A chemist is planning to study a chemical equilibrium for which no measured explicit thermodynamic values are available.However, the reaction involves common chemical species.What information could a chemist use to make predictions about the equilibrium?

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Quizplus · Accepted Answer

All the options provided are valid methods for predicting chemical equilibrium when explicit thermodynamic values are not available. Option A involves using known equilibrium constants of related reactions, which can be combined through Hess's Law to predict the new equilibrium. Options B and C suggest using standard Gibbs free energy ($\Delta G^\circ$) and standard enthalpy ($\Delta H^\circ$) and entropy ($S^\circ$) changes for the reactants and products, which are fundamental thermodynamic quantities that can predict the direction of a reaction and its equilibrium position.

A Chemist Is Planning to Study a Chemical Equilibrium for Which