Ethyl alcohol has a vapor pressure of 20.0mm Hg at 8.0 ° C and a normal boiling point of 78.4 ° C.Estimate the vapor pressure at 45 ° C using (a) the Antoine equation; (b) the Clausius – Clapeyronequation and the two given data points; and (c) linear interpolation between the two given points.Taking the fi rst estimate to be correct, calculate the percentage error associated with the secondand third estimates.

A gas cylinder contains 2.30 mol He, 1.35 mol Ne, and 1.75 mol Ar. If the total pressure in the cylinder is 2290 mmHg, what is the partial pressure of each of the components? Assume constant temperature.

P(He) = ?

P(Ne) = ?

P (Ar) = ?

A 10.00 mL sample of 0.150 M sodium azide, NaN3, a weak base, is titrated with 0.100 M HCl. Calculate the pH after the addition of the following volumes of acid:

(a) 0.00 mL; (b) 9.00 mL; (c) 15.00 mL; (d) 27.00 mL

The Ka of HN3 is 1.9 x 10–5

Assuming you use 2.5 g vanillin and 5.0 mL of a 3.42 M NaBH4 solution, what is the theoretical yield of vanillyl alcohol in moles? in grams?

How many mL of 12 M HCl will be needed to prepare 500 ml of 1.2 ppm HCl solution? What is the pH of this 1.2 ppm HCl solution? Using the right significant figures. MW of HCl=36.5g/mol

I already found the first answer which is 1.4 x 10^-3 mL

How do I find the pH? I know the formula is -log [H+], but I have no information for it?

A 0.5072 g solid sample containing a mixture of LaCl3 (molar mass = 245.26 g/mol) and Ce(NO3)3 (molar mass = 326.13 g/mol) was dissolved in water. The solution was titrated with KIO3, producing the precipitates La(IO3)3(s) and Ce(IO3)3(s). For the complete titration of both La3 and Ce3 , 44.01 mL of 0.1289 M KIO3 was required. Calculate the mass fraction of La and Ce in the sample.

calculate the molar mass? calculate the value of the freezing point depression constant, Kf, for acetic acid.

What mass of propane will occupy the same volume as 0.057 mol of butane at 1.00 atm and 298 K?

My answer: 0.057m x 0.0821Latm/Kmol x 298K = 1.4 L

Suppose a student performed a similar experiment using pentane and hexane as his gases.

Pentane Hexane

Molar Mass (g/mol) 72.15 86.18

Mass (g) 0.541 0.646

Given the data in the figure above, which gas will occupy a larger volume at STP? (This is the question I am stuck on.)

PART A: 137 nmol of an antibody that binds strongly to the antigen protein G is covalently bound to the support of an affinity column with a void volume of 1.95 mL. The association equilibrium constant (K_A) for the binding of protein G to the antibody is 5.19 × 10⁸ M^-1 at pH 7.2. Calculate the retention factor for protein G on this column at pH 7.2. k=?

PART B: At pH 7.2 and a flow rate of 1.00 mL/min, how many minutes would it take protein G to elute from this column? t_r=? min

PART C: If a pH 3.5 elution buffer is applied to the column, protein G elutes at 3.12 min using a flow rate of 1.00 mL/min. Under these conditions, what is the association equilibrium constant between protein G and the antibody? K_A=? M^-1

6. Calculate the concentration of H3O + or HO- , as indicated, when each of the strong acids below is dissolved in the indicated total volume of water.

a) 1.5 moles of HBr is dissolved in 4.0 L of H2O. [H3O + ] = _____________ moles/L

b) 1.0 mole of Ba(OH)2 is dissolved in 10.0 L of H2O. [HO-] = ______________ moles/L

Upon heating, potassium chlorate decomposes to potassium chloride and oxygen gas. The oxygen gas is collected over water at 14.0 °C in a 500.-mL container. If the total pressure is 766 torr,

How many mol of oxygen gas is in the container?
What is the mole fraction of oxygen gas in the container?.
(Mole fraction = mole of substance of interest / mole of the system)

How many grams of potassium chlorate is decomposed?

A 12.0 % NaCl_(aq) has a density of 1.05 g/mL. What is the molality of the solution?

A 2.55 L sample of gas at STP contains hydrogen and oxygen gases. The mole fraction of hydrogen is 0.60. When the sample is combusted to form water, calculate the mass of water formed, assuming complete reaction.

A heater burns normal octane (n-C₈H₁₈) using 20.0 percent excess air. Combustion is complete. The flue gas leaves the stack at a pressure of 100 kPa and a temperature of 160⁰C.

a) Calculate the complete flue gas analysis.

b) What is the volume of the flue gas in cubic meter per kg mol of n-octane?