Answer:
- a) 2N₂O(g) → 2N₂(g) + O₂(g)
Explanation:
Arrange the equations in the proper way for better understanding.
T<em>he reaction between nitrogen and oxygen is given below:</em>
<em />
- <em>2N₂(g) + O₂(g) → 2N₂O(g)</em>
<em />
<em>We therefore know that which of the following reactions can also occur?</em>
<em />
- <em>a) 2N₂O(g) → 2N₂(g) + O₂(g)</em>
- <em>b) N₂(g) + 2O₂(g) → 2NO₂(g)</em>
- <em>c) 2NO₂(g) → N₂(g) + 2O₂(g)</em>
- <em>d) None of the Above</em>
<h2>Solution</h2>
Notice that the first equation, a) 2N₂O(g) → 2N₂(g) + O₂(g), is the reverse of the original equation, 2N₂(g) + O₂(g) → 2N₂O(g).
The reactions in gaseous phase are reversible reactions that can be driven to one or other direction by modifying the conditions of temperature or pressure.
Thus, the equilibrium equation would be:
Which shows that both the forward and the reverse reactions occur.
Whether one or the other are favored would depend on the temperature and pressure: high temperatures would favor the reaction that consumes more heat (the endothermic reaction) and high pressures would favor the reaction that consumes more moles.
Thus, by knowing that one of the reactions can occur you can conclude that the reverse reaction can also occur.
The boiling point of oxygen is higher than nitrogen's boiling
The reason the boiling point of O2 is higher is not because of increased van der Waals interactions, but simple physics. The mass of a molecule of O2 is greater than that of a molecule of N2, so the molecule of O2 traveling at a speed sufficient to break out of the liquid phase has a greater kinetic energy than an analogous N2 molecule.
The net effect is that more energy must be distributed throughout a sample of O2 to achieve a given vapor pressure (in this case equal to atmospheric pressure) than for a sample of N2. More energy means greater temperature.
Water is the component that is produced here.
Answer:
Characteristics of Group
Explanation:
The elements of a group show similar chemical properties but there is a gradual variation in the physical properties of the elements in a group.
