Problem 55
What is the hybridization of phosphorus in the phosphonium ion \(\left(\mathrm{PH}_{4}^{+}\right) ?\)
Problem 56
Explain why (a) \(\mathrm{NH}_{3}\) is more basic than \(\mathrm{PH}_{3},\) (b) \(\mathrm{NH}_{3}\) has a higher boiling point than \(\mathrm{PH}_{3},\) (c) \(\mathrm{PCl}_{5}\) exists but \(\mathrm{NCl}_{5}\) does not, and (d) \(\mathrm{N}_{2}\) is more inert than \(\mathrm{P}_{4}\).
Problem 57
Describe one industrial and one laboratory preparation of \(\mathrm{O}_{2}\)
Problem 58
Give an account of the various kinds of oxides that exist, and illustrate each type by two examples.
Problem 59
Hydrogen peroxide can be prepared by treating barium peroxide with sulfuric acid. Write a balanced equation for this reaction.
Problem 60
Describe the Frasch process for obtaining sulfur.
Problem 61
Describe the contact process for the production of sulfuric acid.
Problem 64
In 2004 , about 48 million tons of sulfuric acid was produced in the United States. Calculate the amount of sulfur (in grams and moles) used to produce that amount of sulfuric acid.
Problem 65
The bad smell of water containing hydrogen sulfide can be removed by the action of chlorine. The reaction is: $$ \mathrm{H}_{2} \mathrm{~S}(a q)+\mathrm{Cl}_{2}(a q) \longrightarrow 2 \mathrm{HCl}(a q)+\mathrm{S}(s) $$ If the hydrogen sulfide content of contaminated water is 22 ppm by mass, calculate the amount of \(\mathrm{Cl}_{2}\) (in grams) required to remove all the \(\mathrm{H}_{2} \mathrm{~S}\) from \(2.0 \times 10^{2}\) gal of water. (1 gallon \(=3.785 \mathrm{~L}\) )
Problem 66
Calculate the amount of \(\mathrm{CaCO}_{3}\) (in grams) that would be required to react with \(50.6 \mathrm{~g}\) of \(\mathrm{SO}_{2}\) emitted by a power plant.
