Consider this gas phase equilibrium system:.
PCl5(g) equilibrium arrow PCl3(g) + Cl2
deltaH...
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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 constant to increase
B) increasing the system volume shifts the equilibrium to the right
C) increasing the temperature shifts the equilibrium to the right
D) a catalyst speeds up the approach to equilibrium and shifts the position from equilibrium to the right.
E) decreasing the total pressure of the system shifts the equilibrium to the right.
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Be sure to answer all parts. the following equilibrium constants were determined at 1123 k: c(s) + co2(g) β 2co(g) k'p = 1.30 Γ 1014 co(g) + cl2(g) β cocl2(g) k''p = 6.00 Γ 10β3 calculate the equilibrium constant at 1123 k for the reaction: c(s) + co2(g) + 2cl2(g) β 2cocl2(g) 4.68 Γ 10 9 (enter your answer in scientific notation.) write the equilibrium constant expression, kp:
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