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

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) + 3 H_(2) rightarrow 2NH_(3)(g) Delta H = -85.4 kJ and Delta S = - 188.3 Jk^(-1) Calculate the temperature at which Gibs 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 N_(2)(g) + 3 H_(2) rightarrow 2NH_(3)(g) Delta H = -85.4 kJ and Delta S = - 188.3 Jk^(-1) Calculate the temperature at which Gibs 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, 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, 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, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g), Delta H = -95.2 kJ and Delta S = -198.1 JK^(-1) . Calculate the temperature at which Gibb's energy change of the reaction (Delta G) becomes equal to zero.