Import Question JSON

$\text{Hint: For spontaneous reaction } \Delta\text{G value is negative}$ $\text{Step 1: Understand the relationship between Gibbs free energy change (}\Delta\text{G) and spontaneity}$ $\text{Gibbs free energy (G) is a thermodynamic potential that measures the maximum reversible work that a system can perform at constant temperature and pressure. The change in Gibbs free energy (}\Delta\text{G) provides a criterion for determining whether a process will occur spontaneously.}$ $\text{Step 2: Examine each statement and determine its correctness}$ $\text{Statement 1: }\Delta\text{G is zero for a reversible reaction.}$ $\text{Analysis: When a system is at equilibrium, }\Delta\text{G = 0. A reversible reaction at equilibrium has equal rates of forward and reverse reactions, and there is no net change in the composition of the system. Therefore, }\Delta\text{G = 0 for a system at equilibrium. This statement is correct.}$ $\text{Statement 2: }\Delta\text{G is positive for a spontaneous reaction.}$ $\text{Analysis: A spontaneous process is one that occurs naturally without external intervention. For a process to be spontaneous at constant temperature and pressure, }\Delta\text{G must be negative (}\Delta\text{G < 0). A positive }\Delta\text{G indicates a non-spontaneous process. Therefore, this statement is incorrect.}$ $\text{Statement 3: }\Delta\text{G is negative for a spontaneous reaction.}$ $\text{Analysis: As explained above, a negative }\Delta\text{G (}\Delta\text{G < 0) indicates that a process is spontaneous at constant temperature and pressure. This statement is correct.}$ $\text{Statement 4: }\Delta\text{G is positive for a non-spontaneous reaction.}$ $\text{Analysis: A non-spontaneous process will not occur naturally and requires input of energy or work. For such processes, }\Delta\text{G is positive (}\Delta\text{G > 0). This statement is correct.}$ $\text{Step 3: Identify the incorrect statement}$ $\text{Based on the analysis above, statement 2 is incorrect because it contradicts the fundamental principle that spontaneous processes have negative }\Delta\text{G values, not positive ones.}$ $\text{Therefore, the answer is option 2: }\Delta\text{G is positive for a spontaneous reaction.}$ $\text{To summarize the correct relationships:}$ $\text{• }\Delta\text{G < 0: Spontaneous process}$ $\text{• }\Delta\text{G > 0: Non-spontaneous process}$ $\text{• }\Delta\text{G = 0: System at equilibrium}$