Question

1) Which of the following describes the relationship between standard free energy and spontaneity?

A-The more positive the value of ?G?, the more spontaneous the process.

B-The more negative the value of ?G?, the more spontaneous the process.

C-When the value of ?G? is zero, the reaction is spontaneous.

D-When the value of ?G? is equal to zero, the reaction is nonspontaneous.

2) A system is observed to spontaneously undergo a change. This change is accompanied by a decrease in the system’s entropy. Has the second law of thermodynamics been violated?

A-No, because the surroundings must have experienced an entropy decrease that is numerically greater than the entropy decrease experienced by the system.

B-No, because the surroundings must have experienced an entropy increase that is numerically greater than the entropy decrease experienced by the system.

C-No, because the surroundings must have experienced an entropy decrease that is numerically smaller than the entropy decrease experienced by the system.

D-No, because the surroundings must have experienced an entropy increase that is numerically smaller than the entropy decrease experienced by the system.

Suppose an ice cube melts in a cup of water. What is the direction of energy flow?

A-From the ice to the water

B-From the water to the ice

C-No net change in energy flow

D-it is impossible to tell.