Question

Given the equation for the reaction: \(\mathrm{N}_{2}+\mathrm{H}_{2} \rightarrow \mathrm{NH}_{3}\) draw a molecular diagram that represents the reaction (make sure it is balanced).

Short answer

The balanced equation for the reaction is: \(\mathrm{N}_{2} + 3\mathrm{H}_{2} \rightarrow 2\mathrm{NH}_{3}\). One nitrogen molecule (N2) reacts with three hydrogen molecules (H2) to yield two ammonia molecules (NH3). The molecular diagram will look like: Initial state: [N ≡ N] + 3[H - H] Final state: 2[N - (H)3] Where [N ≡ N] represents one N2 molecule, [H - H] represents one H2 molecule, and [N - (H)3] represents one NH3 molecule.

Step-by-step solution

Identify the Molecules in the Reaction

Observe the balanced equation: \(\mathrm{N}_{2}+\mathrm{H}_{2}\rightarrow \mathrm{NH}_{3}\). Nitrogen is present as N2, hydrogen as H2, and ammonia as NH3.

Balance the Reaction

In order to draw a molecular diagram, we need to balance the equation first. The balanced equation is: \(\mathrm{N}_{2} + 3\mathrm{H}_{2} \rightarrow 2\mathrm{NH}_{3}\). This means that one nitrogen molecule (N2) reacts with three hydrogen molecules (H2) to yield two ammonia molecules (NH3).

Draw Nitrogen Molecules in their Initial State

Nitrogen molecules consist of two nitrogen atoms bonded together (N2). Since there's only one N2 molecule in the reaction, draw one N2 molecule.

Draw Hydrogen Molecules in their Initial State

Hydrogen molecules consist of two hydrogen atoms bonded together (H2). Three H2 molecules are needed for the reaction, so draw three H2 molecules.

Draw Ammonia Molecules in their Final State

Ammonia molecules consist of one nitrogen atom bonded to three hydrogen atoms (NH3). Two NH3 molecules are produced in the reaction, so draw two NH3 molecules.

Connect the Initial and Final States

Draw arrows representing the reaction, showing the nitrogen molecules and hydrogen molecules being converted to ammonia molecules. Indicate the balanced reaction above the arrows. The final molecular diagram will look like this: N2 + 3H2 → 2NH3 Initial state: [N ≡ N] + 3[H - H] Final state: 2[N - (H)3] Where [N ≡ N] represents one N2 molecule, [H - H] represents one H2 molecule, and [N - (H)3] represents one NH3 molecule.

Key concepts

Balancing Chemical Equations

Understanding how to balance chemical equations is crucial for anyone studying chemistry or related sciences. Balancing chemical equations involves ensuring that the number of atoms for each element is equal on both sides of the reaction. This is a reflection of the law of conservation of mass, which states that mass cannot be created or destroyed in an ordinary chemical reaction.

Let's consider the synthesis of ammonia (NH3) as an example. The unbalanced equation for this reaction is: \(\mathrm{N}_2 + \mathrm{H}_2 \rightarrow \mathrm{NH}_3\). To balance this equation, count the atoms of nitrogen and hydrogen on both sides of the reaction. The balanced equation is: \(\mathrm{N}_2 + 3\mathrm{H}_2 \rightarrow 2\mathrm{NH}_3\) as it fulfills the requirement of having an equal number of nitrogen and hydrogen atoms on either side. In this case, you need three molecules of hydrogen (each having two atoms) to react with one molecule of nitrogen (having two atoms) to produce two molecules of ammonia, each with one nitrogen atom and three hydrogen atoms.

Remember, coefficients in front of molecules indicate how many of each molecule you need, while subscripts indicate how many atoms are in each molecule. This clarity helps in visual representations and molecular diagrams as well.

Molecular Diagrams

Molecular diagrams serve as visual tools to better understand chemical reactions. They provide a snapshot of the molecules involved in the reaction and how they rearrange to form new substances. By drawing diagrams, students can get an intuitive grasp on mole-to-mole relationships and the breaking and forming of bonds in a reaction.

In the case of ammonia synthesis, the molecular diagram starts with molecules of nitrogen (\(\mathrm{N}_2\)) and hydrogen (\(\mathrm{H}_2\)). These are depicted as pairs of atoms bonded together, nitrogen with a triple bond (represented as \(\mathrm{N} \equiv \mathrm{N}\)) and hydrogen with a single bond (represented as \(\mathrm{H}-\mathrm{H}\)). After the reaction occurs, the nitrogen and hydrogen atoms rearrange to form ammonia. The molecular diagram for ammonia illustrates one nitrogen atom bonded to three hydrogen atoms (represented as \(\mathrm{N}-(\mathrm{H})_3\)).

Using molecular diagrams can reveal, at a glance, the balance of a chemical equation and the stoichiometry of the reaction. In the synthesis of ammonia, it becomes immediately apparent that three hydrogens pair with a single nitrogen to satisfy the valency and form two ammonia molecules.

Ammonia Synthesis

Ammonia synthesis refers to the chemical process of forming ammonia (\(\mathrm{NH}_3\)) from its elements: nitrogen (\(\mathrm{N}_2\)) and hydrogen (\(\mathrm{H}_2\)). This process is significant in both industrial terms and for academic study, as ammonia is a key ingredient in fertilizers and many other chemicals.

The classic method of producing ammonia is through the Haber process, which involves a reaction between nitrogen and hydrogen gases under high temperatures and pressures in the presence of a catalyst. The balanced chemical equation for this reaction is: \(\mathrm{N}_2 + 3\mathrm{H}_2 \rightarrow 2\mathrm{NH}_3\).

In a classroom or homework setting, when students are tasked with drawing a molecular diagram for this reaction, it is important for them to understand the balance and movement of atoms. As such, educators may stress the importance of depicting the correct number of nitrogen and hydrogen molecules before the reaction and the resulting ammonia molecules after the reaction, as reflected in the balanced equation. This visualization not only aids in grasping the concept of ammonia synthesis but also reinforces the principles of balancing chemical equations and interpreting molecular diagrams.