K_p has the value 1.00x10^-5 for the equilibrium

CO2(g) + H2(g) <--> CO(g) + H2O(g)

at 25^oC and ΔS_o is -41.9 J/K (ΔH_o and ΔS_o do not change much with temperature). One mole of CO, 2 moles of H₂, and 3 moles of CO₂ are introduced into a 5-liter flask at 25^oC. Calculate

(a) ΔG_o at 25^oC,

(b) the equilibrium pressure,

(c) the moles of each species present at equilibrium,

(d) K_p at 100 0C. The mixture obeys the ideal equation of state.

Calculate the energy gap in J, kJ/mol, eV, and wavenumber (cm^-1) between the level n = 5 and n = 1 of an electron confined to a microscopic 1-D box of length 2.00 Angstroms.

  1- J
  2- kJ/mol
  3 -eV
  4- cm^-1

Determine the oxidation number (oxidation state) for the indicated element in each of the following compounds.

A: Ti in TiO2

B: Al in NaAlH4

C: C in C2O42?

D: N in N2H4

E: N in HNO2

F: Sn in SnCl3?

Would you expect the ligand substitution reactions of transition metal ions to be faster or slower than those of lanthanide ions and the pre-transition metal ions? Explain why.

For the following reaction KClO3---->KCl+1/2 O2 assign oxidation states to each element on each side of the equation...reactants and products. Which element is oxidized? Which element is reduced? Reactants for K, Cl, and O please. Cl is not 5 to -1. i know the rest just need to know it for Cl

Given that the vapor pressure of water is 17.54 Torr at 20 degrees celcius, calculate the vapor pressure lowering of aqueous solutions that are 1.70 m in (a) sucrose C12H22O11 and (b) Aluminum Chloride. Assume 100% dissosiation for electrolytes.

The ΔHvap of a certain compound is 22.01 kJ·mol–1 and its ΔSvap is 54.70 J·mol–1·K–1. What is the boiling point of this compound?

draw the Lewis dot diagram of the following molecules:
a. BBr3
b. IF2-
c. SiO2
d. SOF2

Calculate the pH of a 0.0164 M solution of arginine hydrochloride (arginine·HCl, H2Arg ). Arginine has pKa values of 1.823 (pKa1), 8.991 (pKa2), and 12.01 (pKa3).

Calculate the concentration of each species of arginine in the solution.

H3Arg2+

H2Arg+

HArg

Arg-

part 1: It is recommended that drinking water contain 1.6 ppm fluoride (F^?) for prevention of tooth decay. Consider a reservoir with a diameter of 4.50???10² m and a depth of 14.3 m. (The volume is ?r²h, where r is the radius and h is the height.) How many grams of F^? should be added to give 1.6 ppm?

part 2: Fluoride is provided by hydrogen hexafluorosilicate, H₂SiF₆. How many grams of H₂SiF₆ contain this much F^??

PH experiment:

What is one real-world or practical application for this experiment or portion of this experiment?

Define the following: abscissa, acid, base, endpoint, equivalence point, neutralization, pH, pKa, mono- protic acid, polyprotic acid, ordinate, strong acid, strong base, and weak acid.

Draw the structure of each of the acids in Table 1.

Produce data tables for each of your runs. Leave room in your notebook for lots of data. Record the actual volume of titrant and solution pH as you conduct the experiment.

Identify all potentially hazardous steps in your procedure. In your own words, explain what safety precautions should be taken and why.

Consider the titration of 0.050 M HCl with 0.050 M NaOH. Calculate the pH: (a) of the pure HCl solution; (b) of 25.00 mL acid plus 12.50 mL base; (c) at the equivalence point; and (d) of 25.00 mL acid and 37.50 mL base.

Consider the titration of 0.050 M NaOH with 0.050 M HCl. Calculate the pH: (a) of the pure NaOH solution; (b) of 25.00 mL base plus 12.50 mL acid; (c) at the equivalence point; and (d) of 25.00 mL base and 37.50 mL acid.

In one experiment, an unknown acid was titrated with NaOH. The pH at the equivalence point was 7.75. Was the unknown acid strong or weak? Explain. Hint: The pH of pure water at room temperature is 7.

A 25.0 mL sample of 0.175 M HClO(aq) is titrated with 0.100 M NaOH(aq). What is the pH of a solution after the addition of 25.0 mL of NaOH? (K_aof HClO = 3.5

Stoichiometry Problems for Reaction in Aqueous Solutions

-.The quantity of Cl^– in a municipal water supply is determined by titrating the sample with Ag⁺. The precipitation reaction taking place during the titration is Ag(aq) + Cl(aq) ->AgCl(s)

The end point in this type of titration is marked by a change in color of a special type of indicator. (a) How many grams of chloride ion are in a sample of the water if 20.2 mL of 0.200 M Ag⁺ is needed to react with all the chloride in the sample? (b) If the sample has a mass of 15.0 g, what percentage of Cl^– does it contain?

-.A mysterious white powder is found at a crime scene. A simple chemical analysis concludes that the powder is a mixture of sugar and morphine (C1₇H₁₉NO₃), a weak base similar to ammonia. The crime lab takes 10.00 g of the mysterious white powder, dissolves it in 100.00 mL water, and titrates it to the equivalence point with 2.84 mL of a standard 0.100 M HCl solution. What is the percentage of morphine in the white powder?

-.A sample of an iron ore is dissolved in acid, and the iron is converted to Fe²⁺. The sample is then titrated with 57.20 mL of 0.05240 M MnO₄^– solution. The oxidation-reduction reaction that occurs during titration is

MnO4(aq) + Fe^2+(aq) +8H(aq) -> Mn^2+(aq) +5Fe^3+(aq) + 4H2O(l)

How many moles of MnO₄^– were added to the solution? (b) How many moles of Fe²⁺ were in the sample? (c) How many grams of iron were in the sample? (d) If the sample had a mass of 2.8890 g, what is the percentage of iron in the sample?

-A sample of 70.5 mg of potassium phosphate is added to 25.0 mL of 0.050 M silver nitrate, resulting in the formation of a precipitate. (a) Write the molecular equation for the reaction. (b) What is the limiting reactant in the reaction? (c) Calculate the theoretical yield, in grams, of the precipitate that forms.

Exercise 13.97

The kinetics of the following second-order reaction were studied as a function of temperature:
C2H5Br(aq)+OH?(aq)?C2H5OH(l)+Br?(aq)

Calculate the number of pounds of CO2 released into the atmosphere when a 25.0-gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18, and that the density of gasoline is 0.692 g·mL–1 (this assumption ignores additives). Also assume complete combustion.