The equilibrium concentrations must be identified given S O 3 conversion reaction and enthalpy ( Δ H ) also must be analyzed. Concept Introduction : Concept of equilibrium process : The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed. This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced. Forward Reaction : This type of reaction has involved irreversible , if obtained product cannot be converted back in to respective reactants under the same conditions. Backward Reaction : This type of reaction process involved a reversible , if the products can be converted into a back to reactants. Homogeneous equilibrium : A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or liquid everything is present in the same solution. Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas. Exothermic reaction : This type of chemical reaction release energy by light or heat. Endothermic reaction : This type of chemical reactions that is accompanied by the absorption of heat.

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Chapter 15, Problem 15.78QP

Interpretation Introduction

Interpretation:

The equilibrium concentrations must be identified given SO3 conversion reaction and enthalpy (ΔH) also must be analyzed.

Concept Introduction:

Concept of equilibrium process: The any system at equilibrium subject to change in concentration, temperature, volume or pressure then the system readjusts itself to partly counteract the effect of the applied change and new equilibrium is formed. This equilibrium explain to simple way, a system equilibrium is distributed the system will adjust itself in such a way that the effect of the change will be reduced.

Forward Reaction: This type of reaction has involved irreversible, if obtained product cannot be converted back in to respective reactants under the same conditions. Backward Reaction: This type of reaction process involved a reversible, if the products can be converted into a back to reactants.

Homogeneous equilibrium: A homogeneous equilibrium involved has a everything present in the same phase and same conditions, for example reactions where everything is a gas, or liquid everything is present in the same solution.

Le Chatelier's Principle (Kp): The closed system is an increase in pressure, the equilibrium will shift towards the sides of the reaction with some moles of gas. The decrease in pressure the equilibrium will shift towards the side of the reaction with high moles of gas.

Exothermic reaction: This type of chemical reaction release energy by light or heat.

Endothermic reaction: This type of chemical reactions that is accompanied by the absorption of heat.

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