A mixture of ideal gases is cooled up to liquid helium temperature `(4.22 K)` to form an ideal solution. Is this statement true or false? Justify your answer in not more than two lines.

Explanation

To determine whether the statement "A mixture of ideal gases is cooled up to liquid helium temperature (4.22 K) to form an ideal solution" is true or false, we can analyze the behavior of gases at such low temperatures.

### Step-by-Step Solution:

1. **Understanding Ideal Gases**: Ideal gases are hypothetical gases that perfectly follow the ideal gas law (PV = nRT) under all conditions. However, no real gas behaves perfectly as an ideal gas.

2. **Behavior at Low Temperatures**: When gases are cooled to very low temperatures, such as 4.22 K (the temperature of liquid helium), they exhibit behaviors that deviate from ideal gas behavior. At these temperatures, intermolecular forces become significant.

3. **Intermolecular Forces**: In the case of real gases, attractive forces between molecules can no longer be ignored. These forces lead to deviations from the ideal gas behavior, and the assumption that gas particles do not interact is no longer valid.

4. **Conclusion**: Therefore, a mixture of ideal gases cannot be cooled to form an ideal solution at such low temperatures because the conditions necessary for ideal behavior (no intermolecular forces) do not hold true. Thus, the statement is **false**.

### Final Answer:
The statement is **false** because at low temperatures, intermolecular forces become significant, and ideal gas behavior cannot be maintained.