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Consider this gas phase equilibrium system: PCl5(g) equilibrium arrow PCl3(g) + Cl2 deltaH = +87.8 kJ/mol Which of...

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Chemistry

Consider this gas phase equilibrium system:

PCl5(g) equilibrium arrow PCl3(g) + Cl2
deltaH = +87.8 kJ/mol

Which of these statements are false?
A) increasing the temperature causes the equilibrium constantto increase
B) increasing the system volume shifts the equilibrium to theright
C) increasing the temperature shifts the equilibrium to theright
D) a catalyst speeds up the approach to equilibrium and shiftsthe position from equilibrium to the right.
E) decreasing the total pressure of the system shifts theequilibrium to the right.

Answer & Explanation Solved by verified expert
4.2 Ratings (607 Votes)
Ans false statement d PCl5 g PCl3 g Cl2 g deltaH 878 kJmol delta n moles of products moles of reactants 2 1 1 deltaH ve This is endothermic reaction a true Explanation Endothermic reactions    See Answer
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