InterviewSolution
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InterviewSolution
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for the exothermic formation of sulphur trioxide from sulphur dioxide. And oxygen in the gas phase: `2SO_(2)(g) + O_(2)(g) hArr 2SO_(3) (g)` `K_(p) =40 .5 atm^(-1) at 900 K and Delta H =- 198 kJ` (i) Write the expression for the equilibrium constant for the reaction. (ii) At room temperature `(~~300 K)` will `K_(p)` be greater than less than or equal to `K_(p)` at 900 K . (iii) How will the equilibrium be affected if the volume of the vessel contaning the three gases is reduced, keeping the termperature constant ? What happens ? (iv) What is the effect of adding 1 mole of He (g) to a flask containing `SO_(2),O_(2)` and `SO_(3)` at equilibrium at constant temperatrue ? |
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Answer» (i) The expression for the equilibrium constant `(K_(p))` for the reaction is : `K_(p) =(P_(SO_3)^(2)(g))/(P_(SO_2)^(2)(g)xxP_(O_(2)))=40.5 atm^(-1)` (ii) the forward reaction is exothermic and the backward reaction is endothermic in nature. Therefore ,the increase in temperature favour the backward reaction. This means that the `K_(p)` at 300 K will be greater than the value at 900K. |
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