Question

A chemical dictionary gives the following descriptions of the production of some compounds. Write plausible chemical equations based on these descriptions. (a) lead(II) carbonate: adding a solution of sodium bicarbonate to a solution of lead nitrate. (b) lithium carbonate: reaction of lithium oxide with ammonium carbonate solution. (c) hydrogen peroxide: by the action of dilute sulfuric acid on barium peroxide. (d) lead(IV) oxide: action of an alkaline solution of calcium hypochlorite on lead(II) oxide.

Short answer

The balanced chemical equations are (a) \(NaHCO3 + Pb(NO3)2 \rightarrow PbCO3 + 2NaNO3\), (b) \(Li2O + (NH4)2CO3 \rightarrow Li2CO3 + 2NH3 + H2O\), (c) \(H2SO4 + BaO2 \rightarrow H2O2 + BaSO4\) and (d) \(Ca(ClO)2 + PbO \rightarrow PbO2 + CaCl2\).

Step-by-step solution

Write chemical equation for production of lead(II) carbonate

Start by writing the reactants: sodium bicarbonate (NaHCO3) and lead nitrate (Pb(NO3)2). In this reaction, an exchange of ions takes place, resulting in the formation of lead(II) carbonate (PbCO3) and sodium nitrate (NaNO3). The balanced chemical equation is: \(NaHCO3 + Pb(NO3)2 \rightarrow PbCO3 + 2NaNO3\).

Write chemical equation for production of lithium carbonate

Here, the reactants are lithium oxide (Li2O) and ammonium carbonate ((NH4)2CO3). The products of this reaction are lithium carbonate (Li2CO3) and ammonia (NH3) and water (H2O) . The balanced chemical equation is: \(Li2O + (NH4)2CO3 \rightarrow Li2CO3 + 2NH3 + H2O\).

Write chemical equation for production of hydrogen peroxide

In this case, the reactants are sulfuric acid (H2SO4) and barium peroxide (BaO2). The products of this reaction are hydrogen peroxide (H2O2) and barium sulphate (BaSO4). The balanced chemical equation is: \(H2SO4 + BaO2 \rightarrow H2O2 + BaSO4\).

Write chemical equation for production of lead(IV) oxide

The reactants here are calcium hypochlorite (Ca(ClO)2) and lead(II) oxide (PbO). The reaction yields lead(IV) oxide (PbO2) and calcium chloride (CaCl2). The balanced chemical equation is: \(Ca(ClO)2 + PbO \rightarrow PbO2 + CaCl2\).

Key concepts

Lead(II) Carbonate Synthesis

Understanding the synthesis of lead(II) carbonate is not just about balancing a chemical equation; it is also about comprehending the reaction taking place. When sodium bicarbonate, a commonly used baking soda, reacts with lead nitrate, a soluble lead compound, we observe a double displacement reaction. This occurs when each reactant swaps a part of its chemical structure with the other, resulting in new products.

Lead(II) carbonate, the product of this reaction, is significant in many industries, particularly in the manufacturing of pigments and as a part of some rubber mixtures. This reaction can be visualized in the following balanced chemical equation:
\(NaHCO_3 + Pb(NO_3)_2 \rightarrow PbCO_3 + 2NaNO_3\). Here, the synthesis yields a solid precipitate of lead(II) carbonate and a soluble sodium nitrate.

Lithium Carbonate Formation

Lithium is an element with considerable applications, particularly in the field of batteries. The formation of lithium carbonate involves the reaction between lithium oxide and ammonium carbonate solution. Lithium oxide is a basic oxide that reacts with the ammonium carbonate's acidic properties to neutralize it.

The balanced chemical equation is:
\(Li_2O + (NH_4)_2CO_3 \rightarrow Li_2CO_3 + 2NH_3 + H_2O\).
During this reaction, not only do we get lithium carbonate, a versatile compound used medically and industrially, but we also produce ammonia and water as by-products. This synthesis illustrates the concept of acid-base reaction, where the products are a salt (in this case, lithium carbonate) and water.

Hydrogen Peroxide Production

Hydrogen peroxide is widely recognized for its uses as a disinfectant and bleaching agent. Its production method from barium peroxide and dilute sulfuric acid exemplifies a reaction that gives rise to a less stable peroxide alongside a stable sulfate.

The chemical dynamics for producing hydrogen peroxide are presented in the balanced equation:
\(H_2SO_4 + BaO_2 \rightarrow H_2O_2 + BaSO_4\).
This leads to the formation of hydrogen peroxide and barium sulfate, the latter of which is insoluble and precipitates from the solution. This kind of reaction is particularly interesting due to the decomposition of barium peroxide, which releases the peroxide ion that combines with hydrogen ions to form hydrogen peroxide.

Lead(IV) Oxide Reaction

The reaction that leads to the formation of lead(IV) oxide is a redox reaction, where lead(II) oxide is oxidized to lead(IV) oxide. This process takes us into the realm of environmental chemistry since lead(IV) oxide is encountered in lead-acid batteries.

The chemical representation for this transformation is given by:
\(Ca(ClO)_2 + PbO \rightarrow PbO_2 + CaCl_2\).
This shows us that lead(IV) oxide is formed alongside calcium chloride, which is a by-product in this scenario. It is crucial to understand the redox nature of this reaction as it illustrates the electron transfer processes that are fundamental in many chemical reactions.