A titration of 25.0 mL of 0.100 M triethylamine ((CH₃CH₂)₃N) was performed with 0.0500 M HCl. Given the following data calculate the pKa for triethylammonium ion.

The Clausius-Clapeyron equation and the Antoine equation. The vapor pressure of a liquid can be written in the empirical form known as the Antoine equation, ln (p / p ◦ ) = A1 − (A2 /(T + A3)) where A1, A2, and A3 are empirical constants determined from measurements, and T is the temperature in Kelvin.

(a) Starting with this equation, derive an equation for the enthalpy of vaporization as a function of temperature.

(b) For ethanol (l), A1 = 23.58, A2 = 3.67 × 103 , A3 = −46.702, and p ◦ = 1 Pa. Given that the standard pressure is 1 bar = 1.01325 × 105 Pa, what is the standard boiling temperature?

(c) Calculate ∆h at 298 K and at the standard boiling temperature.

The boiling point elevation constant for water is 0.51 degrees C/m. What is the boiling point of a solution made by dissolving 21.6g of a non-ionizing solute with a molar mass of 103.5 g/mol in 187g of water?

Motion of an election in a hydrogen atom corresponds to the potential energy U(r) = − e^2/(4πε0r) ,

4πε0 r which comes from the Coulomb attraction between the electron and the proton. Using the uncertainty

relation between the momentum of the electron, and its position, estimate the size of the hydrogen atom.

Consider the reaction:
SO2Cl2(g)⇌SO2(g)+Cl2(g) Kp=2.91×10³ at 298 K
In a reaction at equilibrium, the partial pressure of SO2 is 0.135 atm and that of Cl2 is 0.342 atm .

Part A

What is the partial pressure of SO2Cl2 in this mixture?

The Li2+ ion is hydrogenic and has a Lyman series at 740747 cm-1, 877924 cm-1, 925933 cm-1 and beyond. Show that the energy levels are of the form –hcR/n2 and find the value of R for this ion. Go on to predict the wavenumbers of the two longest wavelength transitions of the Balmer series of the ion and find the ionization energy of the ion.

Given the two reactions

H2S⇌HS−+H+,   K1 = 9.24×10⁻⁸, and

HS−⇌S2−+H+,   K2 = 1.15×10⁻¹⁹,

what is the equilibrium constant Kfinal for the following reaction?

S2−+2H+⇌H2S

Part B

Given the two reactions

PbCl2⇌Pb2++2Cl−,   K3 = 1.74×10⁻¹⁰, and

AgCl⇌Ag++Cl−,   K4 = 1.26×10⁻⁴,

what is the equilibrium constant Kfinal for the following reaction?

PbCl2+2Ag+⇌2AgCl+Pb2+

What is the vapor pressure of a solution prepared by adding 50.0 g of NaCl to 250. g of pure water at 25 ^oC? (Water has a vapor pressure of 0.036atm at 25 ^oC)

Explain why either greatly decreasing or increasing the percentage of oxygen in the atmosphere is dangerous.

1)What are amino acids? Amino group, carboxyl end, what is the side chain of an amino acid?

2)What are essential and non-essential amino acid.

3)Which are the essential amino acids?

4)Classify the amino acids based on polarity of the R group:

1. The preparation of nanoparticle solutions adds a reducing reagent, sodium borohydride, to an oxidizing agent, hydrogen peroxide. Is it concievable that these two reagents would react with each other?

2. Why is it important to force the regression line in the Beer's Law plot of absorbance vs. concentration to go through the origin? Would adding the point (0,0) to your data set have the same effect? Why or why not?

I'm in intro chem so pleasee give in simple terms. Don't go too into depth

Methane gas (CH4) is burned in a combustor with a given percentage of excess air. The pressure and temperature of both the air and fuel are 101 kPa and 298 K respectively. Assume that the mole fractions are 79% nitrogen and 21 % oxygen for air (use M=28.97 kg/kmol and R=0.287 kJ/kg-K) and that water is a vapor in the exhaust. Given the values below, determine the following:

--Given Values--

m_fuel (kg) = 100

Excess Air = 25%

a) Determine the air fuel ratio (kmol_air/kmol_fuel) Answer=11.905 +/- 7.9E-02

b) Determine the amount (kmol) of fuel burned. Answer=6.2344 +/- 4.2E-02

c) Determine the amount (kmol) of air used. Answer=74.219 +/- 4.9E-01

d) Determine the amount (kmol) of CO2 produce Answer=6.2344 +/- 4.2E-02

e) Determine the amount (kmol) of H2O produced. Answer=12.4688 +/- 8.3E-02

f) Determine the amount (kmol) of N2 produced. Answer=58.6332 +/- 3.9E-01

g) Determine the amount (kmol) of O2 produced Answer=3.1172 +/- 2.1E-02

h) Determine the Enthalpy (kJ) of the reactants. Answer=-466646 +/- 3.1E+03

i) Determine the adiabatic flame temperature (K). Answer=2015.16 +/- 1.3E+01

j) Determine the Enthalpy (kJ) of CO2 in the products Answer=-1877561 +/- 1.3E+04

k) Determine the Enthalpy (kJ) of H2O in the products. Answer=-2099174 +/- 1.4E+04

l) Determine the Enthalpy (kJ) of N2 in the products. Answer=3323766 +/- 2.2E+04

m) Determine the Enthalpy (kJ) of O2 in the products. Answer=186323 +/- 1.2E+03

A 2.700×10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL.

Part A

Calculate the molality of the salt solution.

Express your answer to four significant figures and include the appropriate units.

Part B

Calculate the mole fraction of salt in this solution.