### Equilibrium of Phosphorus Pentachloride Decomposition**Chemical Reaction:**The decomposition of phosphorus pentachloride (\( \text{PCl}_5 \)) into phosphorus trichloride (\( \text{PCl}_3 \)) and chlorine gas (\( \text{Cl}_2 \)) occurs at high temperatures and is represented by the following chemical equation:\[ \text{PCl}_5(g) \rightleftharpoons \text{PCl}_3(g) + \text{Cl}_2(g) \]**Equilibrium Mixture:**At a specific temperature within a 1.00-L flask, the equilibrium mixture consists of:- 5.72 g of \( \text{PCl}_5 \)- 4.86 g of \( \text{PCl}_3 \)- 3.59 g of \( \text{Cl}_2 \)**Question:**If you add 1.31 g of \( \text{Cl}_2 \), how will the equilibrium be affected?- Shift left- Shift right- No shift will occur*Note:* The addition of chlorine gas (\( \text{Cl}_2 \)) is expected to shift the equilibrium position according to Le Chatelier's Principle. Consider how the system will adjust to the disturbance.

Given reaction : PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)

Phosphorus pentachloride decomposes at high temperatures. PC15 (g) ⇒ PC13 (g) + Cl₂ (g) An equilibrium mixture at some temperature consists of 5.72 g of PC15, 4.86 g of PC13, and 3.59 g of Cl₂ in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur

Phosphorus pentachloride decomposes at high temperatures. PC15 (g) ⇒ PC13 (g) + Cl₂ (g) An equilibrium mixture at some temperature consists of 5.72 g of PC15, 4.86 g of PC13, and 3.59 g of Cl₂ in a 1.00-L flask. a If you add 1.31 g of Cl2, how will the equilibrium be affected? shift left shift right no shift will occur

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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