Which of the following conditions will lead to a spontaneous reaction?
Practice Questions
Q1
Which of the following conditions will lead to a spontaneous reaction?
ΔH > 0 and ΔS < 0
ΔH < 0 and ΔS > 0
ΔH > 0 and ΔS > 0
ΔH < 0 and ΔS < 0
Questions & Step-by-Step Solutions
Which of the following conditions will lead to a spontaneous reaction?
Step 1: Understand that a spontaneous reaction is one that occurs naturally without needing extra energy.
Step 2: Learn about ΔG, which is the change in Gibbs free energy. A spontaneous reaction happens when ΔG is less than 0 (ΔG < 0).
Step 3: Know that ΔG can be calculated using the formula: ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.
Step 4: Recognize that if ΔH (enthalpy change) is less than 0 (ΔH < 0), it means the reaction releases heat, which is favorable for spontaneity.
Step 5: Understand that if ΔS (entropy change) is greater than 0 (ΔS > 0), it means the disorder of the system increases, which is also favorable for spontaneity.
Step 6: Conclude that both conditions (ΔH < 0 and ΔS > 0) together will lead to a negative ΔG, resulting in a spontaneous reaction.
