For a hypothetical reaction ,` 3A rarr A_(3)`
`DeltaC_(p) (i n J)=6.0+2.0xx10^(-3)T`
`DeltaH=-20kJ mol^(-1)` at `300K`
The temperature at which reaction neither absorbs nor releases heat is `:`

For the reaction at 298 k,2A +B rarr C, Delta H= 400 KJ mol^(-1) and Delta S=0.2 KJ k^(-1) mol^(-1). At what temperature will the reaction become spontaneous ?

For the reaction at 298 K : 2A +B to C DeltaH="400 KJ mol"^(-1) , DeltaS ="0.2 JK"^(-1) "mol"^(-1) Determine the temperature at which the reaction would be spontaneous .

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.

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 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 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 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.