Helium gas with a volume of 2.60 L, under a pressure of 0.180 atm and at a temperature of 41.0^∘

step 1 In Problem 2, Chapter 18, the given volume of the helium gas is 2 .6 liters, and its pressure is

Helium gas with a volume of 2.60 L, under a pressure of...

Helium gas with a volume of $2.60 \mathrm{L},$ under a pressure of 0.180 atm and at a temperature of $41.0^{\circ} \mathrm{C},$ is warmed until both pressure and volume are doubled. (a) What is the final temperature? (b) How many grams of helium are there? The molar mass of helium is 4.00 $\mathrm{g} / \mathrm{mol} .$

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Key Concepts

Molar Mass and Stoichiometry

Molar mass is a key concept in stoichiometry that connects the mass of a substance to the number of moles. By using the molar mass, you can convert between grams and moles, allowing you to determine the amount of a substance present, which is critical when working with the ideal gas law to relate mass to the number of molecules involved.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates a gas's pressure (P), volume (V), temperature (T), and the number of moles (n) through the gas constant (R). This law allows you to predict how changes in any one of these parameters will affect the others, which is essential when considering scenarios where temperature, pressure, or volume are altered.

Temperature Conversion to Kelvin

When solving gas law problems, temperature must be expressed in Kelvin, not Celsius. The Kelvin scale is the SI unit for temperature because it starts at absolute zero—the point where molecular motion stops—making it necessary for accurately applying the ideal gas law.

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