Equação de van 't Hoff

A equação de van 't Hoff, em termodinâmica química, relaciona a variação da constante de equilíbrio (K) com a variação da temperatura, proporcional a diferença de entalpia padrão dividido pelo quadrado da temperatura. Esta equação foi proposta inicialmente por Jacobus Henricus van 't Hoff.

Se se assume que o calor da reação, entalpia, não varia com a temperatura, a resolução desta equação diferencial é conduzida por:

Nesta equação é a constante de equilíbrio da temperatura absoluta e é a constante de equilíbrio da temperatura absoluta . é a variação de entalpia e é a constante universal dos gases perfeitos.

Considerando as relações entre energia de Gibbs, Entalpia, Entropia e a constante de equilíbrio K a pressão constante, temos:

( e ),

a equação de Van't Hoff também poderia ser descrita da seguinte maneira:

Portanto, ao representar valores de logaritmo natural da constante de equilíbrio medidos pelo equilíbrio pelo inverso da temperatura se obtém uma linha reta, cuja pendente negativa é igual a variação da entalpia dividida entre a constante dos gases e a ordenada na origem é igual a variação de entropia dividida entre a constante dos gases.

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