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Chapter 4: 4.2 CYL (page 180)

Diatomic chlorine and sodium hydroxide(lye) are commodity chemicals produced in large quantities, along with diatomic hydrogen via the electrolysis of brine according to the following unbalanced equation:

\[NaCl\left( {aq} \right) + {H_2}O\left( l \right) \to NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

Write balanced molecular, complete ionic, and net ionic equations for this process.

Short Answer

Expert verified

The molecular reaction of the given process will be:

\[2NaCl\left( {aq} \right) + 2{H_2}O\left( l \right) \to 2NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

The complete ionic reaction of the given process will be:

The net ionic reaction of the given process will be:

Step by step solution

01

Determine the molecular reaction

Balance the given reaction.

\[2NaCl\left( {aq} \right) + 2{H_2}O\left( l \right) \to 2NaOH\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

02

Determine the complete ionic reaction

Write the ionic form of the reaction in step 1.

\[2N{a^ + }\left( {aq} \right) + 2C{l^ - }\left( {aq} \right) + 2{H_2}O\left( l \right) \to 2N{a^ + }\left( {aq} \right) + 2O{H^ - }\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right).\]

03

Determine the net ionic reaction

Write the net ionic equation by cancelling out the same ions.

\[2C{l^ - }\left( {aq} \right) + 2{H_2}O\left( l \right) \to 2O{H^ - }\left( {aq} \right) + {H_2}\left( g \right) + C{l_2}\left( g \right)\]

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Most popular questions from this chapter

Outline the steps needed to determine the limiting reactant when 30.0 g of propane,\({C_3}{H_8}\), is burned with 75.0 g of oxygen. Determine the limiting reactant.

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process.

(a)The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide.

(b)The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water.

(c)Solid calcium hydroxide is the added to the sea water, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride

(d)The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

(e)Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.

Write a balanced equation describing each of the following chemical reactions.

(a) Solid potassium chlorate, KClO3 decomposes to form solid potassium chloride and diatomic oxygen gas

(b) Solid aluminium metal reacts with solid diatomic iodine to form solid Al2I6

(c) When solid sodium chloride is added to aqueous sulfuric acid, hydrogen chloride gas and aqueous sodium sulfate are produced.

(d) Aqueous solutions of phosphoric acid and potassium hydroxide react to produce aqueous potassium dihydrogen phosphate and liquid water.

Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide).

(a) Write an equation of the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water.

(b)The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solution of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.

Which is the limiting reactant when 5.00 g of H2 and 10 g of O2 react to form water?

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