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lana [24]
3 years ago
5

Which substance in the reaction serves as the electrophile?'?

Chemistry
1 answer:
jok3333 [9.3K]3 years ago
4 0

Electrophiles are reagents attracted to electrons.

Electrophiles tend to be electron-deficient and carry partial positive charges. They are attracted to species with lone pairs of electrons. For example, protons \text{H}^+ have no electrons and tend to share ones with other species, hence behaving as electrophiles in aqueous reactions. In the reaction between \text{H}^+ and ammonia \text{NH}_3, protons would be attracted to lone electron pairs on nitrogen atoms in ammonia molecules, which carry partial positive charges.

The Lewis Acid-base theory define Acids as species that accept electron pairs in a particular acid-base reaction. Electrophiles, by definition, tend to accept electrons. Lewis acids thus behaves as electrophiles in acid-base reactions. In the previous example, \text{H}^+ demonstrates acidic behavior and can be inferred as an electrophile.

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General Formulas and Concepts:

<u>Thermodynamics</u>

Specific Heat Formula: q = mcΔT

  • <em>q</em> is heat (in J)
  • <em>m</em> is mass (in g)
  • <em>c</em> is specific heat (in J/g °C)
  • ΔT is change in temperature (in °C or K)

Explanation:

<u>Step 1: Define</u>

<em>Identify variables</em>

[Given] <em>c</em> = 0.897 J/g °C

[Given] <em>m</em> = 79 g

[Given] ΔT = 28°C

[Solve] <em>q</em>

<em />

<u>Step 2: Solve for </u><em><u>q</u></em>

  1. Substitute in variables [Specific Heat Formula]:                                             q = (79 g)(0.897 J/g °C)(28 °C)
  2. Multiply [Cancel out units]:                                                                               q = (70.863 J/°C)(28 °C)
  3. Multiply [Cancel out units]:                                                                               q = 1984.16 J

<u>Step 3: Check</u>

<em>Follow sig fig rules and round. We are given 2 sig figs as our lowest.</em>

1984.16 J ≈ 2000 J

6 0
2 years ago
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