Question

Balance this chemical equation and assign it a reaction type: \(\mathrm{CO}(g)+\mathrm{NO}(g) \rightarrow \mathrm{CO}_{2}(g)+\mathrm{N}_{2}(g)\)

Short answer

The balanced chemical equation is \( 2\mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \), and the reaction type is Redox Reaction.

Step-by-step solution

Write down the unbalanced chemical equation

The given unbalanced chemical equation is: \( \mathrm{CO}(g) + \mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \)

Count the atoms on each side of the equation

First, we need to count the number of atoms of each element on both sides of the equation. On the reactants side, we have: - 1 Carbon atom - 1 Oxygen atom - 1 Nitrogen atom On the products side, we have: - 1 Carbon atom - 2 Oxygen atoms - 2 Nitrogen atoms

Balance the equation by adjusting coefficients

Now, we will balance the equation by adjusting the coefficients of the reactants and products. First, balance the Nitrogen atoms. To do this, we can place a coefficient of 2 in front of the NO molecule on the reactants side: \( \mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \) Now, we have: - 1 Carbon atom - 1 Oxygen atom - 2 Nitrogen atoms on the reactants side - 1 Carbon atom - 2 Oxygen atoms - 2 Nitrogen atoms on the products side Next, we need to balance the oxygen atoms. Considering that there are 2 oxygen atoms on the products side and only 1 oxygen atom on the reactants side currently, we can place a coefficient of 2 in front of the CO molecule on the reactants side. \( 2\mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \) Now we have: - 2 Carbon atoms - 2 Oxygen atoms - 2 Nitrogen atoms on the reactants side - 2 Carbon atoms - 2 Oxygen atoms - 2 Nitrogen atoms on the products side The equation is now balanced.

Determine the reaction type

In this reaction, Carbon monoxide (CO) and Nitrogen monoxide (NO) react to form Carbon dioxide (CO2) and molecular Nitrogen (N2). This reaction is an example of a Redox (reduction-oxidation) reaction. In this reaction, Carbon in CO is oxidized from an oxidation state of +2 to an oxidation state of +4 in CO2, while Nitrogen in NO is reduced from an oxidation state of +2 to an oxidation state of 0 in N2.

Final Balanced Equation and Reaction Type

The balanced chemical equation is: \( 2\mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \) The reaction type is: Redox Reaction.

Key concepts

Redox Reactions

Redox reactions, short for reduction-oxidation reactions, are fundamental to understanding many chemical processes. These kinds of reactions involve the transfer of electrons between two chemical substances.
In a redox reaction, one substance loses electrons (oxidation) while another gains electrons (reduction). This electron transfer results in a change in the oxidation states of the substances involved. These reactions are integral to many processes in biology, industry, and the environment.
For example, in the given chemical reaction: \(2\mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g)\), Carbon in CO is oxidized as it loses electrons when it forms \(\mathrm{CO}_2\), while Nitrogen in NO is reduced as it gains electrons, transforming into \(\mathrm{N}_2\).

• The oxidation and reduction processes happen simultaneously, each one being necessary for the other.
• Redox reactions are crucial in energy transfer, including batteries and metabolic pathways.

Oxidation States

Oxidation states, or oxidation numbers, are a way to describe how many electrons an atom has gained or lost compared to its elemental state. This concept helps in predicting the behavior of elements in a chemical reaction, particularly in redox reactions.
For instance, in the redox reaction of \(\mathrm{CO}\) and \(\mathrm{NO}\), the oxidation state of Carbon changes from +2 in \(\mathrm{CO}\) to +4 in \(\mathrm{CO}_2\), while the oxidation state of Nitrogen changes from +2 in \(\mathrm{NO}\) to 0 in \(\mathrm{N}_2\).
Understanding oxidation states involves:

• Assigning oxidation numbers based on general rules, such as the element in its natural state having an oxidation number of zero.
• Recognizing that the total charge of a component equals the sum of its oxidation states.
• Balancing redox reactions by ensuring that electron loss equals electron gain.

By following these procedures, it becomes easier to identify which elements undergo oxidation and which undergo reduction.

Coefficients in Chemical Equations

Coefficients in chemical equations are numbers placed before compounds in a chemical reaction to ensure that the equation abides by the Law of Conservation of Mass. This law states that matter cannot be created or destroyed. Thus, the mass and the number of atoms must be the same on both sides of the equation.
In the solution above, coefficients were adjusted for \(\mathrm{CO}\) and \(\mathrm{NO}\) to 2, which balances the number of Carbon, Oxygen, and Nitrogen atoms on both sides of the equation.

• The process of balancing begins by ensuring that the same number of each atom type appears on both sides of the reaction.
• Coefficients are necessary for integer multiples of reactants and products.
• This adjustment does not affect the chemical identity or properties of the substances involved.

Balancing by coefficients ensures that the chemical equation accurately represents a realistic chemical process.

Molecular Equations

A molecular equation is a way of representing a chemical reaction that shows the complete chemical formulas of all reactants and products. It provides a full view of the substances involved in the reaction, without breaking them down into ions or molecules subtly.
In the equation \( 2\mathrm{CO}(g) + 2\mathrm{NO}(g) \rightarrow \mathrm{CO}_2(g) + \mathrm{N}_2(g) \), the reactants and products are shown as complete molecules, which simplifies the understanding of the overall reaction process.
Molecular equations are often used because:

• They clearly show the reactants and products involved in a reaction, providing a straightforward depiction.
• They are useful in describing reactions where the compounds are stable as molecules, such as gases and liquids.
• They help in visualizing the original composition of reactants and products before any dissociation or ionization occurs.

This type of equation forms the basis upon which further analysis, such as ionic and net ionic equations, can be conducted for more complex reactions.