At what temperature does a reaction become spontaneous if ΔH = 50 kJ and ΔS = 0.

At what temperature does a reaction become spontaneous if ΔH = 50 kJ and ΔS = 0.1 kJ/K?

At what temperature does a reaction become spontaneous if ΔH = 50 kJ and ΔS = 0.1 kJ/K?

Step 1: Understand the equation for spontaneity: ΔG = ΔH - TΔS.
Step 2: Recognize that a reaction becomes spontaneous when ΔG = 0.
Step 3: Set ΔG to 0 in the equation: 0 = ΔH - TΔS.
Step 4: Rearrange the equation to solve for T: T = ΔH / ΔS.
Step 5: Substitute the given values into the equation: T = 50 kJ / 0.1 kJ/K.
Step 6: Perform the division: 50 kJ divided by 0.1 kJ/K equals 500 K.
Step 7: Conclude that the temperature at which the reaction becomes spontaneous is 500 K.

Gibbs Free Energy – The relationship between enthalpy (ΔH), entropy (ΔS), and temperature (T) in determining the spontaneity of a reaction through the Gibbs free energy equation (ΔG = ΔH - TΔS).
Spontaneity of Reactions – Understanding that a reaction is spontaneous when ΔG is negative, which can be determined by the values of ΔH and ΔS.
Temperature Dependence – Recognizing how temperature influences the spontaneity of a reaction based on the signs and magnitudes of ΔH and ΔS.