What does a negative ΔG value for a reaction at a specific temperature and pressure indicate?Select one:a.The reaction is at equilibrium.b.The reaction is spontaneous in the forward direction.c.The reaction is non-spontaneous under the given conditions.d.The reaction is spontaneous in the reverse direction.

Which statement is true regarding a process for which ΔH is positive and ΔS is negative? Recall that, for any process: ΔG = ΔH - TΔSSelect answer from the options belowThe process is spontaneous at low temperatures only.The process is not spontaneous at any temperature.The process is spontaneous at all temperatures.The process is spontaneous at high temperatures only.

A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following :Both ΔH and ΔS are negativeBoth ΔH and ΔS are positiveΔH is positive while ΔS is negativeΔH is negative while ΔS is positive

Consider a specific reaction with ΔH° = 66.8 kJ/mol and ΔS° = 105.3 J/mol•K. Assuming that these values do not change with temperature, at what temperature range is the reaction spontaneous in the forward direction?The reaction is spontaneous for temperatures (less than, greater than) T = ________ K.

At constant pressure and temperature, which statement is true?Group of answer choicesAll reactions for which ΔS < 0 are spontaneous.All reactions for which K < 1 are spontaneous.All reactions for which ΔG < 0 are spontaneous.All reactions for which ΔH < 0 are spontaneous.

Consider the reaction described by the chemical equation shown.3C2H2(g)⟶C6H6(l)     ΔH∘rxn=−633.1 kJUse the data from the table of thermodynamic properties to calculate the value of ΔS∘rxn at 25.0 ∘CΔS∘rxn= J⋅K−1Calculate ΔG∘rxnΔG∘rxn= kJIn which direction is the reaction, as written, spontaneous at 25 ∘C and standard pressure?neitherreverseforwardboth