Problem 30
Ground water sometimes contains traces of hydrogen sulfide, which has the odor of rotten eggs. Chlorine gas is used to purify the water for drinking. The resulting sulfur reacts with fluorine gas to give sulfur hexafluoride. The reactions are as follows: $$\begin{aligned}8 \mathrm{H}_{2} \mathrm{~S}(a q)+8 \mathrm{Cl}_{2}(g) & \longrightarrow 16 \mathrm{HCl}(a q)+\mathrm{S}_{8}(s) \\\\\mathrm{S}_{8}(s)+24 \mathrm{~F}_{2}(g) & \longrightarrow 8 \mathrm{SF}_{6}(g)\end{aligned} $$ Starting with \(0.950 \mathrm{~L}\) of \(\mathrm{Cl}_{2}\) (STP) and excess fluorine gas, calculate: (a) the mass of sulfur hexafluoride produced (b) the volume of sulfur hexafluoride produced at STP (c) the volume of aqueous \(0.0265 \mathrm{M} \mathrm{H}_{2} \mathrm{~S}\) that reacted
Problem 31
Sulfuric acid is the single most important industrial chemical. About 40 million tons are manufactured each year. Elemental sulfur is converted to sulfuric acid by the Contact Process as follows: $$\begin{array}{c}S(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g) \\\2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(l) \stackrel{\mathrm{V}_{2}\mathrm{O}_{3}}{\longrightarrow} 2 \mathrm{SO}_{3}(g) \\\\\mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(g)\end{array}$$ Starting with \(1.00 \mathrm{~kg}\) of sulfur and excess oxygen gas, calculate: (a) the mass of sulfur trioxide produced (b) the STP volume of sulfur trioxide produced (c) the mass of sulfuric acid produced assuming a \(55.0 \%\) process yield
Problem 33
. Steering rockets on the space shuttle are powered by the reaction of hydrazine, \(\mathrm{N}_{2} \mathrm{H}_{4}\), and dinitrogen tetraoxide, \(\mathrm{N}_{2} \mathrm{O}_{4}\) The reactions for making hydrazine and the reaction with dinitrogen tetraoxide are as follows: \(2 \mathrm{NH}_{3}(a q)+\mathrm{NaOCl}(a q) \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}(a q)+\mathrm{NaCl}(a q)+\mathrm{H}_{2} \mathrm{O}(I)\) $$2 \mathrm{~N}_{2} \mathrm{H}_{4}(l)+\mathrm{N}_{2} \mathrm{O}_{4}(l) \longrightarrow 3 \mathrm{~N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)$$ Starting with \(50.0 \mathrm{~mL}\) of \(6.00 \mathrm{M}\) ammonia and excess other reactants, calculate: (a) the mass of nitrogen gas produced (b) the volume of nitrogen gas produced at STP (c) the mass of water produced
Problem 34
Hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2}\), is prepared industrially from the reaction of oxygen and isopropyl alcohol, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}\). Hydrogen peroxide reacts explosively with hydrazine, \(\mathrm{N}_{2} \mathrm{H}_{4},\) and is used as a rocket fuel. The reactions for manufacturing hydrazine and the rocket explosion are as follows. $$\begin{array}{l}\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}_{2}(l)+\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}(l) \\\2 \mathrm{H}_{2} \mathrm{O}_{2}(l)+\mathrm{N}_{2} \mathrm{H}_{4}(l) \longrightarrow \mathrm{N}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)\end{array}$$ Starting with \(50.0 \mathrm{~mL}\) of isopropyl alcohol \((d=0.786 \mathrm{~g} / \mathrm{mL})\) and excess other reactants, calculate: (a) the mass of nitrogen gas produced (b) the volume of nitrogen gas produced at STP (c) the mass of water produced
Problem 35
Calculate the mass of nitrogen dioxide gas occupying a volume of \(2.50 \mathrm{~L}\) at \(35{ }^{\circ} \mathrm{C}\) and \(0.974 \mathrm{~atm}\) pressure.
Problem 36
Calculate the molar mass of an unknown gas if an experiment yielded a value of \(1.45 \mathrm{~g} / \mathrm{L}\) at \(100{ }^{\circ} \mathrm{C}\) and \(0.989 \mathrm{~atm} .\)
Problem 37
A 34.5 -g sample of calcium chloride is dissolved in \(500.0 \mathrm{~mL}\) of solution. Find the molar concentration of the calcium ions and chloride ions in solution. (Assume the salt is \(100 \%\) ionized.
Problem 38
What is the molar chloride ion concentration that results from mixing \(100.0 \mathrm{~mL}\) of \(0.156 \mathrm{M}\) lithium chloride and \(150.0 \mathrm{~mL}\) of \(0.225 \mathrm{M}\) barium chloride?
Problem 39
How many milliliters of \(0.100 \mathrm{M}\) hydrochloric acid react with excess zinc metal in order to collect \(50.0 \mathrm{~mL}\) of hydrogen gas over water at STP?
Problem 40
What volume of \(0.150 \mathrm{M}\) hydrochloric acid reacts with excess lead(II) nitrate solution in order to yield \(1.88 \mathrm{~g}\) of lead(II) chloride precipitate?
