If a reaction is exothermic and its entropy change is positive, which statement is true? if a reaction is exothermic and its entropy change is positive, which statement is true? a. the reaction is spontaneous only at higher temperatures. b. the reaction is nonspontaneous at all temperatures. c. the reaction is spontaneous at all temperatures. d. the reaction is spontaneous only at lower temperatures.

Explanation:

The spontaneity of a reaction can be determined by the thermodynamic property named Gibb's free energy or simply free energy (G).

The change in the free energy of a system is defined as the difference between the increase in enthalpy (ΔH) and the product of the temperature (T) times the increase in entropy (ΔS):

The sign of ΔG tells if a reaction is spontaneous according to this:

The question states that a reaction is exothermic, and its entropy change is positive. That means:

Remember that the temperature is stated in absolute scale, so T is always positive.

Hence, ΔG = ΔH - T ΔS = (negative) - T (positive) = (negative) + (negative) = negative.

Conclusion: since ΔG is negative, regardless the temperature, you conclude that the reaction is spontaneous at all temperatures, which is the option c.

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.

m=9

step-by-step explanation: