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?

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 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 298 K 2A + B to C DeltaH = 40 kJ "mol"^(-1) and DeltaS = 0.2 kJ K^(-1) "mol"^(-1) . At what temperature will the reaction beccomes sponatneous 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?

For the reactions at 298 K, 2A + B to 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 considering Delta H and Delta S to be constant over the temperature range ?