College Physics
11th Edition
ISBN: 9781305952300
Author: Raymond A. Serway, Chris Vuille
Publisher: Cengage Learning
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- 6. A heat engine consists of the cycle p shown for 3 moles of an ideal 2p monatomic gas. It starts at point 1 with pressure p and volume V; it goes via an isochoric (constant 1 volume) process from point 1 to 3 point 2 until the pressure doubles; it then goes from point 2 to point 3 via an adiabatic process; finally it goes V from point 3 to point 1 via an isothermal process. А. I What is the volume of the gas at point 3? Express your answer in terms of V (the volume of the gas at point 1). В. What are W12, W23, and W31? Express your answer in terms of p, V. 2.arrow_forwardIn a refrigerator, 2.10 mol of an ideal monatomic gas is taken through the cycle shown in the figure. The temperature at point A is 782.0 K What is the temperature at point D? Karrow_forwardTi An ideal gas is taken through three different isothermal processes. The sketch represents the Pressure vs Volume graph of these processes. Which of the following is true of the temperatures of these three processes? (Assume number of moles stays the same in all three processes) O T1 > T2 > T3 O T1 > T2 = T3 O T3 > T2 >T1 O T1 > T2 < T3arrow_forward
- Consider a process that uses n moles of a monatomic ideal gas operating through a Carnot cycle. The initial temperature and pressure of the gas are T1 and P1, respectively. Consider steps 1 → 2, 2 → 3, 3 → 4, and 4 → 1. In the adiabatic heating, the temperature of the gas is doubled. Write an expression for the volume V3 after this step in terms of V1. Write an expression for P3 in terms of n, R, T3 and V3.arrow_forwardP Example of calculation of work P = 1 Atm V%= 1 litre iii ii P V V,12 V In this cycle the system, which is an ideal monatomic gas, undergoes first isothermal (i) then adiabatic (ii) compression steps, each of which halve the volume, then returns to its starting point via first isothermal (iii) and then adiabatic (iv) expansions, each of which double the volume. How much work is done by the system during the cycle if P, is 1 atmosphere and V, =1 litre?arrow_forwardThe difference AS=S,- S,between the entropies of two states A and B of a system can be calculated as the integral fdQ/T, counting that: B a. A and B are in the same adiabatic b. A and B are at the same temperature c. The integral is calculated over a reversible path d.The system is thermally insulated e. Friction in the process is disregardedarrow_forward
- A certain gasoline engine is modeled as a monatomic ideal gas undergoing an Otto cycle, represented by the p-V diagram shown in the figure. The initial pressure, volume, and temperature are p1 = 1.05 × 105 Pa, V1 = 0.035 m3, and T1 = 290 K, respectively. a)The first step in the Otto cycle is adiabatic compression. Enter an expression for the work performed on the gas during the first step, in terms of V1, V2, and p1. b) Calculate the temperature of the gas, in kelvins, at the end of the first step. c)The fourth and last step in the Otto cycle is isochoric cooling to the initial conditions. Find the amount of heat, in joules, that is discharged by the gas during the fourth step.arrow_forwardView Policies Current Attempt in Progress Air is compressed in a piston-cylinder assembly from p₁ = 25 lbf/in², T₁ = 500°R, V₁ = 9 ft³ to a final volume of V₂ = 1 ft3 in a process described by pv¹.25 = constant. Assume ideal gas behavior and neglect kinetic and potential energy effects. Using constant specific heats evaluated at T₁, determine the work and the heat transfer, in Btu.arrow_forwardAn 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.0arrow_forward
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