The reaction PCl5( s) ⇌PCl3( g)+Cl2( g) is in equilibrium. If the equilibrium concentration of P

step 1 In this problem, I can write the value of KC is equal to PCL3, CL2, PCL5. So as the value of PCL

The reaction PCl5( s) ⇌PCl3( g)+Cl2( g) is in equilibrium....

The reaction $\mathrm{PCl}_5(\mathrm{~s}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$ is in equilibrium. If the equilibrium concentration of $\mathrm{PCI}_3$ $(\mathrm{g})$ is doubled, then concentration of $\mathrm{Cl}_2(\mathrm{~g})$ would become (a) $1 / 2$ of its initial value (b) $1 / 4$ of its initial value (c) four times of its initial value (d) two times of its initial value

The reaction $\mathrm{PCl}_5(\mathrm{~s}) \rightleftharpoons \mathrm{PCl}_3(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g})$ is in equilibrium. If the equilibrium concentration of $\mathrm{PCI}_3$ $(\mathrm{g})$ is doubled, then concentration of $\mathrm{Cl}_2(\mathrm{~g})$ would become
(a) $1 / 2$ of its initial value
(b) $1 / 4$ of its initial value
(c) four times of its initial value
(d) two times of its initial value

Key Concepts

Reaction Quotient

The reaction quotient (Q) is calculated in the same way as the equilibrium constant but for any set of conditions, not just at equilibrium. By comparing Q to K, one can determine the direction in which the system will shift to reach equilibrium: if Q is greater than K, the reaction will shift toward the reactants, and if Q is less than K, it will shift toward the products.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium experiences a disturbance (such as a change in concentration, temperature, or pressure), it will adjust its position to counteract the change and re-establish equilibrium. This principle helps predict the direction in which the reaction will shift in response to the imposed change.

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the forward and reverse reaction rates are equal, resulting in constant concentrations of reactants and products. It is a dynamic balance that persists as long as the conditions (temperature, pressure, etc.) remain unchanged.

Equilibrium Constant

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium. In heterogeneous equilibria, such as those involving solids and gases, the concentrations of pure solids are omitted from the expression, making K depend only on the gaseous or aqueous species.

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