubility of Ag2CrO4?

How many grams of copper be deposited at the cathode of an electrolysis cell if an electric current of 15 mA is applied for 1.0 h through an aqueous solution containing excess Cu2+ ions? Assume the process is 100°0 efficient.

Question 1

Which of the following are variables that can be manipulated in a gas law equation? (Choose all that apply)

Group of answer choices

number of moles

temperature

pressure

mass

Question 2

True or False. According to Charles’s Law, if you have a balloon inside a car at noon during a hot summer day, the molecules inside of the balloon will cause the volume of the balloon to increase.

Group of answer choices

True

False

Question 3

Name the gas law. Volume and pressure are indirectly proportional. Volume will decrease if pressure increases, and volume will increase if pressure decreases.

Group of answer choices

Avagadro’s

Gay-Lussac’s

Charles’s

Boyle’s

Question 4

Name the gas law. Temperature and pressure are directly proportional. If temperature increases, pressure will increase as well.

Group of answer choices

Charles’s

Gay-Lussac’s

Avagadro’s

Boyle’s

Question 5

What effect would a decrease in temperature have on pressure, assuming that volume (T) and moles of gas (n) are kept constant?

Group of answer choices

Pressure would decrease.

Pressure would stay the same regardless of a change in temperature.

Pressure would increase

Question 6

Which temperature scale has NO negative values?

Group of answer choices

Farenheit

Digital

Kelvin

Celcius

Question 7

Calculate the number of moles of gas with a volume of 35.0 L at a temperature of 32°C and pressure of 1.20 atm.

Group of answer choices

10.5 mol

0.596 mol

Did you rearrange PV=nRT correctly for n?

Does your temperature value have the correct units?

1.68 mol

Question 8

What is the temperature (°C) of 5.20 moles of gas in a 40.0 L container with a pressure of 4.50 atm?

Group of answer choices

149°C

237°C

422°C

273°C

Question 9

Calculate the volume of 3.3 moles of gas with a pressure of 950 mmHg and temperature of 25 °C. (Hint: 760 mmHg = 1 atm)

Group of answer choices

5.4 L

0.02 L

11.8 L

64.6 L

Question 10

A balloon has a volume of 875 mL at STP. At what temperature will the balloon have a volume of 1.33 L at a pressure of 0.72 atm?

Group of answer choices

3.08°C

25.7°C

299°C

0.299°C

If you were to add 10.0mL of 0.10M sodium acetate solution, what is the amount of CH3COOH(mol), Amount of CH3COO-(mol), and the predicted pH by the Henderson-Hasselbalch equation?

Given:

Start with sodium acetate

Add HCl

Initial Burette reading: 6.70ml

Final Burette reading: 9.80mL

Amount of HCl added(mol): 3.1 x 10^-4 mol

Justify the phospholipid being the major component of the cell membrane. Be specific and complete.

Question

1) A 1.0 mL aliquot (sample) is taken from a 1.0L solution. Which of the following is/are true when comparing the 1.0 mL solution to the 1.0L solution? Choose all that are true.

-The molarity of the 1.0 mL solution is less than the molarity of the 1.0L solution

-The molarity of each is the same

-The number of moles of solute in each solution is the same

-The number of moles of solute in the 1.0mL solution is less than the number of moles of solute in the 1.0 L solution

2) 5.00 mL is withdrawn from a 1.00L solution of NaCl and diluted to 100.00 mL. If the concentration of the NaCl in the 100.00 mL solution is 0.033, what is the concentration of NaCl in the original 1.00 L solution?

3) What is used as a blank (reference/zero absorbance) for the analysis of the samples in the spectrophotometer?

-Deioniozed water

- Nothing-air

-Acetylsalicylic acid standard solution

- Iron(III) chloride solution

4) The acetylsalycylic acid - iron (III) complex appears violet in color. What color of light is used to measure the absorbance of the solution?

- red

- orange

- green

- blue

- violet

5) A calibration curve for absorbance versus the concentration of the chemical indicator crystal violet is found to have a slope of 48. If a sample of unknown concentration has an absorbance of 1.38, what is the concentration in the unknown sample?

Most of our discussion of transition metals has focused around them becoming positively charged ions. However, many of the transition metals will also become negatively charged ions. Using what you have learned from quantum mechanics and about electron configurations, predict which transition metals are most likely to form anions with a charge of -1 and explain the prediction.

Triethlyamine is added with deionized water, what is the chemical equation? Next, this solution is now neutralzied by adding HCL. What is the chemical equation and name of the salt? Finally, NaOH is added to the solution, what is the chemical equation showing the free amine? Please explain and show steps.

-- Consider a concentration cell. Two Ag-electrodes are immersed in AgNO3 solutions of different concentrations. When the two compartments have an AgNO3-concentration of 1 M and 0.1 M, respectively, the measured voltage is 0.065 V (note: T in not necessarily = 25°C ).

The electrochemical behavior of silver nanoclusters (Agn, with n the number of Ag atoms in the cluster) is investigated using the following electrochemical cells at 298 K:

I. Ag(s) | AgCl (saturated) || Ag+(aq, 0.01M) | Ag(s), E=0.170

II. (Pt electrode) Agn (s, nanocluster) | Ag+(aq, 0.01M) || AgCl (saturated) | Ag(s), with E = +1.030 V for Ag5 nanocluster and E = +0.430 V for Ag10 nanocluster

The standard reduction potential for Ag+ + e- → Ag, is E0 = +0.800 V.

The two nanoclusters Ag5 and Ag10-nanoclusters have standard potentials different from the potential of metallic bulk silver.

c. Calculate the standard potentials of Ag5 and of Ag10 nanoclusters. [for this part use Ksp(AgCl)=1.800·10-5;]

d. What happens, if you put the Ag10 nanoclusters and – in a second experiment – the Ag5 nanoclusters into an aqueous solution of pH=5? Estimate the consequences using the reduction potentials you calculated.