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?

20#15

Given the following half-reactions and associated standard reduction potentials:
AuBr−4(aq)+3e−→Au(s)+4Br−(aq)
E∘red=−0.858V
Eu3+(aq)+e−→Eu2+(aq)
E∘red=−0.43V
IO−(aq)+H2O(l)+2e−→I−(aq)+2OH−(aq)
E∘red=+0.49V
Sn2+(aq)+2e−→Sn(s)
E∘red=−0.14V

a) Write the cell reaction for the combination of these half-cell reactions that leads to the largest positive cell emf.

b) Calculate the value of this emf.

E∘max = _____ V

c) Write the cell reaction for the combination of half-cell reactions that leads to the smallest positive cell emf.

d) Calculate the value of this emf.

E∘min = _____ V

What is the pH at the equivalence point 10.0 mL of 1.00 M NH₃ (K_b = 1.8 x 10^-5) is titrated against 2.00 M HCl?

At 1 atm, how much energy is required to heat 73.0 g of H2O(s) at –22.0 °C to H2O(g) at 121.0 °C?

1. What is the principal use of calcium proprionate (the calcium salt of propionic acid) based from The Merck Index?

2. What is the result of treating calcium chloride with oxalic acid?

3. Explain why oxalic acid can be a deadly poison?

How many unique 1 H NMR signals exist in the spectrum of the following compound: 1,3-dibromobenzene?

Cyanide recovered from the refining of gold ore
can be determined indirectly by EDTA titration. A known
excess of Ni2 is added to the cyanide to form tetracyanonickelate(
II):
4CN + Ni ---> Ni(CN)4
When the excess Ni2 is titrated with standard EDTA,
Ni(CN)4 does not react. In a cyanide analysis, 12.7 mL of
cyanide solution were treated with 25.0 mL of standard solution
containing excess Ni to form tetracyanonickelate. The excess
Ni required 10.1 mL of 0.013 0 M EDTA for complete
reaction. In a separate experiment, 39.3 mL of 0.013 0 M EDTA
were required to react with 30.0 mL of the standard Ni
solution. Calculate the molarity of CN in the 12.7-mL sample
of unknown.

1. Listed below are the atomic weight, density, and atomic radius for three hypothetical alloys. For each determine its crystal structure and then justify your determination.

Alloy // Atomic weight (g/mol) // Density (g/ cm^3) // Atomic Radius (nm)

A // 43.1 // 6.4 // 0.122

B   // 184.4 // 12.3 // 0.146

C // 91.6 // 9.6 // 0.137