Question

Gaseous dinitrogen tetroxide(N2O4) decoposes to form nitrogen dioxide gas (NO2).

Write a balanced equation for this reaction.

In carrying, out and experiment based on this reaction,2.5L of Dinitrogen Tetroxide were used. How many liters of nitrogen dioxide are produced? temperature and pressure were held constant

Answer 1

Answer 2

Here's the breakdown of the solution:

1. Balanced Chemical Equation

The decomposition of dinitrogen tetroxide (N₂O₄) into nitrogen dioxide (NO₂) is represented by the following balanced chemical equation:

N₂O₄(g) → 2NO₂(g)

2. Volume Relationship

Since the temperature and pressure are held constant, we can apply Avogadro's Law, which states that equal volumes of gases contain equal numbers of molecules (or moles) at the same temperature and pressure.

From the balanced equation, we see that 1 mole of N₂O₄ produces 2 moles of NO₂.  Therefore, the volume of NO₂ produced will be twice the volume of N₂O₄ consumed.

3. Calculating Volume of NO₂

Given that 2.5 L of N₂O₄ were used, the volume of NO₂ produced is:

Volume of NO₂ = 2 * (Volume of N₂O₄) Volume of NO₂ = 2 * 2.5 L Volume of NO₂ = 5.0 L

Therefore, 5.0 liters of nitrogen dioxide (NO₂) are produced.

Answer 3

Balanced Equation:

$${\text{N}}_2{\text{O}}_4\to 2{\text{NO}}_2$$$${\text{N}}_2{\text{O}}_4\to 2{\text{NO}}_2$$

Calculation for NO₂ Produced:

• Given: 2.5 L of ${\text{N}}_2{\text{O}}_4$${\text{N}}_2{\text{O}}_4$ (at constant temperature and pressure).

• From the equation: 1 mole of ${\text{N}}_2{\text{O}}_4$${\text{N}}_2{\text{O}}_4$ produces 2 moles of ${\text{NO}}_2$${\text{NO}}_2$.

• Volume ratio: 1 L of ${\text{N}}_2{\text{O}}_4$${\text{N}}_2{\text{O}}_4$ produces 2 L of ${\text{NO}}_2$${\text{NO}}_2$.

• For 2.5 L of ${\text{N}}_2{\text{O}}_4$${\text{N}}_2{\text{O}}_4$:

  $$2.5\text{L}\times 2=5\text{L}\text{of}{\text{NO}}_2$$$$2.5\text{L}\times 2=5\text{L}\text{of}{\text{NO}}_2$$

Answer:

5 liters of ${\text{NO}}_2$${\text{NO}}_2$ are produced.