5. a. Consider this gas phase equilibrium system: PCls(g)PCls(g) + Cl(g) AH-+87.

Question

5. a. Consider this gas phase equilibrium system: PCls(g)PCls(g) + Cl(g) AH-+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. catalyst speeds up the approach to equilibrium and shifts the position of equilibrium to t 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. b. Consider this gas phase equilibrium system 2SO2(g) + O2(g) 2SO3(g), ??"m-:-198 kJ/mol If the volume of the system is compressed at constant temperature, what change will oc position of the equilibrium? A. A shift to produce more SO2 B. A shift to produce more O2 C. No change D. A shift to produce more SO

Explanation / Answer

5. A) The false statement is option D. Because decreasing pressure leads to backward reaction..

B) No change. Because the total system(reactants and products ) volume is decreasing. So neither decrease nor increase.

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