Isochoric Process
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In an isochoric process with heat addition:
 Explanation: Heat addition increases internal energy (ΔU = Q) as no work is done. Temperature rises, but volume remains constant.
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Isochoric processes are significant in:
 Explanation: Bomb calorimeters use constant-volume conditions to measure heat of reactions. Turbines, nozzles, and heat exchangers involve flow or other processes.
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In an isochoric process, enthalpy change is:
 Explanation: Enthalpy change (ΔH = m·cp·ΔT) depends on temperature change and cp. It’s not zero, work-related, or inherently negative.
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For an ideal gas in an isochoric process, pressure and temperature are related by:
Explanation: From the ideal gas law (PV = nRT) at constant volume, P/T = nR/V = constant. Other relations apply to isothermal or adiabatic processes.
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An isochoric process is typically modeled in:
Explanation: Rigid containers maintain constant volume, ideal for isochoric processes. Piston-cylinders allow volume changes; pipes and turbines involve flow.
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In an isochoric process for an ideal gas:
 Explanation: Internal energy of ideal gases depends on temperature, which changes with heat addition. Volume is fixed, and pressure or temperature may vary.
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Specific heat at constant volume (cv) is used in:
 Explanation: cv governs heat addition in constant-volume processes (Q = m·cv·ΔT). cp is used for isobaric; other processes have different heat relations.
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For an ideal gas in an isochoric process, heat added equals:
 Explanation: With W = 0, the First Law (ΔU = Q – W) gives Q = ΔU. All heat increases internal energy, not work or enthalpy.
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In an isochoric process, work done is:
 Explanation: No volume change (ΔV = 0) means no PV work (W = PΔV = 0). Heat transfer drives internal energy changes instead.
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An isochoric process occurs at:
 Explanation: Isochoric processes maintain constant volume, with heat affecting internal energy. Pressure, temperature, or enthalpy may change, unlike isobaric or isothermal processes.
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