A gas is enclosed in a cylinder fitted with a light frictionless piston and maintained at atmospheric pressure. When 254 kcal of heat is added to the gas, the volume is observed to increase slowly from 12.0 m3 to 16.2 m3 . Calculate the work done by the gas.Calculate the change in internal energy of the gas.

For an ideal gas in an isothermal process, there is no change in internal energy. Suppose the gas does work W during such a process. How much energy is transferred by heat?

A cylinder of volume 0.320 m3 contains 10.5 mol of neon gas at 17.4°C. Assume neon behaves as an ideal gas. (a) What is the pressure of the gas? Pa(b) Find the internal energy of the gas. J(c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas? J(d) What is the temperature of the gas at the new volume? K(e) Find the internal energy of the gas when its volume is 1.000 m3. J(f) Compute the change in the internal energy during the expansion. J(g) Compute ΔU − W. J(h) Must thermal energy be transferred to the gas during the constant pressure expansion or be taken away? This answer has not been graded yet. (i) Compute Q, the thermal energy transfer. J(j) What symbolic relationship between Q, ΔU, and W is suggested by the values obtained?

The gas cycled as shown. Calculate the heat supplied to the gas during the process C-A when QA-B = 20.0 J is the heat supplied during the process A-B, the process B-C is adiabatic and the total work done by the gas done during the cycle is 15.0 J?

The work done by 6.02 x 1023 molecules of a monatomic ideal gas (γ = 1.4) in expanding adiabatically is 825 J. The initial temperature and volume of the gas are 393 oC and 100 cm3. Obtain a) the final internal energy of the gas. b) final volume of the gas.

A monatomic ideal gas initially fills a V0 = 0.45 m3 container at P0 = 85 kPa. The gas undergoes an isobaric expansion to V1 = 1.4 m3. Next it undergoes an isovolumetric cooling to its initial temperature T0. Finally it undergoes an isothermal compression to its initial pressure and volume.   1 Calculate the work done by the gas, W1, in kilojoules, during the isobaric expansion (first process).  2 Calculate the heat absorbed Q1, in kilojoules, during the isobaric expansion (first process).  3 Write an expression for the change in internal energy, ΔU1 during the isobaric expansion (first process).  4 Calculate the work done by the gas, W2, in kilojoules, during the isovolumetric cooling (second process).  5 Calculate the heat absorbed Q2, in kilojoules, during the isovolumetric cooling (second process).   6 Calculate the change in internal energy by the gas, ΔU2, in kilojoules, during the isovolumetric cooling (second process).  7 Calculate the work done by the gas, W3, in kilojoules,…

As shown below, a nonideal gas goes through the cycle ABCA. During the process AB, 71.5 J of heat was added to the gas. During the process BC, 8.2 J of heat was removed from the gas. Determine WABCA & QCA. WABCA = QCA P(N/m²) 10 2 2 A 4 6 8 B с 10 V (m³)

When an ideal gas undergoes a quasistatic adiabatic volume change, its pressure p and volume V are related by PVY = a constant, where y is the ratio of the molar specific heats for the gas. Start from the first law of thermodynamics, present a proof of this equation.

A sample of ideal gas in a thermally insulated container with a movable piston is initially in state A.  The gas is taken from state A to state B by an adiabatic process.  The dashed lines represent isotherms.  If W is the work done on the gas, Q is the energy transferred to the gas by heating, and  Delta U be the change in the internal energy of the gas during the process. a) is W greater than zero, zero, or less than zero? Explain briefly  b) is Q greater than zero, zero, or less than zero? Explain briefly. c) is  Delta U  greater than zero, zero, or less than zero? Explain briefly.

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?