For a gaseous phase, first order reaction,
`A_((g))rarr B_((g))+2C_((g))` (rate constant `K=10^(-2) time^(-1)`)
in a closed vessel of `2` litre containing `5` moles of `A_((g))` at `27^(@)C`. then correct statements:

The gaseous reaction A_((g)) + B_((g)) hArr 2C_((g)) + D_((g)) + q kJ is most favoured at :

The K_(c) for given reaction will be A_(2(g))+2B_((g))hArrC_((g))+2D_((g))

The equilibrium constant of the reaction A_(2)(g)+B_(2)(g)hArr 2AB(g) at 373 K is 50. If 1 L of flask containing 1 mole of A_(2)(g) is connected to 2L flask containing 2 moles B_(2)(g) at 100^(@)C , the amount of AB produced at equilibrium at 100^(@)C would be

For the reaction A_((g)) + 3B_((g)) hArr 2C_((g)) at 27^(@)C .2 mole of A, 4 moles of B and 6 moles of C are present in 2 lit vessel. If K_(c) for the reaction is 1.2, the reaction will proceed in

For the reaction A_((g)) + 3B_((g)) hArr 2C_((g)) at 27^(@)C .2 mole of A, 4 moles of B and 6 moles of C are present in 2 lit vessel. If K_(c) for the reaction is 1.2, the reaction will proceed in

A first order gas reaction A_2 B_(2 (g)) to 2 A_((g) ) + 2 B_((g)) at the temperature 400^@ C has the rate constant k = 2.0 xx 10^(-4)s^(-1) . What percentage of A_2 B_2 is decomposed on heating for 900 seconds?