please answer the following questions

1- Assuming the partial pressure of oxygen gas is that of atmospheric oxygen 0.021 atm, rather than the 1.00 atm assumed in the derivation of Equation down, derive an equation describing the oxidizing pE limit of water as a function of pH.

equation is PE=20.75-PH

2- Using the equation derived in Problem 1 and Excel, plot logPO2 as a function of pE at pH 7.00.

3-Calculate the values of [Fe3+], pE and pH at the point in Figure 4.4 where Fe2+ is at a concentration of 1.00 x 10-5M, and Fe(OH)2 and Fe(OH)3 are in equilibrium.

In a factory in which metal parts are degreased with organic solvents, the intern breaks a bottle containing a mixture of 5 liters of tetrachloroethylene (PER, MW = 166 g/mol, ρ = 1.62 g/cm3 , Pv = 18 mm Hg) and 10 liters of trichloroethene (TCE, MW = 131 g/mol, ρ = 1.46 g/cm3 , Pv = 54 mm Hg) in a closed room at 20oC. The room has a total volume of 50 m3 . Assume PER and TCE form an ideal mixture in the liquid phase.

a. What is the composition (in mole fractions) of the liquid mixture in the bottle?

b. What are the equilibrium concentrations of PER and TCE in the air of the room in mg/L? Note: Make sure to use Raoult’s Law. [PER] = 49.9 mg/L

c. What is the composition (in mole fractions) of the remaining liquid on the floor after equilibrium? XPER = 0.790

Determine the pH of each of the following solutions. 7.00×10−2 M HNO3, 0.160 M HNO2, 2.10×10−2 M KOH, 0.245 M CH3NH3I, 0.318 M KC6H5O.

I am not getting the correst answer to these.... please help and show work. Thank you

Assume an atom has K, L, and M electrons and the energies for K, L, and M shells are -5000, -500, and -50 eV. Please give all possible energies of Auger electrons and characteristic X-rays.

When 14.3 g of an organic compound known to be 55.81% C, 7.02% H, and 37.17% O by mass is dissolved in 883.2 g of cyclohexane, the freezing point is 3.98 °C. The normal freezing point of cyclohexane is 6.59 °C. What is the molecular formula for the organic compound? Assume that the organic compound is a molecular solid and does not ionize in water. Kf values for various solvents are given here.

A 5.50 −g sample of a weak acid with Ka=1.3×10−4 was combined with 4.90 mL of 6.20 M NaOH and the resulting solution was diluted to 750 mL. The measured pH of the solution was 4.35.

What is the molar mass of the weak acid?

In a particular redox reaction, MnO2 is oxidized to MnO4– and Fe3 is reduced to Fe2 . Complete and balance the equation for this reaction in acidic solution. Phases are optional.

ethanol(C2H5OH)and gasoline(assumed to be octane,C8H18) are both used as automobile fuel.if gasoline is selling for $4.50/gal,what would the price of ethanol have to be in order to provide the same amount of heat per dollar?The density and ?Hf of octane are 0.7025g/ml and -249.9kJ/mol,respectively and of ethanol are 0.7894g/ml and -277.0 kJ/mol,respectively(1 gal =3.785L)

As with amino acids and peptides, various classes of saponifiable lipids can often be separated by electrophoresis.

a. Could a mixture of phosphatidylcholine and phosphatidylserine be separated by electrophoresis at pH 7? Explain.

b. At what pH range (from pH 0-14) would it be possible to separate a mixture of phosphatidylcholine and phosphatidylethanolamine by electrophoresis? Explain.

Standardized NaOH solutions are typically restandardized if left unused for more than a week or two. The main concern is exposure to the atmosphere (thus it is important to seal the bottle well each time, and not leave it open during a lab period). Why is exposure to the atmosphere a concern (be specific)?

If a titration net volume should be 20.00 mL and a student accidentally goes one drop past this endpoint (~0.05 mL), what will the percent error in this titration be?

If the incorrect titration net volume described in question 3 is used to standardize an NaOH solution, will the calculated [NaOH] be higher or lower than the true value of that solution’s concentration? Explain briefly.

Calculating equilibrium concentrations when the net reaction proceeds forward

Consider mixture B, which will cause the net reaction to proceed forward.

Concentration (M)initial:change:equilibrium:[XY]0.500−x0.500−xnet→⇌[X]0.100+x0.100+x+[Y]0.100+x0.100+x

The change in concentration, x, is negative for the reactants because they are consumed and positive for the products because they are produced.

Part B

Based on a Kc value of 0.260 and the given data table, what are the equilibrium concentrations of  XY, X, and Y, respectively?

Express the molar concentrations numerically.

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Calculating equilibrium concentrations when the net reaction proceeds in reverse

Consider mixture C, which will cause the net reaction to proceed in reverse.

Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x

The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.

Part C

Based on a Kc value of 0.260 and the data table given, what are the equilibrium concentrations of  XY, X, and Y, respectively?

Express the molar concentrations numerically.

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Find the pH and [SO42-] of a 0.0050 M sulfuric acid solution

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128.16 g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m.

If 0.291 g of Mg is reacted with excess HCl and 301 mL of H2 gas is collected in a gas collection tube over water at 25oC and 1 atm of pressure. What is the experimental partial pressure of water vapor in the hydrogen gas?