For the processes `K^+(g) overset(I)(to)K(g) overset(II)(to)K(s) `

Options

A. energy is released in (I) and absorbed in (II)
B. energy is absorbed in (I) and released in (II)
C. energy is absorbed in both the processes
D. energy is released in both the processes

Answer

To solve the question regarding the processes \( K^+(g) \overset{(I)}{\to} K(g) \overset{(II)}{\to} K(s) \), we need to analyze both processes step by step.

### Step 1: Analyze Process I - \( K^+(g) \to K(g) \)

In this step, a potassium ion \( K^+ \) in the gaseous state is gaining an electron to become neutral potassium \( K \) in the gaseous state. This process is known as electron affinity.

- **Energy Change**: When an ion gains an electron, energy is typically released. This is because the electron is attracted to the positively charged ion, leading to a more stable configuration. Therefore, the energy change for this process is negative.

### Step 2: Analyze Process II - \( K(g) \to K(s) \)

In this step, potassium in the gaseous state is being converted to solid potassium. This process is known as condensation or sublimation (depending on the context).

- **Energy Change**: When a gas condenses into a solid, energy is released as well. The gaseous atoms lose kinetic energy and come together to form a solid structure, which is a more ordered state. Thus, the energy change for this process is also negative.

### Conclusion

Both processes involve the release of energy. Therefore, the overall answer is that energy is released in both processes.

### Final Answer:
Energy is released in both processes.

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