What is the entropy change for the mixing of two ideal gases at constant tempera

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Question: What is the entropy change for the mixing of two ideal gases at constant temperature?

Options:

Correct Answer: R ln(2)

Solution:

The entropy change for the mixing of two ideal gases at constant temperature is ΔS = nR ln(2) for equal moles of each gas.

What is the entropy change for the mixing of two ideal gases at constant temperature?

What is the entropy change for the mixing of two ideal gases at constant temperature?

Step 1: Understand that entropy is a measure of disorder or randomness in a system.
Step 2: Recognize that when two ideal gases mix, the overall disorder of the system increases.
Step 3: Identify that we are considering two gases with equal amounts (moles) for simplicity.
Step 4: Recall the formula for the change in entropy (ΔS) when mixing two ideal gases at constant temperature: ΔS = nR ln(2).
Step 5: In this formula, 'n' represents the number of moles of one gas, 'R' is the ideal gas constant, and 'ln(2)' is the natural logarithm of 2.
Step 6: Since we have equal moles of each gas, we can use 'n' for one gas and the formula gives us the total entropy change for the mixing process.

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