### Equilibrium Analysis in Chemical Reactions#### Consider the following equilibrium reaction:\[ \text{PCl}_5(g) \leftrightarrow \text{PCl}_3(g) + \text{Cl}_2(g) \quad \Delta H = 92 \text{kJ} \]The concentration of \( \text{Cl}_2 \) at equilibrium can be increased by:a. Decreasing the temperature.b. Adding \( \text{PCl}_3 \) to the system.c. Adding \( \text{PCl}_5 \) to the system.d. Increasing the pressure.e. Adding a catalyst.#### Explanation of Options:- **Decreasing the temperature:** This affects the equilibrium position if the reaction is exothermic or endothermic. Since the reaction is endothermic (ΔH = 92 kJ), decreasing the temperature will shift the equilibrium to the left, decreasing \( \text{Cl}_2 \) concentration. - **Adding \( \text{PCl}_3 \):** According to Le Chatelier’s principle, adding a product will shift the equilibrium to the left, decreasing \( \text{Cl}_2 \).- **Adding \( \text{PCl}_5 \):** This will shift the equilibrium to the right, increasing the concentration of \( \text{Cl}_2 \).- **Increasing the pressure:** This depends on the number of moles of gas on each side of the equilibrium. Here, there is an equal number of moles of gas (1 mole of \( \text{PCl}_5 \) equals 1 mole of \( \text{PCl}_3 \) + 1 mole of \( \text{Cl}_2 \)), so pressure change won’t significantly affect the equilibrium position.- **Adding a catalyst:** Catalysts speed up the reaction rate to reach equilibrium faster but do not affect the equilibrium concentrations of reactants and products.In summary, the concentration of \( \text{Cl}_2 \) at equilibrium can be increased by option c: **adding \( \text{PCl}_5 \) to the system**.

So we’ve given the above mentioned equilibrium reaction. We will determine which factor will…

Consider the following equilibrium: PCI5(g) → PC13(g) + Cl2(g) ΔΗ 92 k The concentration of Cl2 at equilibrium may be increased by a. decreasing the temperature. adding PC13 to the system. adding PCI5 to the system. c. increasing the pressure. е. adding a catalyst.

Consider the following equilibrium: PCI5(g) → PC13(g) + Cl2(g) ΔΗ 92 k The concentration of Cl2 at equilibrium may be increased by a. decreasing the temperature. adding PC13 to the system. adding PCI5 to the system. c. increasing the pressure. е. adding a catalyst.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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