Questions 1) and 2) refer to this situation: A macroscopic box is divided into t

Question

Questions 1) and 2) refer to this situation: A macroscopic box is divided into two halves by a partition. Each half contains N gas molecules at the same pressure and temperature. Consider what happens to the entropy when the partition is removed 1) If the two halves contain the same gas (e.g., both are oxygen), the entropy will: O decrease significantly O remain almost the same (i.e., a reversible process) O increase significantly Submit 2) If the two halves contain different gases (e.g., oxygen and nitrogen), the entropy wil O decrease significantly. O remain almost the same (i.e., a reversible process) increase significantly. Submit 3) Part 1) is an example of entropy change caused by removal of a constraint (the partition). Now consider the entropy change during quasistatic processes, ones in which V, p, and T change very slowly and are always well defined. Start with 1 liter of argon (an ideal, monatomic gas) at pressure, p 100 kPa, and temperature, T 280 K. Calculate the entropy change AS if we were to let the gas expand to 2 liters (keeping the temperature constant) AS J/K Submit Help 4) Start with 0.09 moles of argon (an ideal, monatomic gas) at pressure, p = 105 kPa, and temperature, T-300 K. Calculate the entropy change AS if we were to add 155 J of heat to the gas (keeping the volume constant). J/K Submit Help

Explanation / Answer

Answer 1

Entropy will remain same due to reversible process

Answer 2

Entropy will increase significantly

As per chegg policy i had done 1st question

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