For the equilibrium reaction `H_(2(g))+I_(2(g))hArr 2HI_((g))`

In the equilibrium reaction CO_(2(g))+C_((s))hArr 2CO_((g)) the partial pressure of CO2 and CO are 0.78 atm and 1.22 atm respectively at equilibrium. Calculate the equilibrium constant

Calculate Deltan_(g) , for the following reactions (i) H_(2(g))+I_(2(g))hArr2HI_((g)) (ii) 2H_(2)O_((g))+2Cl_(2(g))hArr4HCl_((g))+O_(2)((g))

For the reversible reaction N_(2(g))+3H_(2(g))hArr2NH_(3(g))+"Heat" . The equilibrium shifts in forward direction.

If the equilibrium constant for N_(2(g))+O_(2(g))hArr2NO_((g)) is K, the equilibrium constant for 1/2N_(2(g))+1/2O_(2(g))hArrNO_((g)) will be

Two moles of H_(2) and three moles of I_(2) are taken in 2 dm^(3) vessel and heated. If the equilibrium mixture contains 0.8 moles of HI, calculate K_(p) and K_(c) for the reaction H_(2(g))+I_(2(g))hArr 2HI_((g))

For the reaction H_(2(g))+l_(2(g)) hArr 2Hl_((g)) Kc=66.9" at "350^(@)C and 50.0" at "448^(@) . The reaction has