Question

Write balanced chemical equations for the following reactions: (a) production of ammonia, \(\mathrm{NH}_{3}(\mathrm{g}),\) by combining \(\mathrm{N}_{2}(\mathrm{g})\) and \(\mathrm{H}_{2}(\mathrm{g})\) (b) production of methanol, \(\mathrm{CH}_{3} \mathrm{OH}(\ell)\) by combining \(\mathrm{H}_{2}(\mathrm{g})\) and \(\mathrm{CO}(\mathrm{g})\) (c) production of sulfuric acid by combining sulfur, oxygen, and water

Short answer

(a) \( \mathrm{N}_2(g) + 3\mathrm{H}_2(g) \rightarrow 2\mathrm{NH}_3(g) \) (b) \( \mathrm{CO}(g) + 2\mathrm{H}_2(g) \rightarrow \mathrm{CH}_3OH}(l) \) (c) Requires multiple steps: production of \( \mathrm{H}_2SO_4 \) from \( \mathrm{S} \), \( \mathrm{O}_2 \), and \( \mathrm{H}_2O \).

Step-by-step solution

Write Unbalanced Equation for Ammonia Production

The chemical reaction involves combining nitrogen gas, \( \mathrm{N}_2(g) \), with hydrogen gas, \( \mathrm{H}_2(g) \), to form ammonia, \( \mathrm{NH}_3(g) \). The unbalanced equation is:\[ \mathrm{N}_2(g) + \mathrm{H}_2(g) \rightarrow \mathrm{NH}_3(g) \]

Balance the Ammonia Production Equation

For ammonia production, start by balancing nitrogen atoms. We need 2 ammonia molecules to balance with the 2 nitrogen atoms in \( \mathrm{N}_2 \). Then adjust hydrogen atoms: since there are 6 hydrogens in 2 \( \mathrm{NH}_3 \), 3 molecules of \( \mathrm{H}_2 \) are required:\[ \mathrm{N}_2(g) + 3\mathrm{H}_2(g) \rightarrow 2\mathrm{NH}_3(g) \]

Write Unbalanced Equation for Methanol Production

Methanol is produced by combining \( \mathrm{H}_2(g) \) and \( \mathrm{CO}(g) \). The initial unbalanced equation is:\[ \mathrm{CO}(g) + \mathrm{H}_2(g) \rightarrow \mathrm{CH}_3OH}(l) \]

Balance the Methanol Production Equation

To balance the methanol equation, balance the carbon atoms: 1 molecule of \( \mathrm{CO} \) is needed. Then, balance the hydrogen atoms: 2 atoms from \( \mathrm{CH}_3OH \) and 1 extra \( \mathrm{H}_2 \) balance the 4 total hydrogen atoms, for a balanced equation:\[ \mathrm{CO}(g) + 2 \mathrm{H}_2(g) \rightarrow \mathrm{CH}_3OH}(l) \]

Write Unbalanced Equation for Sulfuric Acid Production

Sulfuric acid is produced from sulfur, oxygen, and water. The unbalanced reaction involves sulfur \( \mathrm{S}(s) \), oxygen \( \mathrm{O}_2(g) \), and water \( \mathrm{H}_2O(l) \) forming \( \mathrm{H}_2SO_4(l) \) :\[ \mathrm{S}(s) + \mathrm{O}_2(g) + \mathrm{H}_2O(l) \rightarrow \mathrm{H}_2SO_4(l) \]

Balance the Sulfuric Acid Production Equation

To form sulfuric acid, convert sulfur to \( \mathrm{SO_2} \) by reacting with \( \mathrm{O_2} \), then further react \( \mathrm{SO_2} \) with \( \mathrm{O_2} \) and \( \mathrm{H}_2O \) to produce \( \mathrm{H}_2SO_4 \). The balanced multi-step equations are:1. \[ \mathrm{S}(s) + \mathrm{O}_{2}(g) \rightarrow \mathrm{SO}_{2}(g) \]2. \[ 2 \mathrm{SO}_{2}(g) + \mathrm{O}_{2}(g) \rightarrow 2\mathrm{SO}_{3}(g) \]3. \[ \mathrm{SO}_{3}(g) + \mathrm{H}_{2}O(l) \rightarrow \mathrm{H}_{2}SO_{4}(l) \]

Key concepts

Chemical Reactions

Chemical reactions are processes where substances, known as reactants, transform into different substances, called products. These changes involve the breaking of bonds in the reactants and the formation of new bonds to create the products.
A chemical equation represents these changes and includes the chemical formulas of reactants on the left and products on the right, separated by an arrow.

• Reactants: Substances that initiate the chemical reaction.
• Products: Substances formed as a result of the reaction.

Balancing chemical equations is crucial because it follows the law of conservation of mass, which states that matter cannot be created or destroyed. This means the number of each type of atom must be the same on both sides of the equation.

• Start by writing the unbalanced equation.
• Count the number of each type of atom on both sides.
• Adjust coefficients to balance the atoms.
• Ensure the same number and type of atoms appear in reactants and products.

Ammonia Production

Ammonia production involves the synthesis of ammonia (\( \mathrm{NH}_{3}(\mathrm{g}) \)) from nitrogen (\( \mathrm{N}_{2}(\mathrm{g}) \)) and hydrogen (\( \mathrm{H}_{2}(\mathrm{g}) \)). This chemical reaction is represented by the balanced equation:\[\mathrm{N}_2(g) + 3\mathrm{H}_2(g) \rightarrow 2\mathrm{NH}_3(g)\]The balancing process starts by ensuring there are equal numbers of nitrogen atoms on both sides. Since two nitrogen atoms are found in the ammonia molecule, we use 2 molecules of ammonia to balance with the 2 nitrogen atoms in\( \mathrm{N}_2 \).
Next, adjust the hydrogen atoms. With 6 hydrogen atoms present in 2 ammonia molecules, we add 3 hydrogen molecules (each containing 2 hydrogen atoms) to balance. This balanced equation is essential for understanding the stoichiometry in industrial ammonia production processes, such as the Haber-Bosch process.

• Used in fertilizers, explosives, and household products.
• Critical for agricultural productivity.

Methanol Production

Producing methanol involves combining carbon monoxide \( \mathrm{CO}(g) \) and hydrogen \( \mathrm{H}_{2}(g) \) under controlled conditions to form methanol \( \mathrm{CH}_{3} \mathrm{OH}(l) \). The balanced equation is as follows:\[\mathrm{CO}(g) + 2 \mathrm{H}_2(g) \rightarrow \mathrm{CH}_3OH(l)\]The equation starts by ensuring 1 carbon atom in carbon monoxide balances with 1 carbon atom in the methanol product. To address the hydrogen atoms, consider that 2 atoms are needed from hydrogen gas on top of the 2 hydrogen atoms present in methanol, making a total of 4 hydrogen atoms balanced across reactants and products.

• Methanol is a feedstock for formaldehyde production.
• Used as a fuel and antifreeze.

Sulfuric Acid Synthesis

Sulfuric acid is synthesized from sulfur,\( \mathrm{S}(s) \), oxygen,\( \mathrm{O}_{2}(g) \), and water,\( \mathrm{H}_2O(l) \). The balanced synthesis involves multiple steps:1. Sulfur reacts with oxygen to form sulfur dioxide:\[\mathrm{S}(s) + \mathrm{O}_{2}(g) \rightarrow \mathrm{SO}_{2}(g)\]2. Sulfur dioxide further reacts with oxygen to create sulfur trioxide:\[2 \mathrm{SO}_{2}(g) + \mathrm{O}_{2}(g) \rightarrow 2\mathrm{SO}_{3}(g)\]3. Finally, sulfur trioxide reacts with water to produce sulfuric acid:\[\mathrm{SO}_{3}(g) + \mathrm{H}_{2}O(l) \rightarrow \mathrm{H}_{2}SO_{4}(l)\]These reactions collectively illustrate the complexity of balancing multi-step processes. Sulfuric acid is one of the most produced industrial chemicals, serving key roles in the production of fertilizers, in petroleum refining, and in wastewater processing.

• Strong acid used in industrial chemical reactions.
• Vital in manufacturing applications.