Which of the following conditions will ensure that a chemical reaction will definitely proceed in the forward direction, toward products? a. ΔH>0b. ΔS>ΔH/Tc. ΔSsys>0d. ΔSsurr>ΔSsyse. ΔH<0

When ΔS > ΔH / T, then the reaction will proceed forward

Explanation:

The entity that determines the whether a reaction will occur on its own in the forward direction (Spontaneity or Feasibility) is Gibb's free energy. Gibb's free energy is the energy available to do work. It is denoted as 'G'. It cannot be easily measured. The change (ΔG) can only be measured. ΔG = ΔH - TΔS

when ΔG is positive, The reaction is not spontaneous (reaction will not occur on its own)

When ΔG is negative, The reaction is spontaneous (reaction will occur on its own)

When ΔG is zero, the reaction is in equilibrium

Option A and E are not correct. ΔH (Enthalpy) cannot determine spontaneity

Option C and D cannot alone determine spontaneity of reaction

For reaction to be spontaneous, TΔS > ΔH

Therefore, ΔS > ΔH/T