Suppose a 500. mL flask is filled with 1.0 mol of N₂ and 1.5 mol of NO. This reaction becomes possible: N₂(g) + O₂(g) 2NO(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O₂. You can leave out the M symbol for molarity. initial change equilibrium 1 N₂ 0 0 0 0₂ X 0 NO 0 0 Undo
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![**Transcription for Educational Website: Setting up a Reaction Table**
Suppose a 500 mL flask is filled with 1.0 mol of N₂ and 1.5 mol of NO. This reaction becomes possible:
\[ \text{N}_2 (g) + \text{O}_2 (g) \rightleftharpoons 2\text{NO} (g) \]
Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium.
Use \( x \) to stand for the unknown change in the molarity of \( \text{O}_2 \). You can leave out the \( M \) symbol for molarity.
\[\begin{array}{cccc}
& \text{N}_2 & \text{O}_2 & \text{NO} \\
\hline
\text{initial} & & & \\
\text{change} & & x & \\
\text{equilibrium} & & & \\
\end{array} \]
The diagram provides an interactive section where you can input values for each stage: initial, change, and equilibrium.
- **Initial:** Indicates the starting molarity of each compound.
- **Change:** Shows how molarity is affected by the reaction.
- **Equilibrium:** Represents molarity when the reaction stabilizes.
An "Undo" feature allows corrections or adjustments as you input the values.
**Credits:**
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Moles of N2 = 1.0 mol
Moles of O2 = 1.5 mol
Volume of flask = 500 ml
= 0.5 L
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