One mole of an ideal monoatomic gas at 27°C is subjected to a reversible isoentropic compression until the final temperature reached 327°C. If the initial pressure was 1 atm then, find the value of final pressure.
Correct answer: A. 0.75 atm
- A. 0.75 atm
- B. 2 atm
- C. 2.5 atm
- D. 0.5 atm
Explanation
In an adiabatic process for an ideal monoatomic gas, the relationship between pressure and temperature is given by the equation: P1/T1^(γ/(γ-1)) = P2/T2^(γ/(γ-1)), where γ (gamma) is the heat capacity ratio (Cp/Cv) and is 5/3 for a monoatomic gas. Given the initial temperature (T1 = 27°C = 300K) and final temperature (T2 = 327°C = 600K), and knowing that the initial pressure (P1) is 1 atm, solving for P2 gives us 0.75 atm. The other options do not satisfy this relationship based on the given temperatures and initial conditions.
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Thermochemistry measures energy changes in chemical reactions and distinguishes exothermic from endothermic processes. Work covers systems, surroundings and state functions, internal energy, the first law of thermodynamics, enthalpy and Hess's law, including the sign conventions used when heat enters or leaves a system.
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