During the compression stroke of a certain gasoline engine, the pressure increases from 1.00 atm to 20.0 atm. If the process is adiabatic and the air–fuel mixture behaves as a diatomic ideal gas, (a) by what factor does the volume change and (b) by what factor does the temperature change? Assuming the compression starts with 0.016 0 mol of gas at 27.0°C, find the values of (c) Q, (d) ΔEint, and (e) W that characterize the process.

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 diatomic ideal gas contracts at constant pressure of 159 kPa from 2.7 m³ to 1.7 m³. Calculate the change in the internal energy in kJ during the process.

Air (a diatomic ideal gas) at 25.0°C and atmospheric pressure is drawn into a bicycle pump (see figure below) that has a cylinder with an inner diameter of 2.50 cm and length 53.5 cm. The downstroke adiabatically compresses the air, which reaches a gauge pressure of 8.00 x 10° Pa before entering the tire. We wish to investigate the temperature increase of the pump.

An ideal gas undergoes the thermodynamic process shown in the ??PV diagram in the figure. Determine whether each of the values (a) Δ?ΔU, (b) ?W, (c) ?Q for the gas is positive, negative, or zero. (Note that ?W is the work done ??on the gas.) Hint: First use the ideal gas law to find the initial and final temperatures in terms of ?0P0 and ?0V0 and determine if the final temperature is greater than, less than, or equal to the initial temperature.   (a) ΔU A.+ B.- C.0   (b) W A.+ B.- C.0   (c) Q A.+ B.- C.0

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.

One mole of an ideal gas, for which CV,m = 3/2R, initially at 298 K and 1.00 × 10^5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 1.00 × 10^6 Pa. Calculate the final temperature of the gas. Calculate q, w, ΔU, and ΔH for this process.

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