Do you think that eggs are healthy food? Explain using the appropriate chemistry terminology, and provide at least two references to support your arguments.

1. A 0.17-mole sample of nitrogen gas occupies a volume of 2.80 L . What is the volume of 0.29 mol of nitrogen gas under the same conditions? Express your answer using two significant figures. V=

2. A sample of gas with an initial volume of 32.0 L at a pressure of 760 mmHg and a temperature of 320 K is compressed to a volume of 16.3 L and warmed to a temperature of 445 K . What is the final pressure of the gas? Pfinal =

3.

6. Use the combined gas law to complete the following table (assume the number of moles of gas to be constant): . Complete each column

1) Rank the following from the strongest acid to the weakest acid. Explain with reasons please.
A) CH3CH2OH
B) CH3OCH3
C) CH3—NH—CH3
D) CH3—C≡CH
E) CH3—CH=CH2

2) Draw all possible isomers that have the molecular formula C5H12O and name them using the systematic IUPAC name.

3) The following compound has 2 isomers. One isomer has a dipole moment of 0 D, whereas the other has a dipole moment of 2.95 D. Propose structures for the 2 isomers that are consistent with these data. ClCH=CHCl

1. can ice be melted merely by applying pressure? how about dry ice? Explain your answers.
2. explain how the solid liquid line in the phase diagram of water differs in character from the solid liquid line in the phase diagrams of most other substances such as CO2.
3. which phase of a substance (gas, liquid or soild) is most likely to be the stable phase:(A) at low temperature and high presumes (b)at high temperature and low pressure?
4. at what temperature and pressures does a substance behave as a supercritical fluid?
5. explain why a needle floats on the surface of water but sinks in a container of methanol?
6. explain why the plumbing in a house may burst If the temperature in the house drops below O°C?
7. a hot needle sinks when placed on the surface of cold water but a cold needle floats why?
8.what kind of intermoloccular force must be overcome as (a) soild CO2 sublime (b) CHC13 boils (c) ice melts?

The oxidation of copper(I) oxide, Cu2O(s), to copper(II) oxide, CuO(s), is an exothermic process,

2Cu2O(s) + O2(g) ----> 4CuO(s) Delta H (reaction)= -292.0 Kj/ mol

Calculate the energy released as heat when 9.67 g of Cu2O(s) undergo oxidation at constant pressure.

How much 6.0M NaOH must be added to .500 L of a buffer that is .0200M acetic acid and .025 M sodium acetate to raise the pH to 5.75 at 25C?

In which of the following pairs of bonds is the shorter bond length not followed by the longer bond length?

1. Describe below (briefly) a) the motivation for hybridization in valence bond theory and b) why valence bond theory cannot predict magnetism. In your answer, make sure to include a description of how molecular orbital theory addresses magnetism.

What is the pH of a solution which begins to precipitate PbS (Ksp = 8.4 x I 0-28 from a solution which is 0.01 M with respect to Pb2+ and has an H2S concentration of 0.02M. Im totally stuck so if you could walk me through to the answer, that would be awesome.

Consider what is the pH of the solution when 25.0mL of 0.01M NaOH is added to 25.0mL of 0.01M acetic acid. Is it the same as in the case of HCl solution? What will the pH of the solution be if exactly 12.50mL of 0.01M NaOH solution is added to 25.0mL of 0.01M acetic acid solution?

Describe the protein Keratin with cited sources describing the function of this protein.

a) Give the mathematical equilibrium constant expression Kc and Kp (not the value!) for the reaction

2N2O5(g) ↔ 4NO2 (g) + O2(g)

b) At 250oC the concentrations of N2O5, NO2 and O2 are 0.100 mol/L, 0.0283 mol/L and 0.0105 mol/L. Calculate the values for Kc and Kp

An electrochemical cell is based on the following two half-reactions:

Ox: Sn(s)→Sn2+(aq, 1.65 M )+2e−

Red: ClO2(g, 0.165 atm )+e−→ClO−2(aq, 1.90 M )

Compute the cell potential at 25 ∘C.

Consider mixing an excess of lead(II) nitrate (aq) with 200.0 mL of 0.400 M sodium chloride. Determine the mass of solid formed, assuming a complete reaction

What volume (in mL) of 0.800 M lead(II) nitrate must you add to make sure you make the mass of product you calculated in problem 3?

A 0.1044 g sample of the salt MCl was dissolved in water (making it in the aqueous phase). An excess of AgNO3 (aq) was added, precipitating 0.0889 g AgCl. What is the identity of M?

For the following reactions, state whether you expect ΔSrxn to be positive or negative.

•Ag+(aq) + Cl–(aq) → AgCl(s)

•H2O(s) → H2O(g)

•H2(g) + Cl2(g) → 2HCl(g)

•N2(g) + 3H2(g) → 2NH3(g)

•H2O(l) → H2O(s)

•2H2(g) + O2(g) → 2H2O(g)

•2NO2(g) → N2O4(g)

•CO2(g) → CO2(s)

•2Hg(l) + O2(g) → 2HgO (s)

Question is graded for accuracy so best answers please