Question

For a certain reaction, the change in Enthalpy is negative and the change in Entropy is positive at a temperature of 300K: ΔH < 0, and TΔS > 0. Question 1: Is ΔG = ΔH – TΔS positive or negative? Question 2: Is it a spontaneous reaction or not?

a) ΔG > 0, Non-spontaneous
b) ΔG < 0, Spontaneous
c) ΔG > 0, Spontaneous
d) ΔG < 0, Non-spontaneous

Answer 1

ΔG is calculated using the equation ΔG = ΔH - TΔS, where negative ΔH and positive TΔS indicate that ΔG might be negative.

Step-by-step explanation:

The Gibbs free energy (ΔG) can be determined using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy and ΔS is the change in entropy. In this case, ΔH is negative and TΔS is positive since the temperature is 300K.

For Question 1, the value of ΔG can be determined by subtracting TΔS from ΔH. Since both ΔH and TΔS have opposite signs, the value of ΔG will depend on which term has a greater magnitude.

For Question 2, a reaction is spontaneous if ΔG is negative. Therefore, if ΔG is less than zero, the reaction is spontaneous. Based on the given information, the correct answer is option b) ΔG < 0, Spontaneous.