For the reaction at `300K` `A(g) hArr V(g)+S(g)` `Delta_(r) H^(@)=-30kJ //mol`, `Delta_(r)S^(@)=-0.1Kj.k^(-1).mol^(-1)` What is the value of equilibrium constant ?
For the reation at 300 K A(g)hArrV(g)+S(g) Delta_(r)H^(@)=-kJ//mol, Delta_(r)S^(@)=-0.1K^(-1).mol^(-1) What is the value of equilibrium constant ?
For the reaction at A(g) rarr B(g) + E(g), DeltaH^(@) = -30 KJ mol^(-1) , the decrease in standard entropy is 0.1 KJK^(-1)mol^(-1) .The equilibrium constant K for the reaction is ________.
For the reaction, A(g)+B(g) rarr C(g)+D(g), DeltaH^(@) and DeltaS^(@) are respectively, -29.8 kJ mol^(-1) and -0.100 kJ K^(-1) mol^(-1) at 298 K The equilibrium constant for the reaction at 298 K is :
For the reaction at 300K (take R=8JK^-1mole^-1 2A(g)+B(s)rarr2D(g) , Delta U^(0)=-10kJ and Delta S^(0)=-50JK^-1 . Find the value of Delta G^(0)
The reaction, MgO(s) + C(s) to Mg(s) + CO(g), for which Delta_(r)H^(@)= +491.1 " " kJ " " mol^(-1) and Delta_(r)S^(@)= 198.0 JK^(-1)mol^(-1) , is not feasible at 289 K . Temperature above which reaction will be feasible is :
For the hypothetical reaction A_(2)(g) + B_(2)(g) hArr 2AB(g) If Delta_(r)G^(@) and Delta_(r)S^(@) are 20 JK^(-1)mol^(-1) respectively at 200 K. Delta_(r)C_(p) is 20 JK^(-1) mol^(-1) then Delta_(r)H^(@) "at" 400 K is :
