In a reaction `A + B hArrC + D`, the concentration of A, B, C and D (in moles/litre) are `0.5, 0.8, 0.4` and `1.0` respectively. The equilibrium constant is

In a reaction A+Bharr C+D the concentrations of A,B,C and D in (moles/litre) are 0.5, 0.8, 0.4 and 1.0 respectively. The equillibrium constant is

For a reaction 2A+B hArr C+D , the partial pressures of A, B , C and D at equilibrium are 0.5, 0.8, 0.7 and 1.2 atmospheres respectively. The value of K_(p) for this reaction is

For a reaction 2A + B ⇌ C + D , the partial pressure of A, B, C and D at equiliberium are 0.5, 0.8 0.7 and 1.2 atmosphere respectively. The value of k_p for this reaction is :

In the reversible reaction A + B hArr C + D, the concentration of each C and D at equilobrium was 0.8 mole/litre, then the equilibrium constant K_(c) will be

In the reversible reaction A + B hArr C + D, the concentration of each C and D at equilobrium was 0.8 mole/litre, then the equilibrium constant K_(c) will be

For a gaseous equilibrium, A +2B hArr C + 3D the partial pressures of A, B, C and D are found to be 0.20, 0.10, 0.30 and 0.50 atm respectively. Predict the value of equilibrium constant.

On a given condition, the equilibrium concentration of HI , H_(2) and I_(2) are 0.80 , 0.10 and 0.10 mole/litre. The equilibrium constant for the reaction H_(2) + I_(2) hArr 2HI will be