The Elements in Nature and Industry

Based on a concentration of $\mathbf{0}\mathbf{.}\mathbf{065}\mathbf{ }{\mathbf{gBr}}^{\mathbf{-}}\mathbf{/}\mathbf{L}$  the ocean is estimated to have $\mathbf{\text{\$ 391,000,000}}$ of  ${\mathbf{\text{Br}}}_{\mathbf{2}}\mathbf{/}{\mathbf{\text{mi}}}^{\mathbf{3}}$ at recent prices.

a) What is the price per gram of  ${\mathbf{\text{Br}}}_{\mathbf{\text{2}}}\mathbf{\text{?}}$

b) Find the mass (in g) of ${\mathbf{\text{AgNO}}}_{\mathbf{\text{3}}}$ needed to precipitate $\mathbf{\text{90.0\% }}$ of the  in of ocean water.

c) Use Appendix C to find how low $\left[{\text{Cl}}^{\text{ - }}\right]$ must be to prevent the unwanted precipitation of  

d) Given a  $\left[{\text{Cl}}^{\text{ - }}\right]$of about 0.3M, is precipitation with silver ion a practical way to obtain bromine from the ocean? Explain.

: Many metal oxides are converted to the free metal by reduction with other elements, such as $\mathbf{\text{C}}$ or $\mathbf{\text{Si}}$. For each of the following reactions, calculate the temperature at which the reduction occurs spontaneously:

(a) ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}\mathbf{\text{(s)}}\mathbf{\to }{\mathbf{\text{Mn(s) + O}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$

(b) ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}\mathbf{\text{(s) + 2C(graphite)}}\mathbf{\to }\mathbf{\text{Mn(s) + 2CO(g)}}$

(c) ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}\mathbf{\text{(s) + C(graphite)}}\mathbf{\to }{\mathbf{\text{Mn(s) + CO}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$

(d) ${\mathbf{\text{MnO}}}_{\mathbf{\text{2}}}\mathbf{\text{(s) + Si(s)}}\mathbf{\to }{\mathbf{\text{Mn(s) + SiO}}}_{\mathbf{\text{2}}}\mathbf{\text{(s)}}$

Diagrams of environmental cycles are simplified to omit minor contributors. For example, the production of lime from limestone is not shown in the cycle for carbon (Figure , ). Which labelled category in the figure includes this process? Name two other processes that contribute to this category.

The following steps are unbalanced half-reactions involved in the nitrogen cycle. Balance each half-reaction to show the number of electrons lost or gained, and state whether it is an oxidation or a reduction (all occur in acidic conditions):

  ${\mathbf{\text{(a) N}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}\mathbf{\to }\mathbf{\text{NO(g)}}$

${\mathbf{\text{(b)N}}}_{\mathbf{\text{2}}}\mathbf{\text{O(g)}}\mathbf{\to }{\mathbf{\text{NO}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$

${\mathbf{\text{(c)NH}}}_{\mathbf{\text{3}}}\mathbf{\text{(aq)}}\mathbf{\to }{\mathbf{\text{NO}}}_{\mathbf{\text{2}}}^{\mathbf{\text{-}}}\mathbf{\text{(aq)}}$

${{\mathbf{\text{(d)NO}}}_{\mathbf{\text{3}}}}^{\mathbf{\text{-}}}\mathbf{\text{(aq)}}\mathbf{\to }{{\mathbf{\text{NO}}}_{\mathbf{\text{2}}}}^{\mathbf{\text{-}}}\mathbf{\text{(aq)}}$

${\mathbf{\text{(e)N}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}\mathbf{\to }{\mathbf{\text{NO}}}_{\mathbf{\text{3}}}^{\mathbf{\text{-}}}\mathbf{\text{(aq)}}$

Nitrogen fixation requires a great deal of energy because the   bond is strong. 

(a) How do the processes of atmospheric and industrial fixation reflect this energy requirement? 

(b) How do the thermodynamics of the two processes differ? (Hint: Examine the respective heats of formation.) 

(c) In view of the mild conditions for biological fixation, what must be the source of the “great deal of energy”? 

(d) What would be the most obvious environmental result of a low activation energy for   fixation?

Question: (a) Which region of Earth’s crust is not involved in the phosphorus cycle? (b) Name two roles organisms play in the cycle.

Describe three pathways for the utilization of atmospheric nitrogen. Is human activity a significant factor? Explain.

Carbon dioxide enters the atmosphere by natural processes and from human activity. Why is the latter a cause of concern?

Define the term fixation. Name two elements that undergo environmental fixation. What natural forms of them are fixed?

Use atomic and molecular properties to explain why life is based on carbon, rather than some other element such as silicon.

Describe two ways in which the biosphere has influenced the composition of Earth’s crust.

Aluminium is widely distributed throughout the world in the form of aluminosilicates. What property of these minerals prevents them from being a source of aluminium?

What material is the source for commercial production of each of the following elements: 

(a) aluminium;

 (b) nitrogen;

 (c) chlorine; 

(d) calcium;

 (e) sodium?

Metallic elements can be recovered from ores that are oxides, carbonates, halides, or sulphides. Give an example of each type.

How does the position of a metal in the periodic table relate to whether it occurs primarily as an oxide or as a sulfide?

The location of elements in the regions of Earth has enormous practical importance.

 (a) Define the term differentiation, and explain which physical property of a substance is primarily responsible for this process. 

(b) What are the four most abundant elements in the crust?

(c) Which element is abundant in the crust and mantle but not the core?

Hydrogen is by far the most abundant element cosmically. In interstellar space, it exists mainly as${\mathbf{H}}_{\mathbf{2}}$In contrast, on Earth, it exists very rarely ${\mathbf{H}}_{\mathbf{2}}$ as and is ninth in abundance in the crust. Why is hydrogen so abundant in the universe? Why is hydrogen so rare as a diatomic gas in Earth’s atmosphere?

$\mathbf{N}\mathbf{-}\mathbf{N}$ bonds?

(a) In the industrial production of iron, what is the reducing substance loaded into the blast furnace? 

(b) In addition to furnishing the reducing power, what other function does this substance serve? 

(c) What is the formula of the active reducing agent in the process? 

(d) Write equations for the stepwise reduction of ${\mathbf{Fe}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{3}}$ to iron in the furnace.

One of the substances loaded into a blast furnace is limestone, which produces lime in the furnace. 

(a) Give the chemical equation for the reaction forming lime. 

(b) Explain the purpose of lime in the furnace. The term flux is often used as a label for a substance acting as the lime does. What is the derivation of this word, and how does it relate to the function of the lime?

(c) Write a chemical equation describing the action of lime flux.

The last step in the Dow process for the production of magnesium metal involves electrolysis of molten ${\mathbf{\text{MgCl}}}_{\mathbf{\text{2}}}$.

(a) Why isn't the electrolysis carried out with aqueous ${\mathbf{\text{MgCl}}}_{\mathbf{\text{2}}}$? What are the products of this aqueous electrolysis?

(b) Do the high temperatures required to melt ${\mathbf{\text{MgCl}}}_{\mathbf{\text{2}}}$ favor products or reactants? (Hint: Consider the ${{\mathbf{\Delta H}}_{\mathbf{f}}}^{\mathbf{0}}$ of ${\mathbf{\text{MgCl}}}_{\mathbf{\text{2}}}$.)

lodine is the only halogen that occurs in a positive oxidation state, in  impurities within Chile saltpeter, ${\mathbf{\text{NaNO}}}_{\mathbf{\text{3}}}$.

(a) Is this mode of occurrence consistent with iodine's location in the periodic table? Explain.

(b) In the production of ${\mathbf{\text{I}}}_{\mathbf{\text{2}}}\mathbf{\text{,I}}{{\mathbf{\text{O}}}_{\mathbf{\text{3}}}}^{\mathbf{\text{ - }}}$reacts with $\mathbf{\text{HS}}{{\mathbf{\text{O}}}_{\mathbf{\text{3}}}}^{\mathbf{\text{ - }}}$:

$\mathbf{\text{I}}{{\mathbf{\text{O}}}_{\mathbf{\text{3}}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq) + HS}}{{\mathbf{\text{O}}}_{\mathbf{\text{3}}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq)}}\mathbf{\to }\mathbf{\text{HS}}{{\mathbf{\text{O}}}_{\mathbf{\text{4}}}}^{\mathbf{\text{ - }}}\mathbf{\text{(aq) + S}}{{\mathbf{\text{O}}}_{\mathbf{\text{4}}}}^{\mathbf{\text{2 - }}}{\mathbf{\text{(aq) + H}}}_{\mathbf{\text{2}}}{\mathbf{\text{O(I) + I}}}_{\mathbf{\text{2}}}\mathbf{\text{(s)}}\mathbf{ }$ 

[unbalanced] Identify the oxidizing and reducing agents.

(c) If $\mathbf{0}\mathbf{.}\mathbf{78}\mathbf{ }\mathbf{mol}\mathbf{\%}$ of an ${\mathbf{\text{NaNO}}}_{\mathbf{\text{3}}}$ deposit is  ${\mathbf{\text{NaIO}}}_{\mathbf{\text{3}}}$, how much ${\mathbf{\text{I}}}_{\mathbf{\text{2}}}$  (in g) can be obtained from  $\mathbf{\text{1.000}}$ton (2000. Ib) of the deposit?

Selenium is prepared by the reaction of ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}{\mathbf{\text{SeO}}}_{\mathbf{\text{3}}}$ with gaseous ${\mathbf{\text{SO}}}_{\mathbf{\text{2}}}$.

(a) What redox process does the sulfur dioxide undergo? What is the oxidation state of sulfur in the product? 

(b) Given that the reaction occurs in acidic aqueous solution, what is the formula of the sulfur-containing species? 

(c) Write the balanced redox equation for the process.

${\mathbf{\text{F}}}_{\mathbf{\text{2}}}{\mathbf{\text{ and Cl}}}_{\mathbf{\text{2}}}$ are produced by electrolytic oxidation, whereas ${\mathbf{\text{Br}}}_{\mathbf{\text{2}}}{\mathbf{\text{ and l}}}_{\mathbf{\text{2}}}$ are produced by chemical oxidation of the halide ions in a concentrated aqueous solution (brine) by a more electronegative halogen. Give two reasons why ${\mathbf{\text{Cl}}}_{\mathbf{\text{2}}}$ isn't prepared this way.

Define: (a) ore; (b) mineral; (c) gangue; (d) brine.

Define: (a) roasting; (b) smelting; (c) flotation; (d) refining.

Phosphorus is one of the impurities present in pig iron that is removed in the basic-oxygen process. Assuming phosphorus is present as P atoms, write equations for its oxidation and subsequent reaction in the basic slag.

What factors determine which reducing agent is selected for producing a specific metal?

Use atomic properties to explain the reduction of a less active metal by a more active one: 

(a) in aqueous solution; 

(b) in the molten state. Give a specific example of each process.

Which group of elements gives each of the following alloys: (a) brass; (b) stainless steel; (c) bronze; (d) sterling silver?

$\begin{array}{l}\mathbf{\text{1.Cu,Ag}}\\ \mathbf{\text{2.Cu,Sn,Zn}}\\ \mathbf{\text{3.Ag,Au}}\\ \mathbf{\text{4.Fe,Cr,Ni}}\\ \mathbf{\text{5.Fe,V}}\\ \mathbf{\text{6.Cu,Zn}}\end{array}$

How are each of the following involved in iron metallurgy?

What are the distinguishing features of each extraction process:

 pyrometallurgy, electrometallurgy, and hydrometallurgy? Explain briefly how the types of metallurgy are used in the production of

(a) Fe; 

(b) Na; 

(c) Au; 

(d) Al.

Why is cryolite used in the electrolysis of aluminum oxide?

(a) What is a kinetic isotope effect? 

(b) Do compounds of hydrogen exhibit a relatively large or small kinetic isotope effect? Explain. 

(c) Carbon compounds also exhibit a kinetic isotope effect. How do you expect it to compare in magnitude with that for hydrogen compounds? Why?

How is Le Châtelier's principle involved in the production of elemental potassium?

Elemental Li and $\mathbf{Na}$  are prepared by electrolysis of a molten salt, whereas $\mathbf{\text{K,Rb}}$ , and $\mathbf{\text{Cs}}$  are prepared by chemical reduction. 

(a) In general terms, explain why the alkali metals cannot be prepared by electrolysis of their aqueous salt solutions. 

(b) Use ionization energies (see the Family Portraits, pp. 572 and 576 ) to explain why Calcium should not be able to isolate $\mathbf{\text{Rb}}$  from molten  $\mathbf{\text{RbX(X=}}$ halide). 

(c) Use physical properties to explain why Calcium is used to isolate Rb from molten RbX. 

(d) Can Ca be used to isolate Cs from molten CsX? Explain.

A Downs cell operating at $\mathbf{\text{77.0 A}}$  produces  $\mathbf{\text{31.0 kg}}$ of  .

(a) What volume of  ${\mathbf{\text{Cl}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$ is produced at $\mathbf{\text{1.0}}$  atm and  ${\mathbf{\text{540.}}}^{\mathbf{\text{°}}}\mathbf{\text{C}}$?

(b) How many coulombs were passed through the cell?

(c) How long did the cell operate?

The use of silica to form slag in the production of phosphorus from phosphate rock was introduced by Robert Boyle more than years ago. When fluorapatite $\mathbf{[}{\mathbf{Ca}}_{\mathbf{5}}{\mathbf{\left(}{\mathbf{PO}}_{\mathbf{4}}\mathbf{\right)}}_{\mathbf{3}}\mathbf{ }\mathbf{F}\mathbf{]}$ is used in phosphorus production, most of the fluorine atoms appear in the slag, but some end up in toxic and corrosive ${\mathbf{SiF}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}$.

(a) If   by mass of the fluorine in $\mathbf{100}\mathbf{.}\mathbf{kg}$ of ${\mathbf{Ca}}_{\mathbf{5}}{\mathbf{\left(}{\mathbf{PO}}_{\mathbf{4}}\mathbf{\right)}}_{\mathbf{3}}\mathbf{F}$ forms ${\mathbf{SiF}}_{\mathbf{4}}$, what volume of this gas is collected at $\mathbf{1}\mathbf{.}\mathbf{00}\mathbf{ }\mathbf{atm}$and the industrial furnace temperature of $\mathbf{1450}\mathbf{°}\mathbf{C}$?

(b) In some facilities, the ${\mathbf{SiF}}_{\mathbf{4}}$ is used to produce sodium hexafluoro silicate $\left({\mathrm{Na}}_2{\mathrm{SiF}}_6\right)$which is sold for water fluoridation:

$\mathbf{2}{\mathbf{SiF}}_{\mathbf{4}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{N}{\mathbf{a}}_{\mathbf{2}}{\mathbf{CO}}_{\mathbf{3}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}\mathbf{\left(}\mathbf{l}\mathbf{\right)}\mathbf{\to }{\mathbf{Na}}_{\mathbf{2}}{\mathbf{SiF}}_{\mathbf{6}}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}\mathbf{+}\mathbf{Si}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}\mathbf{+}\mathbf{C}{\mathbf{O}}_{\mathbf{2}}\mathbf{\left(}\mathbf{g}\mathbf{\right)}\mathbf{+}\mathbf{2}\mathbf{HF}\mathbf{\left(}\mathbf{aq}\mathbf{\right)}$

How many cubic meters of drinking water can be fluoridated to a level of  $\mathbf{1}\mathbf{.}\mathbf{0}\mathbf{ppm}$

What is the mass percent of iron in each of the following iron ores: ${\mathbf{\text{Fe}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{3}}}{\mathbf{\text{, Fe}}}_{\mathbf{\text{3}}}{\mathbf{\text{O}}}_{\mathbf{\text{4}}}{\mathbf{\text{, FeS}}}_{\mathbf{\text{2}}}$?

Silicon is prepared by the reduction of ${\mathbf{\text{K}}}_{\mathbf{\text{2}}}{\mathbf{\text{SiF}}}_{\mathbf{\text{6}}}\mathbf{\text{ with Al}}$. Write the equation for this reaction. (Hint: Can ${\mathbf{\text{F}}}^{\mathbf{-}}$ be oxidized in this reaction? Can $\mathbf{K}$ be reduced?)

The products of the chlor-alkali process,  $\mathit{C}{\mathit{I}}_{\mathbf{2}}$ and  $\mathbf{NaOH}$, are kept separated. 

(a) Why is this necessary when  ${\mathbf{\text{CI}}}_{\mathbf{2}}$  is the desired product?

(b)  ${\mathbf{\text{ClO}}}_{}^{\mathbf{-}}$ or  ${\mathbf{\text{CIO}}}_3^{-}$ may form by disproportionation of  ${\mathbf{\text{CI}}}_{\mathbf{2}}$  in basic solution. What determines which product forms? 

(c) What mole ratio of  ${\mathbf{\text{CI}}}_{\mathbf{2}}$ to  ${\mathbf{\text{OH}}}^{-}$will produce ${\mathbf{\text{ClO}}}_{}^{\mathbf{-}}$ ?  ${\mathbf{\text{CIO}}}_3^{-}$ ?

The key step in the manufacture of sulfuric acid is the oxidation of sulfur dioxide in the presence of a catalyst, such as  ${\mathbf{\text{V}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{5}}}$. At  ${727}^o$C,  $\mathbf{\text{0.010}}$ mol of  ${\mathbf{\text{SO}}}_{\mathbf{\text{2}}}$ is injected into an empty 2.00-L container  $\left(\text{Kp = 3.18}\right)\mathbf{\text{.}}$

(a) What is the equilibrium pressure of  ${\mathbf{\text{O}}}_{\mathbf{\text{2}}}$ that is needed to maintain a 1/1 mole ratio of ${\mathbf{\text{SO}}}_{\mathbf{\text{3}}}$  to ${\mathbf{\text{SO}}}_{\mathbf{\text{2}}}$ ? 

(b) What is the equilibrium pressure of  ${\mathbf{\text{O}}}_{\mathbf{\text{2}}}$ needed to maintain a  mole ratio of ${\text{SO}}_{\text{3}}$  to  ${\mathbf{\text{SO}}}_{\mathbf{\text{2}}}$?

Tetraphosphorus decaoxide $\left({\text{P}}_{\text{4}}{\text{O}}_{\text{10}}\right)$ is made from phosphate rock and used as a drying agent in the laboratory. 

(a) Write a balanced equation for its reaction with water. 

(b) What is the pH of a solution formed from the addition of 8.5 g of  $\mathbf{\left(}{\mathbf{\text{P}}}_{\mathbf{\text{4}}}{\mathbf{\text{O}}}_{\mathbf{\text{10}}}\mathbf{\right)}$ in sufficient water to form $\mathbf{\text{0.750}}$ L? (See Table  18.5, p. 803 , for additional information.)

The final step in the smelting of  

${\mathbf{\text{Cu}}}_{\mathbf{\text{2}}}{\mathbf{\text{S(s) + 2Cu}}}_{\mathbf{\text{2}}}\mathbf{\text{O(s)}}\mathbf{\to }{\mathbf{\text{6Cu(l) + SO}}}_{\mathbf{\text{2}}}\mathbf{\text{(g)}}$ 

(a) Give the oxidation states of copper in ${\mathbf{\text{Cu}}}_{\mathbf{\text{2}}}{\mathbf{\text{S, Cu}}}_{\mathbf{\text{2}}}\mathbf{\text{O, and Cu.}}$ 

(b) What are the oxidizing and reducing agents in this reaction?

A piece of with a surface area of ${\mathbf{\text{2.5 m}}}^{\mathbf{\text{2}}}$ is anodized to produce a film of $\mathbf{\text{Al}}{}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{3 }}}\mathbf{\text{that is 23}}\mathbf{\mu }\mathbf{(}\mathbf{\text{23}}\mathbf{\times }{\mathbf{\text{10}}}^{\mathbf{-}\mathbf{6}}\mathbf{\text{ m}}\mathbf{)}$thick. 

(a) How many coulombs flow through the cell in this process (assume that the density of the $\mathbf{\text{Al}}{}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{3 }}}$layer is $\mathbf{\text{3.97 g/cm3 }}$)? 

(b) If it takes min to produce this film, what current must flow through the cell?

Heavy water ${\mathbf{\text{D}}}_{\mathbf{\text{2}}}\mathbf{\text{O}}$ is used to make deuterated chemicals. 

(a) What major species, aside from the starting compounds, do you expect to find in a solution of  ${\mathbf{\text{CH}}}_{\mathbf{\text{3}}}\mathbf{\text{OH}}$ and  ${\mathbf{\text{D}}}_{\mathbf{\text{2}}}\mathbf{\text{O}}$? 

(b) Write equations to explain how these various species arise. (Hint: Consider the autoionization of both components.)

The production of ${\mathbf{\text{H}}}_{\mathbf{\text{2 }}}$ gas by the electrolysis of water typically requires about $\mathbf{\text{400 kJ }}$ of energy per mole. 

(a) Use the relationship between work and cell potential $\left(\text{Section 21.4}\right)$ to calculate the minimum work needed to form ${\mathbf{\text{1.0 mol of H}}}_{\mathbf{\text{2 }}}$ gas at a cell potential of $\mathbf{\text{1.24 V. }}$ 

(b) What is the energy efficiency of the cell operation? 

(c) Find the cost of producing ${\mathbf{\text{500. mol of H}}}_{\mathbf{\text{2}}}$ if electricity is $0.06per $\mathbf{kilowatt}\mathbf{·}\mathbf{hour}$$\left(\text{1 watt}·\text{second = 1 joule}\right)\mathbf{\text{.}}$

A blast furnace uses ${\mathbf{\text{Fe}}}_{\mathbf{\text{2}}}{\mathbf{\text{O}}}_{\mathbf{\text{3}}}$  to produce $\mathbf{\text{8400 t}}$  of  $\mathbf{\text{Fe}}$ per day. 

(a) What mass of  ${\mathbf{\text{CO}}}_{\mathbf{\text{2}}}$ is produced each day? 

(b) Compare this amount of  ${\text{CO}}_{\text{2}}$ with that produced by  1.0 million automobiles, each burning  $\mathbf{\text{5.0 gal}}$ of gasoline a day. Assume that gasoline has the formula ${\mathbf{\text{C}}}_{\mathbf{\text{8}}}{\mathbf{\text{H}}}_{\mathbf{\text{18}}}$  and a density of  $\mathbf{\text{0.74 g/mL}}$, and that it burns completely. (Note that U.S. gasoline consumption is over  $\mathbf{4}\mathbf{\times }{\mathbf{10}}^{\mathbf{8}}\mathit{g}\mathit{a}\mathit{l}\mathbf{/}\mathit{d}\mathit{a}\mathit{y}$.)

(a) What are the components of the reaction mixture following the water-gas shift reaction? 

(b) Explain how zeolites (Gallery,) are used to purify the ${\mathbf{\text{H}}}_{\mathbf{\text{2}}}$ formed

Among the exothermic steps in the manufacture of sulfuric acid is the process of hydrating ${\mathbf{\text{SO}}}_{\mathbf{\text{3}}}$. 

(a) Write two chemical reactions that show this process. 

(b) Why is the direct reaction of ${\mathbf{\text{SO}}}_{\mathbf{\text{3}}}$ with water not feasible?