A reaction at 300 K with `DeltaG^(@)` `=- 1743 J//mol` consister of 3 mole of A(g), mole of B(g) and 3 mole of C (g). If A, B and C(g) . If A,B and C are equal are in equilibrium in 1 liter container then the reaction may be
`[Given :2=e^(0.7), R=8.3 J//K-mol]`

A reaction at 400 K with approximate DeltaG^(@)=3207 J//"mole" , consists of 4 mole of substance A, 2 mole of substance B and 3 mole of substance C at equilibrium in 1 litre container, then which of the following is correctly balanced reaction ? [Take : log 3 =0.48, log 2= 0.3 in x =2.30 log x R=8.3 J//"mole"//K ]

3 mols of A and 1 mol of B are mixed in a 1L container. The reaction taking place is A(g)+B(g) iff 2C(g) . If 1.5 mol of C is formed at equilibrium, the K_(c) of the reaction is

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

1 mole of 'A' 1.5 mole of 'B' and 2 mole of 'C' are taken in a vessel of volume one litre. At equilibrium concentration of C is 0.5 mole /L .Equilibrium constant for the reaction , A_((g))+B_((g) hArr C_((g)) is

1 mole of 'A' 1.5 mole of 'B' and 2 mole of 'C' are taken in a vessel of volume one litre. At equilibrium concentration of C is 0.5 mole /L .Equilibrium constant for the reaction , A_((g))+B_((g) hArr C_((g)) is