JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
For the reaction, \(2S{O_2}{\kern 1pt} (g)\, + \,{O_2}\,(g)\, \to \,2S{O_3}\,(g)\) \({\Delta _H}\, = \, - 57.2\,kJ\,mo{l^{ - 1}}\) and \({K_C} = 1.7\, \times \,{10^{16}}\) Which of the following statement is \(INCORRECT\) ?
- A The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
- B The equilibrium will shift in forward direction as the pressure increase.
- C The equilibrium constant decreases as the temperature increases.
- D The addition of inert gas at constant volume will not affect the equilibrium constant.
Answer & Solution
Correct Answer
(A) The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
Step-by-step Solution
Detailed explanation
In option \((B)\,-\,\Delta n_g\) is \(-ve\) therefore increase in pressure will bring reaction in forward direction. In option \((C)-\) as the reaction is exothermic therefore increase in temperature will decrease the equilibrium constant. In option \((D)-\) Equilibrium constant…
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