Question

Statement 1: An endothermic reaction can be spontaneous
Statement 2: Both the enthalpy and the entropy changes affect the Gibbs free-energy change of the reaction.

• A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1.
  
• B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
  
• C. Statement 1 is correct but Statement 2 is not correct.
• D. Statement 1 is not correct but Statement 2 is correct.
• E. Both the Statement 1 and Statement 2 are not correct.

Answer 1

Answer: (B)

Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.

For a spontaneous reaction :

$△G\to (-)ve$

i.e. $△H-T△S\to (-)ve$

$△G$ can be negative if :

a) $△H\to (-)ve$

$△S\to (+)ve$

b)$△H\to (+)ve$

$△T\to (+)ve$

$T△S>△H$

Hence, statement 1 is correct.

eg- ice is melting at room temperature

Also, statement 2 is correct as change in gibbs energy$\left(△G\right)$ depends on enthalpy change $\left(△H\right)$ and entropy change$\left(△S\right)$

Statement 2 doesn't explain statement 1

eg- ice cube melts at room temperature because of increase of entropy overcomes the change to a higher energy state.

Hence, Statement 2 is not the correct explanation of statement 1

The option is B.