Question

The gases nitrogen dioxide and oxygen react to produce dinitrogen pentoxide gas.

Short answer

The balanced chemical equation for the reaction between nitrogen dioxide and oxygen gas to produce dinitrogen pentoxide gas is: \(4NO_2(g) + O_2(g) \rightarrow 2N_2O_5(g)\)

Step-by-step solution

1. Write down the chemical formulas of the given gases

We have three gases given: nitrogen dioxide, oxygen, and dinitrogen pentoxide. Their chemical formulas are: - Nitrogen dioxide: \(NO_2\) - Oxygen: \(O_2\) - Dinitrogen pentoxide: \(N_2O_5\)

2. Write the unbalanced chemical equation

Now we need to write the unbalanced chemical equation for this reaction. The equation is as follows: \(NO_2 + O_2 \rightarrow N_2O_5\)

3. Balance the chemical equation

To balance the equation, we need to count the number of atoms for each element on both sides and make sure they are equal. We can achieve this by placing coefficients in front of the chemical formulas. Starting with the nitrogen atoms: on the left side, we have 1 nitrogen atom in nitrogen dioxide, and on the right side, we have 2 nitrogen atoms in dinitrogen pentoxide. So, we need to multiply the nitrogen dioxide molecule on the left by 2 to balance the nitrogen atoms: \(2NO_2 + O_2 \rightarrow N_2O_5\) Now, let's count the oxygen atoms: On the left side, we have 4 oxygen atoms (2 in each nitrogen dioxide) and 2 oxygen atoms in the oxygen gas, which sums up to 6, and on the right side, we have 5 oxygen atoms in dinitrogen pentoxide. To balance the oxygen atoms, we can change the coefficient of oxygen gas to ½: \(2NO_2 + \frac{1}{2}O_2 \rightarrow N_2O_5\) However, it is common practice to use whole numbers as coefficients in chemical equations. So, we will multiply the whole equation by 2 to get rid of the fraction: \(4NO_2 + O_2 \rightarrow 2N_2O_5\) Now the balanced equation is: \(4NO_2(g) + O_2(g) \rightarrow 2N_2O_5(g)\)

4. Summary

In summary, we analyzed the given information, wrote down the chemical formulas for the given gases, wrote the unbalanced chemical equation, and then balanced it. The balanced chemical equation for the reaction between nitrogen dioxide and oxygen gas to produce dinitrogen pentoxide gas is: \(4NO_2(g) + O_2(g) \rightarrow 2N_2O_5(g)\)

Key concepts

Balancing Equations

Balancing chemical equations is a fundamental aspect of chemistry that ensures the law of conservation of mass is obeyed. This law states that matter cannot be created or destroyed in a chemical reaction. Therefore, the mass of the reactants must equal the mass of the products. To balance an equation, follow these simple steps:

• First, write the unbalanced chemical equation using the correct chemical formulas for all reactants and products.
• Next, count the number of atoms for each element on both sides of the equation.
• Add coefficients—a number placed in front of a molecule—to equalize the number of atoms for each element on both sides.

For the reaction of nitrogen dioxide and oxygen to form dinitrogen pentoxide, balancing requires careful attention to both nitrogen and oxygen atoms. Initially, the unbalanced equation is: \(NO_2 + O_2 \rightarrow N_2O_5\).
By adjusting coefficients, our final balanced equation becomes \(4NO_2 + O_2 \rightarrow 2N_2O_5\). This shows that four nitrogen dioxide molecules react with one oxygen molecule to form two dinitrogen pentoxide molecules.

Chemical Formulas

Chemical formulas represent the types and numbers of atoms in a substance, offering a concise way to depict the composition of compounds. For instance, \(NO_2\) stands for nitrogen dioxide, comprising one nitrogen atom and two oxygen atoms per molecule. Chemical formulas are vital for writing chemical equations, helping chemists understand the reacting species and the products formed.
The formula for dinitrogen pentoxide, \(N_2O_5\), indicates each molecule contains two nitrogen atoms and five oxygen atoms. Chemical formulas allow us to see clearly how substances are transformed in a reaction, which is crucial for correctly setting up equations before balancing them.

• Recognize different types of atoms represented by chemical symbols, like N for nitrogen and O for oxygen.
• Use subscripts in formulas to show the number of each type of atom in a molecule.
• Ensure the sum of individual atoms from reactants equals that of the products to comply with conservation laws.

Dinitrogen Pentoxide

Dinitrogen pentoxide, represented by the formula \(N_2O_5\), is a compound formed when nitrogen dioxide and oxygen gas react under certain conditions. It is one of the nitrogen oxides and is significant due to its role in atmospheric chemistry. As a product in the lesson's chemical reaction, it highlights the transformation of smaller molecules like \(NO_2\) and \(O_2\) into larger, more complex structures.

• Comprised of 2 nitrogen and 5 oxygen atoms, making it a nitrogen oxide with high oxygen content.
• Acts as an acid anhydride, forming nitric acid (\(HNO_3\)) when reacted with water.
• Due to its reactive nature, it serves significant functions in pollution control and chemical synthesis.

Reacting \(NO_2\) with \(O_2\) produces \(N_2O_5\), and understanding this transformation through balanced equations is key to mastering chemical reaction mechanisms.

Nitrogen Dioxide

Nitrogen dioxide, \(NO_2\), is a reddish-brown gas notorious for its role in atmospheric pollution, contributing to smog and respiratory issues. In chemistry, it's notable for its ability to react with other gases, including oxygen, to form more significant compounds such as dinitrogen pentoxide. This compound:

• Contains one nitrogen atom bonded to two oxygen atoms, forming a polar molecule.
• Is a primary pollutant emitted from vehicles and industrial processes.
• Can react further, forming acids like nitric acid (\(HNO_3\)) under the influence of water.

In our chemical reaction \(4NO_2 + O_2 \rightarrow 2N_2O_5\), nitrogen dioxide plays a critical part as a reactant, showing how pollution sources can contribute to forming other nitrogen oxides.