Question

Give the balanced equation for each of the following chemical reactions: a. Glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) reacts with oxygen gas to produce gaseous carbon dioxide and water vapor. b. Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron((III) chloride and hydrogen sulfide gas. c. Carbon disulfide liquid reacts with ammonia gas to produce hydrogen sulfide gas and solid ammonium thiocyanate \(\left(\mathrm{NH}_{4} \mathrm{SCN}\right)\)

Short answer

The balanced equations for the given reactions are: a. \[\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} + 6\mathrm{O}_{2} \rightarrow 6\mathrm{CO}_{2} + 6\mathrm{H}_{2} \mathrm{O}\] b. \[2\mathrm{Fe}_{2} \mathrm{S}_{3} + 6\mathrm{HCl} \rightarrow 4\mathrm{FeCl}_{3} + 3\mathrm{H}_{2} \mathrm{S}\] c. \[\mathrm{CS}_{2} + 2\mathrm{NH}_{3} \rightarrow \mathrm{H}_{2} \mathrm{S} + 2\mathrm{NH}_{4} \mathrm{SCN}\]

Step-by-step solution

a. Balancing glucose and oxygen reaction

1. Write the unbalanced equation: \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} + \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2} + \mathrm{H}_{2} \mathrm{O}\) 2. Count the number of atoms for each element type: On the reactants side: 6 C, 12 H, 8 O. On the products side: 1 C, 2 H, 3 O. 3. Balance the equation by adjusting coefficients: \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} + 6\mathrm{O}_{2} \rightarrow 6\mathrm{CO}_{2} + 6\mathrm{H}_{2} \mathrm{O}\) The balanced equation is: \[\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6} + 6\mathrm{O}_{2} \rightarrow 6\mathrm{CO}_{2} + 6\mathrm{H}_{2} \mathrm{O}\]

b. Balancing iron(III) sulfide and hydrogen chloride reaction

1. Write the unbalanced equation: \(\mathrm{Fe}_{2} \mathrm{S}_{3} + \mathrm{HCl} \rightarrow \mathrm{FeCl}_{3} + \mathrm{H}_{2} \mathrm{S}\) 2. Count the number of atoms for each element type: On the reactants side: 2 Fe, 3 S, 1 H, 1 Cl. On the products side: 1 Fe, 1 S, 2 H, 3 Cl. 3. Balance the equation by adjusting coefficients: \(2\mathrm{Fe}_{2} \mathrm{S}_{3} + 6\mathrm{HCl} \rightarrow 4\mathrm{FeCl}_{3} + 3\mathrm{H}_{2} \mathrm{S}\) The balanced equation is: \[2\mathrm{Fe}_{2} \mathrm{S}_{3} + 6\mathrm{HCl} \rightarrow 4\mathrm{FeCl}_{3} + 3\mathrm{H}_{2} \mathrm{S}\]

c. Balancing carbon disulfide and ammonia reaction

1. Write the unbalanced equation: \(\mathrm{CS}_{2} + \mathrm{NH}_{3} \rightarrow \mathrm{H}_{2} \mathrm{S} + \mathrm{NH}_{4} \mathrm{SCN}\) 2. Count the number of atoms for each element type: On the reactants side: 1 C, 2 S, 1 N, 3 H. On the products side: 1 N, 5 H, 2 S, 1 C. 3. Balance the equation by adjusting coefficients: \(\mathrm{CS}_{2} + 2\mathrm{NH}_{3} \rightarrow \mathrm{H}_{2} \mathrm{S} + 2\mathrm{NH}_{4} \mathrm{SCN}\) The balanced equation is: \[\mathrm{CS}_{2} + 2\mathrm{NH}_{3} \rightarrow \mathrm{H}_{2} \mathrm{S} + 2\mathrm{NH}_{4} \mathrm{SCN}\]

Key concepts

Chemical Reactions

Chemical reactions are processes where elements or compounds, known as reactants, transform into new substances called products. This change involves the breaking and reforming of chemical bonds. Recognizing a chemical reaction mainly relies on indicators such as the release of gas, formation of a solid precipitate, or a visible color change.

Chemical equations are the language of chemistry used to represent these reactions. The reactants are written on the left, products on the right, and an arrow pointing to the products signifies the direction of the reaction. It’s crucial to note that atoms are neither created nor destroyed in these processes—only rearranged.

• Unbalanced equations simply list the reactants and products.
• Balanced equations account for the conservation of mass, ensuring the equation reflects the same number of each type of atom on both sides.

Balancing equations is essential for accurately representing a chemical change.

Stoichiometry

Stoichiometry is like a cookbook for chemistry. It provides the proportions in which chemicals combine and react. This concept is crucial for predicting the amounts of products formed from reactants in chemical reactions.

At the heart of stoichiometry is the balanced chemical equation. It provides the necessary conversion factors to relate different substances in a reaction. For instance, the balanced equation for glucose combustion: \[\mathrm{C}_{6}\mathrm{H}_{12}\mathrm{O}_{6} + 6\mathrm{O}_{2} \rightarrow 6\mathrm{CO}_{2} + 6\mathrm{H}_{2}\mathrm{O}\]Here, it indicates:

• 1 molecule of glucose combines with 6 molecules of oxygen.
• Produces 6 molecules of carbon dioxide and 6 molecules of water.

These ratios can extend from molecules to moles, enabling calculations of quantities in, for example, grams or liters, revealing the reaction's full scope.

Glucose Combustion

Glucose combustion is a type of chemical reaction known as an exothermic reaction, where energy is released in the form of heat. This specific process involves glucose (a sugar) reacting with oxygen to produce carbon dioxide and water. It's a vital reaction in respiratory cells, fueling our bodies by releasing stored energy.

The balanced equation is:\[\mathrm{C}_{6}\mathrm{H}_{12}\mathrm{O}_{6} + 6\mathrm{O}_{2} \rightarrow 6\mathrm{CO}_{2} + 6\mathrm{H}_{2}\mathrm{O}\]

• Each glucose molecule reacts with six oxygen molecules.
• The end products, carbon dioxide and water, are also the main components expelled in respiration.

Understanding glucose combustion is crucial for appreciating processes like metabolism and cellular respiration.

Iron(III) Chloride Formation

The formation of Iron(III) chloride exemplifies a synthesis reaction. This is where simpler substances combine to form a more complex product. It occurs when iron(III) sulfide reacts with hydrogen chloride to produce iron(III) chloride and hydrogen sulfide.

The balanced chemical equation is: \[2\mathrm{Fe}_{2} \mathrm{S}_{3} + 6\mathrm{HCl} \rightarrow 4\mathrm{FeCl}_{3} + 3\mathrm{H}_{2} \mathrm{S}\]In this reaction:

• Two units of iron(III) sulfide react with six units of hydrogen chloride.
• This results in the formation of iron(III) chloride and hydrogen sulfide gas.

The result, iron(III) chloride, has significant applications, including use in water purification and as a catalyst in various chemical reactions.