A cylinder with a piston holds 4.50 moles of a diatomic gas. The gas in the cylinder absorbs 975 J of energy due to the higher temperature of the environment. At the same time, the cylinder expands to a larger volume, doing 112 J of work on the environment.   (a) What is the change in internal energy of the gas in the cylinder (in J)?   (b) What is the change in temperature of the gas (in K)?

Consider the following figure. (The x axis is marked in increments of 2 m³.) P (Pa) 6 X 106 4 X 106 2 X 106 V (m³) (a) Determine the work done on a gas that expands from i to f as indicated in the figure. MJ Ⓡ (b) How much work is performed on the gas if it is compressed from f to i along the same path? MJ

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?

Suppose a gas absorbs 498 J of energy while doing 147 J of work on its environment. Calculate the change in the internal energy of the gas.

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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?