Consider the following reaction.
2 answers:
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Answer:
True
Explanation:
Resonance is a concept that was introduced when it was not possible to represent a compound with a single Lewis structure. Lewis formulas represent localized electrons, either shared by two atoms in a covalent bond or as non-shared electrons belonging to a given atom. Certain organic compounds, especially those containing multiple bonds can be described by more than one Lewis structure. In these cases, the true Lewis structure has an electronic distribution that is a "hybrid" of all possible Lewis structures of that molecule. Each of Lewis's structures is known as resonance or canonical forms and they are related to each other by a double-headed arrow, where all possible positions of electrons in that molecule are represented.
This type of compound has multiple bonds (double or triple) where electrons are not fixed, but move quickly between atoms, "resonating" between the different Lewis structures. For this reason, when a resonance hybrid has a negative charge, this charge moves between the different resonant structures.
Many times, an intermediate Lewis structure is drawn, with dotted lines, simulating approaching the real structure of the compound, and where this phenomenon of electron and charge mobility can be observed. For example, as we can observe in the ozone resonance image.
Answer:
V₂ = 16.5 L
Explanation:
To solve this problem we use <em>Avogadro's law, </em>which applies when temperature and pressure remain constant:
V₁/n₁ = V₂/n₂
In this case, V₁ is 22.0 L, n₁ is [mol CO + mol NO], V₂ is our unknown, and n₂ is [mol CO₂ + mol N₂].
- n₁ = mol CO + mol NO = 0.1900 + 0.1900 = 0.3800 mol
<em>We use the reaction to calculate n₂</em>:
2CO(g) + 2NO(g) → 2CO₂(g) + N₂(g)
- mol CO₂:
0.1900 mol CO * 0.1900 mol CO₂
- mol N₂:
0.1900 mol NO * 0.095 mol N₂
- n₂ = mol CO₂ + mol N₂ = 0.1900 + 0.095 = 0.2850 mol
Calculating V₂:
22.0 L / 0.3800 mol = V₂ / 0.2850 mol
V₂ = 16.5 L