To calculate the equilibrium constant values are given the spontaneous and non-spontaneous reaction at 25°C with supporting of equilibrium table values. Concept Introduction: Equilibrium constant : Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction. Spontaneous reaction : This reaction is said to be spontaneous it occurs without being drive by some of outside force. The two driving forces for all chemical reactions , first one is enthalpy and second one is entropy, spontaneous reactions occurs without outside intervention. Non-spontaneous reaction : This type of reaction explain as, endergonic reaction (mean by heat absorption non-spontaneous process) or unfavorable reaction in a chemical reaction in which the standard change in free energy is positive and energy is absorbed.

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Chapter 15, Problem 15.141QP

Interpretation Introduction

Interpretation:

To calculate the equilibrium constant values are given the spontaneous and non-spontaneous reaction at 25°C with supporting of equilibrium table values.

Concept Introduction:

Equilibrium constant: Concentration of the products to the respective molar concentration of reactants it is called equilibrium constant. If the K value is less than one the reaction will move to the left side and the K values is higher (or) greater than one the reaction will move to the right side of reaction.

Spontaneous reaction: This reaction is said to be spontaneous it occurs without being drive by some of outside force. The two driving forces for all chemical reactions, first one is enthalpy and second one is entropy, spontaneous reactions occurs without outside intervention.

Non-spontaneous reaction: This type of reaction explain as, endergonic reaction (mean by heat absorption non-spontaneous process) or unfavorable reaction in a chemical reaction in which the standard change in free energy is positive and energy is absorbed.

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