Which statement about the following equilibrium is correct? 2SO2 (g) + O2(g) ⇌ 2SO3(g) ΔH= - 395 KJ/ mole
Correct answer: A. The value of Kp falls, with a rise in temperature
- A. The value of Kp falls, with a rise in temperature
- B. The value of Kp falls with an increase in pressure
- C. The value of Kc is equal to Kp
- D. The value of Kc remains constant with rise in temperature.
Explanation
The reaction is exothermic, With increase in temperature the reaction moves towards the reactants side increasing the partial pressure of reactants, thus the partial pressure of products decreases and the value of Kp decreases
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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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