The temperature of 1.89 mol of a monatomic ideal gas is 376 K. The internal energy of this gas is doubled by the addition of heat. How much heat is needed when it is added at (a) constant volume and (b) constant pressure? (a) number              units (b) number                 units

An ideal gas initially at 340 K undergoes an isobaric expansion at 2.50 kPa. The volume increases from 1.00 m3 to 3.00 m3 and 12.6 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

A helium-filled toy balloon has a gauge pressure of 0.400 atm and a volume of 11.0 liters. How much greater is the internal energy (in J) of the helium in the balloon than it would be at zero gauge pressure?

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?

Three moles of a monatomic ideal gas are heated at a constant volume of 2.01 m³. The amount of heat added is 5.40 x 103 J. (a) What is the change in the temperature of the gas? (b) Find the change in its internal energy. (c) Determine the change in pressure. (a) Number i (b) Number i (c) Number i Units Units Units

A container having a volume of 2.30 L holds 1.80 g of helium gas at a temperature of 29.0 °C. (a) Find the pressure in the container. P = atm (b) Helium behaves as an ideal monoatomic gas. Find the internal energy of the system. Eint =

Under constant-volume conditions, 2800 J of heat is added to 1.6 moles of an ideal gas. As a result, the temperature of the gas increases by 140 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.

A sealed ideal gas system contains 2.0 moles of monatomic ideal gas, initially at temperature 300 K and pressure 1.2 atm. The system is allowed to expand isothermally to five times its original volume. How much heat is transferred into the system during this process? 7.09 kJ 11.2 kJ 8.03 kJ Zero 4.97 kJ