Acetic acid has a normal boiling point of 118 ∘C and a ΔHvap of 23.4 kJ/mol.What is the vapor pressure (in mmHg) of acetic acid at 40 ∘C?

how do you find bond angle measurement with a line bond structures

One mole of an ideal gas at 1.00 atm and 298K with C_{p,m=3.5R is put through the}

following cycle: a) (reversible) constant volume heating to twice its initial

temperature; b) reversible, adiabatic expansion back to its initial temperature;

c) reversible isothermal compression back to 1.00 atm. Calculate ΔS for each step and

overall. d) What is the change of entropy of the surroundings?

A chemistry graduate student is given 100.mL of a 1.50M diethylamine C2H52NH solution. Diethylamine is a weak base with =Kb×1.310−3. What mass of C2H52NH2Cl should the student dissolve in the C2H52NH solution to turn it into a buffer with pH =11.35? You may assume that the volume of the solution doesn't change when the C2H52NH2Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.

A. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

NO₃^-

H₃PO₄

NH₄⁺

HClO

None of the Above

B. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

NH₄⁺

NH₃

Ca(OH)₂

Br^-

None of the Above

C. Which of the following can behave as Bronsted-Lowry bases in aqueous solution?

HCO₃^-

NaOH

KOH

HF

None of the Above

* please help me I am really struggling with this concept. I fully cannot seem to grasp it and really need to understand it*

Find the pH of each of the following solutions of mixtures of acids.

a) 0.120 MM in HBrHBr and 0.135 MM in HCHO2HCHO2

Express your answer to three decimal places.

b) 0.155 MM in HNO2HNO2 and 9.0×10⁻² MM in HNO3HNO3

Express your answer to two decimal places.

c) 0.185 MM in HCHO2HCHO2 and 0.22 MM in HC2H3O2HC2H3O2

Express your answer to two decimal places.

d) 4.5×10⁻² MM in acetic acid and 4.5×10⁻² MM in hydrocyanic acid

Express your answer to two decimal places.

Osmium (76Os) has seven naturally occurring isotopes, six of which are stable. Osmium 193 is a beta-emitter. A sample of 193Os with mass of 58.36 μg emits 13.52×108 β

particles in a time interval of 32 min. What is the half-life (in years) of this nuclide?

1. What normally happens when iodine is added to starch?

2.Tube 2 contained starch at the beginning of the experiment. How do you explain the reaction with iodine at the end of the experiment?

3. What food substance is tested by using Benedict's solution?

Determine the pH?

1)   0.18M KCHO2

2)   0.15M CH3NH3I

3)   0.19M KI

thanks

Rather than titrating the active ingredient in an antacid directly with a standard solution of a strong acid in our buret, in this experiement we first dissolve the antacid tablet in a measured excess of standard acid, and then titrate (with standard sodium hydroxide solution) the portion of the acid that was not consumed by the tablet. Explain.

Organic Structures Shapes and Isomerism

Hands-On Labs, Inc.
Version 42-0183-00-02

Lab Report Assistant

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor.

Exercise 1: Organic Structures Shapes and Isomerism

Data Table 1. The Tetrahedral Carbon Atom.

Data Table 2. Alkanes and Alkyl Groups.

Data Table 3. Isomers.

INSERT A PICTURE OF YOUR BUTANE ISOMERS.

Data Table 4. Cycloalkanes.

Questions

Part A

What is the difference in the number of carbon atoms between methane and ethane and between ethane and propane?

Part B

What is the difference in the number of hydrogen atoms between methane and ethane and between ethane and propane?

Part C

What is the formula for a 6 carbon alkane?

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