`2SO_(2)+O_(2)hArr 2SO_(3)`. Starting with 2 moles `SO_(2)` and 1 mole `O_(2)` in 1L flask, mixture required 0.4 mole `MnO_(4)^(-)` in acidic medium. Hence, `K_9c)` is

2SO_2+O_2 hArr 2SO_3 Starting with 2 mol of SO_2 and 1 mol of O_2 in 1-L flask, mixture required 0.4 mol of MnO_4^- in acidic medium . Find the K_c value

An equilibrium is established SO_2 , O_2 and SO_3 as SO_2(g)+1/2O_(2)(g) hArr SO_3(g) starting with 2 moles SO_2 and 1.5 moles O_2 in 5 litre flask.The equilibrium mixture required 0.4 moles of KMnO_4 in acidic medium.The value of K_C^(@) is :

For the equilibrium 2SO_(2)+O_(2)hArr 2SO_(3) we start with 2 moles of SO_(2) and 1 mole of O_(2) at 3 atm. When equilibrium is attained, pressure changes to 2.5atm. Hence, K_(p) is :

2SO_(2)(g)+O_(2)(g)hArr2SO_(3)(g) Starting with 2 mol of SO_(2) and 1 mol O_(2) in one litre flask. After some time equilibrium established. In another experiment same mol of SO_(2) presetn at equilibrium required 1000 ml 0.4 M KMnO_(4) ub acidic medium. The value of equilibrium constant K_(C) for the reaction is

In the reaction, 2SO_(2) +O_(2) to 2SO_(3) when 1 mole of SO_(2) and 1 mole of O_(2) are made to react to completion