Which reaction, with the following value of `DeltaH` and `DeltaS` at `350K` is spontaneous and endothermic?
`DeltaHKJmol^(-1)DeltaSKJmol^(-1)DeltaHKJ mol^(-1)DeltaSKJ mol^(-1)`

Which reaction, with the following values of DeltaH, DeltaS at 400K is spontaneous and endothermic ?

From the following values of DeltaH and DeltaS , decide whether or not these reaction are feasible at 298 K. Reaction A : DeltaH =- 10.5 xx 10^3 J mol^(-1), DeltaS = + 31J K^(-1) mol^(-1) Reaction B : DeltaH = - 11.7 xx 10^3 J mol^(-1), DeltaS = - 105 J K^(-1) mol^(-1)

Determine whether the reactions with the following DeltaHandDeltaS values are spontaneous or non-spontaneous. State whether the reactions are exothermin or endothermic. (a) Delta=-110kJ,DeltaS=+40JK^(-1)" at "400K (b) DeltaH=+40kJ,DeltaS=-120JK^(-1)" at "250K

Determine whether reactions With following DeltaH and DeltaS values are spontaneous or non spontaneous. State whether they are exothermic or endothermic. DeltaH = + 40 kj and DeltaS =-120 JK-1 mol-1 at 250K

Determine whether reactions With following DeltaH and DeltaS values are spontaneous or non spontaneous. State whether they are exothermic or endothermic. DeltaH =-110 kj and DeltaS = + 40JK-lmol-1 at 400 K

Calculate the value of DeltaG at 700K for the reaction, nX to mB . Given that value of DeltaH=-113kJ mol^(-1) and DeltaS=-145JK^(-1)mol^(-1).

The values of DeltaH and DeltaS for two reactions are given below: Reaction A : DeltaH =- 10.0 xx 10^(3)J mol^(-1) DeltaS = +30 J K^(-1) mol^(-1) Reaction B: DeltaH =- 11.0 xx 10^(3)J mol^(-1) DeltaS =- 100J K^(-1) mol^(-1) Decide whether these reactions are spontaneous or not at 300K .

The values of DeltaH and DeltaS for two reactions are given below: Reaction A : DeltaH =- 10.0 xx 10^(3)J mol^(-1) DeltaS = +30 J K^(-1) mol^(-1) Reaction B: DeltaH =- 11.0 xx 10^(3)J mol^(-1) DeltaS =- 100J K^(-1) mol^(-1) Decide whether these reactions are spontaneous or not at 300K .

The value of DeltaH and DeltaS for two reactions are given below : Reaction A : DeltaH = -10.5 xx 10^(3) J "mol"^(-1) DeltaS = + 31 J K^(-1) "mol"^(-1) Reaction B : DeltaH = -11.7 xx 10^(3) J "mol"^(-1) DeltaS = -105 J K^(-1) "mol"^(-1) Decide whether these reactions are spontaneous or not at 298 K.

Determine whether the reactions with the following AH and AS values are spontaneous or non-spontaneous. State whether they are exothermic or endothermic: DeltaH =- 40 kj and DeltaS = + 135J K-1 at 300 K DeltaH = -60 kj and DeltaS = -160 JK-1 at 400K