As temperature increases does a compounds vapor pressure change? Does its boiling point change? Explain

use daltons law to calculate pressures in mixtures of gases.

any examples on this review? please provide a problem with steps leading to a solution to help me review, thanks!

Why might percent recovery be low during extractions?

A mixture that contains benzoic acid, 4-chloroaniline and naphthalene. The 4-chloroaniline is separated first by extraction with hydrochloric acid.Since no phenolic compound is present in this mixture, two extractions with base solution are not required; thus, the benzoic acid could be separated from the neutral compound by extraction with either aqueous sodium bicarbonate or aqueous sodium hydroxide solution. We have chosen to extract the acidic compound into the aqueous layer using sodium hydroxide.

My percent recovery for 4-chloroaniline= 13% Benzoic acid: 30.2% Naphthalene: 25.2%

Use bond enthalpies to estimate

a) the enthalpy of the anaerobic breakdown of glucose to lactic acid in cells that are starved of oxygen, C6H12O6(aq) → 2 CH3CH(OH)COOH(aq),

b) the enthalpy of combustion of glucose. Ignore the contributions of enthalpies of fusion and vaporization.

Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points:

SHOW ALL WORK IN NEAT DETAIL ON A SEPARATE PAGE. (Be sure to write chemical equations and Ka or Kb expressions when needed.)

a. (4 Pts) Before any NaOH is added.

b. (4 Pts) After 18.7 mL of NaOH are added.

c. (4 Pts) After 25.00 mL of NaOH are added.

d. (4 Pts) After 50.00 mL of NaOH are added.

e. (4 Pts) After 53.00 mL of NaOH are added.

f. (1 Pt) What is the pKa of the acid (show calculation)?

Find the pH during the titration of 20.00 mL of 0.1500 M benzoic acid, C6H5COOH (Ka = 6.3 10-5), with 0.1500 M NaOH solution after the following additions of titrant. (a) 0 mL (b) 10.00 mL (c) 15.00 mL (d) 20.00 mL (e) 25.00 mL

Describe how the retention time of a peak is calculated if dichloromethane is injected with the sample

Ethanol (C2H5OH) is a very important chemical.in addition to being widely used as an industrial solvent,a gasoline additive,and an alternative fuel,it is well known as the alcoholic beverages.A common name for ethanol is grain alcohol because it is formed by the fermentation of glucose (C6H12O6) and other sugars in grains such as corn,wheat and barley:
C6H12O6---'C2H5OH + CO2
The previous reaction has been carried out for many centuries and is one of the oldest manufacturing processes.In a more recent development,ethanol can be prepared by reacting ethylene (found in petroleum) with water:
C2H4 +H2O ---C2H5OH
a.write the balanced equation for each of the two reactions above
b.Calcute the % A.E ( for the product ethanol) for the two reactions.
c.Explain how you can determine which reaction has the higher atom economy without doing the calculation in part (b) above .
d.Is either method sustainable?Which one? justify your answer.
e.Given the result from parts (b) and (d) above ,select one of the two methods as the better candidate overall for preparing ethanol.justify your selection.

There are two possible methods for recovering copper from a solution of copper (II) sulfate, one uses precipitation and the other uses redox.

(a) Copper(II) ions can be precipitated as copper(II) carbonate.

CuSO₄(aq) + Na₂CO₃(aq) → CuCO₃(s) + Na₂SO₄(aq)

How many mL of 0.144 M Na₂CO₃ would be needed to precipitate all of the copper ions in 25.5 mL of 0.165 M CuSO₄? How many grams of CuCO₃ could be recovered? (Include units in your answer. More information.)

(b) Copper(II) ions can be displaced by aluminum metal.

3 CuSO₄(aq) + 2 Al(s) → Al₂(SO₄)₃(aq) + 3 Cu(s)

How many grams of Al would be needed to displace all of the copper ions in 25.5 mL of 0.165 M CuSO₄? How many grams of Cu could be recovered? (Include units in your answer. More information.)

Please be very specific with the answers!! I only have one submission left and im very lost!

Part A

Aspirin (acetylsalicylic acid, C9H8O4) is a weak monoprotic acid. To determine its acid-dissociation constant, a student dissolved 2.00 g of aspirin in 0.600 L of water and measured the pH. What was the Ka value calculated by the student if the pHof the solution was 2.62?

Express your answer numerically using two significant figures.

Part B

A 0.100 M solution of ethylamine (C2H5NH2) has a pH of 11.87. Calculate the Kb for ethylamine.

Express your answer numerically using two significant figures.

Analyze the reactions below and determine which of them has the largest relative increase in entropy? Circle your choice and explain your answer qualitatively.

CO (g) + 3 H2 (g) <---> CH4 (g) + H2O (G)

C (s) + H2O (g) <---> CO (g) + H2 (g)

CH4 (g) + Cl (g) <----> CH3Cl (g) + HCl (g)

Complete and Balance each reaction in molecular, ionic, and net ionic form:

1. AgNO3(aq) + K2CrO4(aq) ---->

Ionic:

Net Ionic:

2. Ba(NO3)2(aq) + (NH4)3PO4(aq) ---->

Ionic:

Net Ionic:

3. NaHCO3(aq) + H3PO4(aq) ----->

Ionic:

Net Ionic: