[2SO_(2)+O_(2)rightleftharpoons2SO_(3)],[" Starting with "2mol" of "SO_(2)" and "1mol" of "O_(2)" in "1],[" L flask,mixture required "0.4molMnO_(4)^(-)" in acidic "],[" medium,the value of "K_(C)" in L mol "^(-1)for" above "],[" reaction 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

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

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 :

5 mol of Fe_(2)(C_(2)O_(4)) is oxidised by x mol of K_(2)Cr_(2)O_(7) in acidic medium, calculate the value of x ?

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

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