For a reaction `H_(2(g))+I_(2(g))rarr2HI_((g)`, `Delta H=37.5(kJ)/(mol)` and `Delta S=150JK^(-1)mol^(-1)`. The temperature at which the reaction will be at equilibrium is.
`200K`
`250K`
`300K`
`350K`

For a hypothetical reaction A(g) + 3B(g) to 2C(g). Delta H = -100 kJ and Delta S = -200 Jk^(-1) . Then the temperature at which the reaction will be in equilibrium is

A process has Delta H = 8 K J mol^(-1) " and " Delta S = 80JK^(-1) mol^(-1) The temperature at which the process will be in equilibrium is ____________ K.

For the reaction, N_(2)(g) +3H_(2)(g) rarr 2NH_(3)(g) DeltaH =- 95.0 kJ and DeltaS = - 19000 J K^(-1) Calculate the temperature in centigrade at which it will attain equilibrium.

For the reaction Ag_(2)O(s)rarr 2Ag(s)+1//2O_(2)(g) the value of Delta H=30.56 KJ mol^(_1) and Delta S = 66 JK^(-1)mol^(-1) . The temperature at which the free energy change for the reaction will be zero is :-

Delta H and Delta S for the reaction, Ag_(2)O(s)to 2A(s)+(1)/(2)O_(2)(g) , are 30.56 kJ mol^(-1) and 66.0 J mol^(-1) respectively. Calculate the temperature at which this reaction will be at equilibrium. Predict whether the forward reaction will be favoured above or below this temperature.

For the reaction N_(2)(g) + 3H_(2) rarr 2NH_(3)(g) Delta H = - 95.4 kJ and Delta S = -198.3 JK^(-1) Calculate the temperature at which Gibbs energy change (Delta G) is equal to zero. Predict the nature of the reaction at this temperature and above it.

For the reaction N_(2)(g) + 3H_(2) rarr 2NH_(3)(g) Delta H = - 95.4 kJ and Delta S = -198.3 JK^(-1) Calculate the temperature at which Gibbs energy change (Delta G) is equal to zero. Predict the nature of the reaction at this temperature and above it.

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction X_(2)O_(4(l)) rarr 2XO_(2(g)), Delta U= 2.1 "kcal", Delta S= 20 "cal " K^(-1) at 300K, Hence Delta G is