During a reversible adiabatic expansion of an ideal gas, which of the following is not true? (a) PV = constant, (b) PV = nRT, (c) TV-1 = constant, (d) W = f Pdv (W is the magnitude of the work done by the gas) (e) PV = constant.
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- A sample of an ideal gas is expanded to twice its original volume of 1.00 m³ in a quasi-static process for which P=aV², with α= 4.53 atm/m6, as shown in the P-V plot below. How much work is done on the expanding gas? P Les P=av² 1.00 m³ 2.00 m³Assume that 9.63 moles of a monatomic ideal gas expand adiabatically, lowering the temperature from 388 to 262 K. Calculate (a) the work done by the gas (including the algebraic sign) and (b) the change in the gas's internal energy.A cylinder containing n mol of an ideal gas undergoes an adibatic process. Starting with dW = pdV and using the condition pVY = constant, show that the work done by the gas: 1 W × (p;V; - PfV¢) %3D Starting from the first law of thermodynamics in differential form, prove that the work done by the gas is n×Cy(T; - Tf).
- A monatomic ideal gas expands adiabatically from 1.8 m³ to 4 m³. If the initial pressure is 102 kPa, calculate the energy in kJ transferred to or from the system by heat.An ideal monatomic gas expands adiabatically from 0.530 m³ to 1.72 m³. If the initial pressure and temperature are 1.30 × 105 Pa and 355 K, respectively, find the number of moles in the gas, the final gas pressure, the final gas temperature, and the work done on the gas. HINT (a) the number of moles in the gas (Enter your answer to at least three significant figures.) mol (b) the final gas pressure (Enter your answer in Pa, to at least three significant figures.) Pa (c) the final gas temperature (in K) K (d) the work done on the gas (in J) JSuppose 6.36 moles of a monatomic ideal gas expand adiabatically, and its temperature decreases from 387 to 263 K. Determine (a) the work done (including the algebraic sign) by the gas, and (b) the change in its internal energy.
- The first law of thermodynamics, ΔU = Q - W, when written as Q = W + ΔU, says that the heat into a system can be used to do work and/or increase the internal energy. Therefore, which process requires the most heat? Isobaric, isochoric, or adiabatic?Which one of the following statements is true about a sealed ideal gas system? You can increase the internal energy of the system without increasing its temperature. To raise the temperature of the system, you must add heat. No work occurs during a constant-pressure process. In an adiabatic process, no energy leaves or enters the system. In an isothermal process, the internal energy of the system remains the same.An ideal monatomic gas expands isothermally from 0.570 m³ to 1.25 m³ at a constant temperature of 800 K. If the initial pressure is 1.18 x 105 Pa find the following. (a) the work done on the gas (b) the thermal energy transfer Q J (c) the change in the internal energy J