What is the specific heat of oxygen (O₂; M = 32.00 g/mol) at constant volume? How does it compare with specific heat for liquid water? Hint: C_v = 20.85 J/mol•K.

Calculate the heat absorbed by 1.4 moles of an ideal diatomic gas to increase its temperature by 38 K if it is placed in a constant volume container. Assume the process occurs at temperatures near room temperature.

A 0.32 mol gas sample has its thermal energy as a function of temperature plotted as shown below. Find the heat capacity of the gas at constant volume.

A mysterious diatomic gas has a strong covalent bond that requires high temperatures to experience vibrational modes. The vibration modes are experienced at temperatures greater than or equal to 1000 K. Suppose the gas enters a combustion chamber of an Otto cycle engine that reaches ignition temperatures of 2400 K; find the theoretical ratio of specific heats of the mysterious gas at 2400 K.

A refrigerator takes out 2.5 J of heat energy from a 4.0 mol of an element. Calculate the decrease in temperature of the element if it is (i) Neon, (ii) Oxygen, (iii) A solid element

3.2 g of neon at T = 20℃ comes into contact (through a conducting boundary) with 4.2 g of nitrogen at  T =  320℃. Calculate the amount of heat that flows between the gases to establish thermal equilibrium and state the direction of flow.

2.50 g of nitrogen moves at an rms speed of 1150 m/s. The gas expands, doing 925 J of work to the surroundings, and absorbs 650. J of heat from the surrounding. Calculate the rms speed of the nitrogen molecules after this process.