Question

Which of the following statements is true for the product-favored reaction shown at 25ºC ?

A_(g)   ---> B_(g)   ΔH  = - 20 kJ/mole ΔS = - 26 J/mole•K

		the reaction is enthalpy and entropy driven
		this reaction is at equilibrium at 25ºC
		the reaction is entropy driven
		the reaction is enthalpy driven
		In the reaction, the overall entropy change for the universe is negative

Answer 1

For any reaction to occur the value of ∆G should be negative.

∆G=∆H-T∆S

Here ∆H and ∆S are negative values.

Here the value of ∆H is negative hence it is clear that it is exothermic reaction.

A spontaneous reaction will have positive value of ∆ S.

Here ∆S is also negative.Hence it should be overcome by the ∆H value to proceed the reaction into product side.

Hence the above reaction is enthalpy driven.