In an ideal gas law experiment, how is the temperature of the hydrogen gas typically determined?

If 10 L of O_2 at 273 K and 1 atm is compressed to a 7 L container at 250 K, what will be the final pressure of the gas (in atm), assuming ideal gas behavior?

At what temperature (in K) would 2.10 moles of N_2 gas exert a pressure of 1.25 atm in a 25.0 L tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

What is the volume occupied by 51.0 g of ammonia (NH_3) gas at standard temperature and pressure (STP)?

A 5.00 L tank contains 10.00 grams of oxygen gas (O_2) at a temperature of 350 K. What is the pressure in the tank in atmospheres (atm)? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

A 6.00 L tank contains 20.0 grams of nitrogen gas (N_2) at a temperature of 385 K. What is the pressure inside the tank? (Use R = 0.0821 L·atm·mol^{-1}·K^{-1})

A sample of nitrogen gas occupies 2.50 L at 300 K and 1.00 atm. If the gas is completely vaporized from liquid nitrogen at its boiling point (77 K), and the pressure remains constant, which of the following equations would you use to determine the heat of vaporization (ΔH_vap) of nitrogen using the Ideal Gas Law and the given data?

A gas expands from state i to state f in the figure, with the pressure remaining constant. Which equation best describes the relationship between the initial and final volumes and temperatures according to the ideal gas law?

Which equation correctly relates the molar mass (M), density (d), pressure (P), and temperature (T) of an ideal gas using the ideal gas law?