For a reaction
`DeltaH=+29kJ" "mol^(-1),DeltaS=-35KJ^(-1)" "mol^(-1)`
at what temperature, the reaction will be spontaneous?

For the homogeneous reactions: xA+yBtolY+mZ DeltaH=-30kJ" "mol^(-1),DeltaS=-100JK^(-1)" "mol^(-1) At what temperature the reaction is at equilibrium?

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 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?

In the reaction, AtoB+C,DeltaH=25kJ*mol^(-1) and DeltaS=62.5J*K^(-1) . At which temperature the reaction will occur spontaneously at constant pressure?

For the reaction at 298 K, 2A+BtoC 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 constant over the temperature range?

(i) State hess's law. (ii) For the following reaction at 298K 2X+Y to Z DeltaH=300kJ*mol^(-1) and DeltaS=0.2kJ*K^(-1)*mol^(-1) At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?