I believe the answer is c I just wanted to make sure.

What can help overcome a positive enthalpy of solution and allow a solid solute to dissolve in water?
A. A decrease in entropy
B. A large amount of energy released
C. An increase in entropy
D. A large amount of energy absorbed

I agree

So do I

Ah, it seems you've stumbled upon a chemistry question! Let me inject a bit of humor to help brighten your learning experience.

Well, well, well... looks like we have a solid solute trying to dissolve in water. It's like a little fish trying to swim in the vast ocean! So, how can this little fish overcome its positive enthalpy of solution and dive into the watery depths?

Option A: A decrease in entropy. Hmm, that's like trying to stuff a clown back into a tiny car. It just doesn't work! So, this option is out of the picture.

Option B: A large amount of energy released. Well, well, well, who doesn't love fireworks? But in this case, we're talking about dissolving, not exploding. So, let's move on.

Option C: An increase in entropy. Now we're talking! Picture the solute molecules doing a lively dance party in the water, causing chaos and an increase in disorder. It's like a circus show in a glass! This option is looking mighty promising.

Option D: A large amount of energy absorbed. Hmm, absorbing energy is like a clown trying to swallow an entire watermelon. It's a bit too much to handle. So, let's toss this option aside.

So, my dear friend, the answer you've been clowning around for is C: An increase in entropy. It's the key to dissolving that solid solute in water, turning it into a happy, dissolved fishy!

The correct answer is C. An increase in entropy.

To determine the correct answer, let's analyze the question. It is asking what can help overcome a positive enthalpy of solution and allow a solid solute to dissolve in water. The enthalpy of solution refers to the heat energy released or absorbed when a solute dissolves in a solvent like water.

In this case, a positive enthalpy of solution indicates that the process requires energy to overcome the forces holding the solute together and separate its particles. Conversely, a negative enthalpy of solution signifies that the process releases energy as the solute dissolves.

Now, let's evaluate the options:

A. A decrease in entropy: Entropy refers to the level of disorder within a system. Decreasing the entropy would make the system more ordered, which is not favorable for dissolution.

B. A large amount of energy released: Releasing a large amount of energy is more indicative of a negative enthalpy of solution, where the solute dissolves readily, rather than overcoming a positive enthalpy of solution.

C. An increase in entropy: Increasing the entropy of the system promotes disorder, making it easier for the solute particles to separate and dissolve. Therefore, an increase in entropy can help overcome a positive enthalpy of solution and facilitate solid solute dissolution.

D. A large amount of energy absorbed: Absorbing a large amount of energy would imply an endothermic process, which does not contribute to overcoming a positive enthalpy of solution.

With this analysis, we can conclude that the correct answer is C. An increase in entropy can help overcome a positive enthalpy of solution and allow a solid solute to dissolve in water.