Question

Complete and balance the following equations: (a) \(\mathrm{Ba}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (b) \(\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\) (c) \(\mathrm{N}_{2} \mathrm{O}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\)

Short answer

(a) \( \mathrm{Ba}(s) + 2\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ba(OH)}_{2}(aq) + \mathrm{H}_{2}(g) \); (b) \( \mathrm{CaO}(s) + \mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{Ca(OH)}_{2}(aq) \); (c) \( \mathrm{N}_{2} \mathrm{O}_{3}(g) + \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 2\mathrm{HNO}_{2}(aq) \)."

Step-by-step solution

Understanding the Problem

We need to complete and balance the given chemical equations. Each reaction involves adding reactants and products until the equation is balanced, meaning the number of atoms for each element is equal on both sides of the equation.

Completing Equation (a)

For equation (a), when barium (Ba) reacts with water (H₂O), it forms barium hydroxide, Ba(OH)₂, and hydrogen gas, H₂. The unbalanced equation is: \( \mathrm{Ba}(\mathrm{s}) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ba(OH)}_{2}(aq) + \mathrm{H}_{2}(g) \).

Balancing Equation (a)

For balancing, ensure the number of each type of atom is the same on both sides. Here, you need 2 water molecules for every barium atom: \( \mathrm{Ba}(\mathrm{s}) + 2\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ba(OH)}_{2}(aq) + \mathrm{H}_{2}(g) \).

Completing Equation (b)

Calcium oxide (CaO) reacts with water to form calcium hydroxide, Ca(OH)₂. The unbalanced equation is: \( \mathrm{CaO}(s) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca(OH)}_{2}(aq) \).

Balancing Equation (b)

In this equation, the number of atoms is already balanced since one calcium, two oxygen, and two hydrogen atoms are present on both sides: \( \mathrm{CaO}(s) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca(OH)}_{2}(aq) \).

Completing Equation (c)

Dinitrogen trioxide (N₂O₃) reacts with water to form nitric acid, HNO₂. The unbalanced equation is: \( \mathrm{N}_{2} \mathrm{O}_{3}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2\mathrm{HNO}_{2}(aq) \).

Balancing Equation (c)

The equation is already balanced since there are 2 nitrogen, 4 oxygen, and 2 hydrogen atoms on both sides: \( \mathrm{N}_{2} \mathrm{O}_{3}(g) + \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2\mathrm{HNO}_{2}(aq) \).

Key concepts

Chemical Reactions

Chemical reactions are processes where substances, called reactants, are transformed into different substances, known as products. These reactions are essential in chemistry as they enable the understanding of how different materials interact with each other. Reactants interact to form products, and this transformation can be represented by a chemical equation.

• In a chemical equation, reactants are typically placed on the left side, while the products are positioned on the right. An arrow signifies the direction of the reactions, indicating the conversion of reactants to products.
• Balancing chemical equations is crucial because it obeys the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Hence, each side of a chemical equation must have the same number of atoms for each element.
• For example, in the reaction between barium and water: depicted by the equation: \( \mathrm{Ba} + 2\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Ba(OH)}_{2} + \mathrm{H}_{2} \), the process involves restructuring atoms to form new compounds, specifically barium hydroxide and hydrogen gas.

Stoichiometry

Stoichiometry is a fundamental concept in chemistry that deals with the measurement and calculation of the quantities of reactants and products involved in a chemical reaction. Understanding stoichiometry is key to predicting the amounts of substances consumed and produced.

• This concept is applied by using balanced chemical equations to determine the proportions in which reactants combine and products form.
• It enables chemists to calculate precisely how much of each reactant is required to produce a desired amount of product, avoiding excess or deficit.
• For instance, in the reaction of calcium oxide and water to form calcium hydroxide: \( \mathrm{CaO} + \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Ca(OH)}_{2} \), stoichiometry helps us determine that exactly one mole of calcium oxide reacts with one mole of water to produce one mole of calcium hydroxide.
• Through stoichiometry, one can also calculate the yield of reactions, a critical aspect in both laboratory and industrial chemical processes.

Inorganic Chemistry

Inorganic chemistry deals with the properties and behavior of inorganic compounds, which are compounds not primarily composed of carbon. This branch of chemistry is vast, encompassing the study of metals, minerals, and organometallic compounds.

• The reactions involving inorganic compounds such as oxides, acids, bases, and salts often exhibit unique and diverse properties.
• Inorganic reactions include the formation of new bonds, ionic interactions, and complexation, all of which are critical in both natural and industrial processes.
• For example, the reaction between dinitrogen trioxide and water forming nitric acid: \( \mathrm{N}_{2} \mathrm{O}_{3} + \mathrm{H}_{2} \mathrm{O} \rightarrow 2\mathrm{HNO}_{2} \), illustrates a classic inorganic reaction where a gas reacts with a liquid, showcasing the versatile nature of inorganic chemistry.
• Inorganic chemistry also plays a crucial role in fields such as materials science, geochemistry, and catalysis.