Write a balanced equation for the reaction that occurs in each of the following cases: (c) Sodium reacts with oxygen.

Verified step by step guidance

Identify the reactants: Sodium (Na) and Oxygen (O_2).

Determine the product: Sodium reacts with oxygen to form sodium oxide (Na_2O).

Write the unbalanced equation: Na + O_2 \rightarrow Na_2O.

Balance the equation by adjusting coefficients: Start by balancing the sodium atoms. Since there are 2 sodium atoms in Na_2O, place a coefficient of 2 in front of Na: 2Na + O_2 \rightarrow Na_2O.

Check the balance of oxygen atoms: There are 2 oxygen atoms on the reactant side and 1 on the product side. Place a coefficient of 2 in front of Na_2O to balance the oxygen: 4Na + O_2 \rightarrow 2Na_2O.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas.

Sodium and Oxygen Reaction

When sodium (Na) reacts with oxygen (O2), it forms sodium oxide (Na2O). This reaction is an example of a combustion reaction where a metal reacts with a non-metal. Sodium is a highly reactive alkali metal, and it reacts vigorously with oxygen, often producing heat and light.

Types of Chemical Reactions

Chemical reactions can be classified into several types, including synthesis, decomposition, single replacement, and double replacement. The reaction between sodium and oxygen is a synthesis reaction, where two or more reactants combine to form a single product. Understanding these classifications helps in predicting the products and balancing the equations.

Recommended video:

Guided course

02:25

Common Types of Alkane Reactions

Related Practice

Textbook Question

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Potassium metal is exposed to an atmosphere of chlorine gas.

views

Textbook Question

Write a balanced equation for the reaction that occurs in each of the following cases: (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal reacts with molten sulfur.

views

Textbook Question

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Cesium is added to water.

views

Textbook Question

(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens to form halides. Compare the roles of hydrogen and halogens in these reactions. Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. (b) What is the oxidation number and electron configuration of calcium in each product?

Textbook Question

Potassium and hydrogen react to form the ionic compound potassium hydride. (b) Use data in Figures 7.10 and 7.12 to determine the energy change in kJ/mol for the following two reactions:

K(g) + H(g) → K⁺(g) + H^-(g)

K(g) + H(g) → K^-(g) + H⁺(g)