Consider this gas phase equilibrium system: PCl 5 (g) PCl 3 (g)+ Cl 2 (g)$\Delta$Hº rxn = +87.8 kJ/mol. Which of these statements is false?

The Answer of Consider this gas phase equilibrium system: PCl 5 (g) PCl 3 (g)+ Cl 2 (g)$\Delta$Hº rxn = +87.8 kJ/mol. Which of these statements is false?

Consider this gas phase equilibrium system: PCl 5 (g) PCl 3 (g)+ Cl 2 (g)$\Delta$Hº rxn = +87.8 kJ/mol. Which of these statements is false?

The Answer of Consider this gas phase equilibrium system: PCl 5 (g) PCl 3 (g)+ Cl 2 (g)$\Delta$Hº rxn = +87.8 kJ/mol. Which of these statements is false?

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Consider This Gas Phase Equilibrium System: PCl₅(g) $\Delta$

Question 53

Multiple Choice

Consider this gas phase equilibrium system: PCl₅(g) $Consider this gas phase equilibrium system: PCl5(g) PCl3(g) + Cl2(g) \Delta Hºrxn = +87.8 kJ/mol. Which of these statements is false? A) Increasing the system volume shifts the equilibrium to the right. B) Increasing the temperature shifts the equilibrium to the right. C) A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right. D) Decreasing the total pressure of the system shifts the equilibrium to the right. E) Increasing the temperature causes the equilibrium constant to increase.$
PCl₃(g) + Cl₂(g) $\Delta$ Hº_rxn = +87.8 kJ/mol.
Which of these statements is false?

A) Increasing the system volume shifts the equilibrium to the right.
B) Increasing the temperature shifts the equilibrium to the right.
C) A catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to the right.
D) Decreasing the total pressure of the system shifts the equilibrium to the right.
E) Increasing the temperature causes the equilibrium constant to increase.

Correct Answer: