You are testing some novel fuel mixtures for potential use in automobiles. Your testing apparatus is a 2.54cm inner diameter cylinder fitted with a piston, designed to mimic a cylinder found in a car engine. A fuel/air mixture is ignited while a force of 256.0 N is applied to the piston. If there are 0.160 mol of gas after combustion at 260.0°C, and the atmospheric pressure is 1.01325 × 105 Pa, what is the pressure of gas inside the cylinder at these initial conditions? Assume the combustion products behave ideally. What is the volume of gas in the cylinder? The force applied to the piston is then reduced to 126.0 N and the gas responds in a two step process. The first, quick step is adiabatic. During the second, slower step, the gas returns to 260.0°C from heat provided by the cylinder walls. Assume that the change in kinetic and potential energies in both steps is negligible. Consider the energy balance equation for a closed system: where ΔU is the change in internal energy, ΔEk is the change in kinetic energy, ΔEp is the change in potential energy, Q is heat and W is work. For the first step of the two step process, sort the terms in the energy balance equation based on if they are zero or non-zero. For the second step of the process, sort the terms in the energy balance equation based on if they are zero or non-zero. For the overall process, sort the terms in the energy balance equation based on if they are zero or non-zero. What is the final pressure of the gas? What is the final volume of the gas? How much heat was added to the gas in this process?
The question belongs to Chemical Engineering and it discusses about calculation of volume of gas in cylinder, pressure of gas in cylinder and heat added to the gas in the process.
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