Chemistry
Chemistry
Problem
Liquid neon is commonly transported in dewars and then allowed to vaporize for use as a cryogenic refrigerant. Suppose 1.75 g of liquid neon completely vaporizes and the gas is collected in a 1.25 L rigid container at 2.50 atm. The ambient laboratory temperature is 23.0 °C. (a) Convert all given quantities to the units required for a consistent single calculation and state those converted values. (b) Calculate the volume the neon gas would occupy at the same temperature if its pressure were adjusted to exactly 1.00 atm, keeping the amount of gas constant. (c) Many cryogenic facilities instead report volumes in cubic meters (m). Convert your answer in part (b) to cubic meters using appropriate significant figures.Intuitive explanation
The key here is recognizing that you have all the information needed to find the actual temperature of the neon gas using the ideal gas law—which won't be room temperature, since the problem tells you the pressure and volume of the vaporized gas. Once you calculate the real temperature, you can compare it to the ambient temperature to understand the thermal state of your cryogenic system. This is a straightforward application of where you solve for after finding the number of moles from the mass of neon.
Intuitive explanation
The key here is recognizing that you have all the information needed to find the actual temperature of the neon gas using the ideal gas law—which won't be room temperature, since the problem tells you the pressure and volume of the vaporized gas. Once you calculate the real temperature, you can compare it to the ambient temperature to understand the thermal state of your cryogenic system. This is a straightforward application of where you solve for after finding the number of moles from the mass of neon.