Consider a metal cylinder containing 160 grams of oxygen gas with a molar mass of 16 g/mol in a room at 25.0 degrees Celsius. The cylinder is moved and kept outside the room on a hot summer day. The oxygen gas in the cylinder comes into equilibrium with the surrounding temperature, as 600 J of heat is conducted through the cylinder walls. Ignoring the expansion of the metal cylinder, determine the equilibrium temperature. To solve the problem, first, identify the known and unknown quantities. Next, the number of moles can be determined by dividing the mass of the gas by its molar mass. Recall the molar heat capacity equation at constant volume. Oxygen is a diatomic gas; by substituting the degree of freedom, the equation of molar heat capacity for an ideal diatomic gas at a constant volume can be obtained. Lastly, by rearranging the equation and substituting the values, the temperature change is determined to be 2.88 degrees Celsius, and the equilibrium temperature to be 27.88 degrees Celsius.