A) increasing the pressure
B) decreasing the temperature
C) adding some Hz
D) All of the above
Correct Answer: D
Solution :
Key Idea According to Le-Chateliers principle ?If a system in equilibrium is subjected to change of concentration, temperature or pressure. The equilibrium shifts in a direction that tends to undo the effect of the change imposed.? Conclusion 1.If in a reaction in equilibrium, the concentration of any reactant is increased the equilibrium shifts in the forward direction. 2.Exothermic reactions are favoured by low temperature whereas endothermic reactions are favoured by high temperature. 3.Low pressure favours those reactions which take place with increase in total number of moles. High pressure favours those reactions which take place with decrease in total number of moles. However, pressure has no effect on an equilibrium reaction which proceeds with no change in total number of moles. For the gas phase reaction \[\underset{\underbrace{1\,mole\,\,\,\,\,\,\,1\,mole}_{2\,\,mole}}{\mathop{{{C}_{2}}{{H}_{4}}+{{H}_{2}}}}\,\underset{1\,\,mol}{\mathop{{{C}_{2}}{{H}_{6}}}}\,\,\,\,(\Delta H=-32.7\,kcal)\] This reaction is exothermic and number of moles decrease. Therefore, favourable condition for the formation \[{{C}_{2}}{{H}_{6}}\] are 1.Low temperature 2.High pressure 3.Excess of \[{{C}_{2}}{{H}_{4}}\] and \[{{H}_{2}}\].
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