For N2 + 3H2 ⇌ 2NH3; ∆H = Negative, then
Correct answer: B. Kp = Kc (RT)-2
- A. Kp = Kc
- B. Kp = Kc (RT)-2
- C. Kp = Kc RT
- D. Kp = Kc (RT)-1
Explanation
Option B is correct.In the reaction N2 + 3H2 <=> 2NH3. There are 4 moles of gas on the reactants side and 2 moles of gas on the products side. This means that Δn = -2. Substituting the values of Δn and R into the equation, we get: Kp = Kc(RT)-2 Therefore, the equilibrium constant, Kp, is equal to the equilibrium constant, Kc, multiplied by the square of the product of R and temperature. In conclusion, for the reaction N2 + 3H2 <=> 2NH3, Kp = Kc (RT)-2.
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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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