A cylinder with a piston holds 3.00 moles of a diatomic gas. The gas in the cylinder absorbs 875 J of energy due to the higher temperature of the environment. At the same time, the cylinder expands to a larger volume, doing 137 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)?

A chemical reaction transfers 6250 J of thermal energy into 12.0 moles of an ideal gas while the system expands by 2.00 x 10-2 m3 at a constant pressure of 1.25 x 10o5 Pa. HINT (a) To find the change in internal energy, first calculate the work done on the gas and then apply the first law of thermodynamics. (b) For an ideal gas at constant pressure, PAV = NRAT. Click the hint button again to remove this hint. (a) Find the change in the internal energy (in J). (b) Calculate the change in temperature of the gas (in K).

A sample of gas in a cylinder is compressed by a piston at a constant pressure of 0.800 atm. The volume of the cylinder decreases from 6.50 L to 1.00 L, while at the same time 420 J of energy leaves the gas by heat. (a) What is the work done on the gas (in J)? (b) What is the change in its internal energy (in J)?

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 12.0 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? K