Which statement about the following equilibrium is correct?2SO2 (g) + O2(g) ⇌ 2SO3(g) ΔH= - 395 KJ/ mole
Correct answer: A. The value of falls K, with rise in temperature
- A. The value of falls K, with rise in temperature
- B. The value of Kp falls with an increase in pressure
- C. The value of K is equal to Kp
- D. The value of K remains constant with rise in temperature.
Explanation
Kp equals the partial pressure of gases at the product side upon the partial pressure of gases at the reactant side. Increasing the temperature favors the reactant side as the backward reaction in this case is endothermic.The shift of equilibrium to reactant side causes the partial pressure of gases of reactant side to increase and pressure at product side to decrease. This in turn causes the value of Kp to fall.
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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