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For the following reaction, the reactants are the favored species at equilibrium. Classify each of the reactants and the products based on their strength as Bronsted-Lowry acids or bases.
HCN + C9H7N --><-- CN- + C9H7NH+
HCN
C9H7NH+
C9H7N
CN-
Stronger Bronsted-LowrTy acid
Weaker Bronsted-Lowry acid
Stronger Bronsted-Lowry base
Weaker Bronsted-Lowry base

Respuesta :

At equilibrium, HCN is weaker Bronsted-Lowry acid, C₉H₇NH⁺ is stronger Bronsted-Lowry acid, C₉H₇NH is weaker  Bronsted-Lowry base and CN⁻ is stronger Bronsted-Lowry base.

CN⁻ + C₉H₇NH⁺ → HCN + C₉H₇N

Products are favored. So, CN⁻ accepted the proton instead of C₉H₇N and C₉H₇NH⁺ lost its proton instead of HCN.

 C₉H₇NH⁺ - stronger Bronsted-Lowry acid

 C₉H₇N - weaker  Bronsted-Lowry base

 HCN - weaker Bronsted-Lowry acid

 CN⁻ - stronger Bronsted-Lowry base

So, at equilibrium, HCN is weaker Bronsted-Lowry acid, C₉H₇NH⁺ is stronger Bronsted-Lowry acid, C₉H₇NH is weaker  Bronsted-Lowry base and CN⁻ is stronger Bronsted-Lowry base.

To learn more about  Bronsted-Lowry acids or bases, Here :

https://brainly.com/question/14407412?referrer=searchResults

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