For a reaction `Delta H=300kJ//"mole",Delta S=300J// "mole K"` . At what temperature the reaction can attain equilibrium

For a chemical reaction, DeltaS = -0.035 kJ//K and DeltaH = -20 kJ . At what temperature does the reaction turn spontaneous?

For a reaction, P+Q rarr R+S . The value of DeltaH^(@) is -"30 kJ mol"^(-1) and DeltaS" is "-"100 J K"^(-1)"mol"^(-1) . At what temperature the reaction will be at equilibrium?

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 at 300 K, 2A + B to C Delta H = 450 kJ mol^(-1) and DeltaS = 0.2 kJ K^(-1) mol^(-1) .At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

For a certain reaction Delta H^(@) =- 224 kJ and Delta S^(@) =- 153 JK At what temperature will it change from spontaneous to non- spontaneous ?

For a reaction A(s)to B(s), DeltaG_(300)^(@)=-2kJ//"mole" Where A and B ar allotropic forms. At what external pressure will the reaction attain equillbrium at 300K, if specific volume of A and B are 10mL//g and 15mL//g respectively and molar mass of A is 40g: