Since for isothermal process,
PV=nRT for n moles of gas
T is same throughout isothermal process
so
so work done during isothermal expansion
A gas undergoes an isothermal expansion form V_1 = 3.7L followed by isobaric p = cst...
12. 1 mole of an ideal gas undergoes an isothermal expansion from V1 = 1.4L followed by isobaric compression, p = cst.if P1 = 4.4atm, p2 = 1.7atm → ?- m calculate the work done by gas during the expansion. Express work in J = N·m! • For isothermal processes, AT = 0 T = cst → w=faw=fr&v=/MRT AV 594 Show your work like: `x-int_0^5 v(t)dt rarr x-int_0^5(-4*t)dt=-50 m 13. 1 mole of an ideal gas undergoes an isothermal expansion...
An ideal gas undergoes the following steps reversibly: I. Isothermal expansion from (P_1, T_1, V_1) to (P_2, T_1, V_2) II. Isochoric change from (P_2, T_1, V_2) to (P_3, T_2, V_2) Determine w, q, Delta U, and Delta H for each step.
Consider an ideal gas having initial pressure and volume p_1, V_1 in terms of p_1, V_1 and gamma, write down an expression for the variation of p with V during (a) isothermal expansion, (b) adiabatic expansion, (c) Show that the slope d p/dV of the path on a p-V diagram is steeper for adiabatic processes than for isothermal processes, given that gamma = C_p/C_v> I.
1.00 mile of a monoatomic ideal gas at 298 K undergoes isothermal expansion from an initial pressure of 12.0 bar to 5.00 bar. Calculate the work if the expansion is done a) against a constant external pressure b) reversibly and isothermally. Problem 3 1.00 mole of a monoatomic ideal gas at 298 K undergoes isothermal expansion from an initial pressure of 12.0 bar to 5.00 bar. Calculate the work if the expansion is done (a) against a constant external pressure...
An ideal gas (1.82 moles) undergoes the following reversible Carnot cycle. (1) An isothermal expansion at Thot=850K from 3.20L to 20.40L. (2) An adiabatic expansion until the temperature falls to 298K. The system then undergoes (3) an isothermal compression and a subsequent (4) adiabatic compression until the initial state is reached. a. Calculate work and ΔS for each step in the cycle and its overall efficiency. b. Determine ΔH and ΔU for steps (1) and (2). c. Explain why ΔUcycle=...
A 3-mole of a monatomic ideal gas undergoes an isothermal expansion at 450 K, as the volume increased from 0.010 m3 to 0.060 m3. What is the work done by the gas and the change in the internal energy of the gas respectively during this process? (R = 8.31 J/mol · K) 15.1 kJ, 3.6 kJ 20.1 kJ, O.O kJ 20.1 kJ, 18.5 kJ -17.2 kJ, 20.1 kJ -20.1 kJ, O kJ
an ideal gas undergoes irreversible isothermal expansion. which is correct? The answer is A. Please explain why. An ideal gas undergoes irreversible isothermal expansion. Which is correct? 2.
The work done by the gas is negative for an A)constant volume process B)adiabatic expansion C)isothermal expansion D)isothermal compression
A monatomic ideal gas undergoes isothermal expansion from 0.08 m3 to 0.22 m3 at a constant temperature (initial pressure is 310 kPa). What are its (a) internal energy change (ΔEΔE), (b) net heat transfer (Q), and (c) net work done (W)? Use negative quantity for heat transfer out of the system or work done on the system.
PLEASE I NEED A DETAILED EXPLANATION TO THIS SOLUTION (e) Oxygen gas undergoes isobaric expansion due to heating. The energy transfer by heating, for the gas, is Q-+4 x 105 J. Find the energy transfer by working, for the gas (Hints: from initial volume Vo to final volume 'jat constant P: P V PVİ-Plg. Also, you do not need to know n or P)