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A monoatomic ideal gas is taken through the cycle A → B → C → A shown in the figure.
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If we know that the internal energy of the monoatomic ideal gas remains constant during the process B → C, what must be the pressure pC at point C in terms of the original pressure p0? Express the work WBC done by the gas during the process B → C in terms of p0 and V0. |
| Express the heat QBC flowing into the gas during the process B → C in terms of p0 and V0. |
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- In the process illustrated by the pV diagram in the image, the temperature of the ideal gas remains constant at 136 ∘C . Part A: How many moles of gas are involved? Part B: What volume does this gas occupy at a? (express in cubic meters) Part C: How much work was done by or on the gas from a to b? and by how much did the internal energy of the gas change during this process?Please help meConsider the following two-step process. Heat is allowed to flow out of an ideal gas at constant volume so that its pressure drops from P₁ = 2.7 atm to P2 = 1.7 atm. Then the gas expands at constant pressure, from a volume of V₁ = 5.9 L to V₂ = 9.6 L, where the temperature reaches its original value. See the figure ( Figure 1). Figure P P₁ P2 σ P D HÅ AU = Value Units Submit Request Answer Part C 1 of 1 wwwww ? Calculate the total heat flow into or out of the gas. Express your answer to two significant figures and include the appropriate units. ☐ με Value Units Submit Request Answer
- An sulated container holds 100g of water at 30C. A 50g ice cube at 0C is dropped into the water and no heat is allowed to enter or leave the ice water container. What is the final termperature and thermodynamic state of the system after it comes to equilibrium. Hello. This is a practice problem I'm working on and I'm not sure if I'm aproaching the problem correctly. Thank you for the help.Calculate the change in the internal energy of the gas. USE IMAGE AS REFERNCELook at the P-V diagram below (Diagram 1). Calculate the work done by the gas for the paths A, B and C. Assume that in Diagram 1, P1 = 1 atm, P2 = 4 atm, V1 = 5 L, V2 = 15 L. a) WA = 1013 J, WB = 0, WC = -2533 J b) WA = 0.01 J, WB = 0, WC = -0.025 J c) WA = 2533 J, WB = 0, WC = -1013 J Calculate the work done by the gas for the path AB in Diagram 2. Use the data: P1 = 1 atm, P2 = 4 atm, V1 = 5 L, V2 = 20 L. (Path AB is an "isothermal" which means the temperature T is constant on this path). a) 0.012 J b) 1220 J c) 0.0278 J d) 2809 J
- In the figure below, the change in internal energy of a gas that is taken from A to C along the blue path is +900 J. The work done on the gas along the red path ABC is -570 J. (b) If the pressure at point A is five times that of point C, what is the work done on the system in going from C to D?In the figure below, the change in internal energy of a gas that is taken from A to C along the blue path is +870 J. The work done on the gas along the red path ABC is -520 J. (a) How much energy must be added to the system by heat as it goes from A through B to C? (b) If the pressure at point A is five times that of point C, what is the work done on the system in going from C to D? (c) What is the energy exchanged with the surroundings by heat as the gas goes from C to A along the green path? (d) If the change in internal energy in going from point D to point A is +555 J, how much energy must be added to the system by heat as it goes from point C to point D?A particular thermodynamic cycle acting on a monatomic ideal gas (y = 1.67) includes an isobaric expansion, an isochoric cooling, and then a isothermic contraction. The PV diagram is shown in the image below. P V The isobaric expansion occurs at a pressure of 2.265 × 105 Pa and changes the volume of the gas from 5.9 × 10 2 m³ to 10.98 × 10-2 m³. What is the efficiency of the process?
- You would like to raise the temperature of an ideal gas from 295 K to 960 K in an adiabatic process. a)What compression ratio will do the job for a monatomic gas? b)What compression ratio will do the job for a diatomic gas?Part A: If you supply 2950 J of heat to 6.00 moles of an ideal diatomic gas initially at 23.0 ∘C in a perfectly rigid container, what will be the final temperature of the gas? Express in degrees Celsius. Part B: Suppose the gas in the container were an ideal monatomic gas instead. How much heat would you need to add to produce the same temperature change? Part C: Which pV diagram expresses these processes?