A gas contained in a cylinder fitted with a frictionless piston expands against a constant external pressure of 1 atm from a volume of 5L to a volume of 10L. In doing so, it absorbs 400 J of thermal energy from its surroundings. Determine the change in the internal energy of the system.

A cylinder contains 5.0 moles of a monatomic ideal gas at a pressure 2.0x105 Pa. The gas is then compressed at constant pressure from an initial volume of 0.090 m³ to 0.040 m. 5. a) b) c) What is the work done by the gas? What is the change in the internal energy of the gas? How much heat energy flows into the gas during this process? (-1.0x10* J] (-1.5x10* J] (-2.5x10' J]

A cylinder of volume 0.300 m3 contains 10.0 mol of neon gas at 20.0°C. Assume neon behaves as an ideal gas. (a) What is the pressure of the gas? (b) Find the internal energy of the gas. (c) Suppose the gas expands at constant pressure to a volume of 1.000 m3. How much work is done on the gas? (d) What is the temperature of the gas at the new volume? (e) Find the internal energy of the gas when its volume is 1.000 m3. (f) Compute the change in the internal energy during the expansion. (g) Compute ΔU - W. (h) Must thermal energy be transferred to the gas during the constant pressure expansion or be taken away? (i) Compute Q, the thermal energy transfer. (j) What symbolic relationship between Q, ΔU, and W is suggested by the values obtained?

An ideal gas initially at 350 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 11.2 kJ is transferred to the gas by heat. (a) What is the change in internal energy of the gas? kJ (b) What is the final temperature of the gas?