For a given reaction, `DeltaH=35.5kJ*mol^(-1)` and `DeltaS=83.6J*mol^(-1)`. The reaction is spontaneous at (assume that `DeltaH and DeltaS` do not vary with temperature)-

For a given reaction DeltaH=35.5kJmol^(-1) and DeltaS=83.6JK^(-1)mol^(-1) .The reaction is spontaneous at :(Assume that DeltaH and DeltaS do no vary with temperature)

For a given reaction, DeltaH = 35.5 kJ mol^(-1) and Delta S = 83.6 JK^(-1) mol^(-1) . The reaction is spontaneous at (Assume that DeltaH and DeltaS do not vary with temperature)

For a given reaction DeltaH="35.5 k Jmol"^(-1) and DeltaS="83.6 Jk"^(-1)"mol"^(-1) . The reaction is spontaneous at (Assume that DeltaH and DeltaS) do not vary with temperature)

For a given reaction , Delta H = 3.5 kJ mol^(-1) and Delta S = 83.6 J * K^(-1) mol^(-1) . The reaction is spontaneous at (assume DeltaH and Delta S do not vary with temperature) -

For a given reaction, DeltaH=35.5 KJ "mol"^(-1) and DeltaS=83.6 JK^(-1) "mol"^(-1) . The reaction is spontaneous at: (Assume that DeltaH and deltaS so not vary with temperature)