Taking into account the ideal gas law, at 654.81 K 16.3 g of nitrogen gas have a pressure of 1.25 atm in a 25.0 L tank.
Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.
An ideal gas is characterized by three state variables: absolute pressure (P), volume (V), and absolute temperature (T). The relationship between them constitutes the ideal gas law, an equation that relates the three variables if the amount of substance, number of moles n, remains constant and where R is the molar constant of the gases:
P× V = n× R× T
Now, taking into account this law, and isolating the temperature variable (T), you get:
[tex]T=\frac{PxV}{nxR}[/tex]
In this case, you know:
- P= 1.25 atm
- V= 25 L
- n= [tex]16.3 gramsx\frac{1 mole}{28 grams}[/tex]= 0.582 moles where 28 g/mole is the molar mass of the N₂ gas, that is, the amount of mass that a substance contains in one mole.
- R=0.082 [tex]\frac{atmL}{molK}[/tex]
Replacing:
[tex]T=\frac{1.25 atmx25 L}{0.582 molesx0.082\frac{atmL}{molK} }[/tex]
Solving:
T= 654.81 K
In summary, at 654.81 K 16.3 g of nitrogen gas have a pressure of 1.25 atm in a 25.0 L tank.
Learn more:
https://brainly.com/question/4147359?referrer=searchResults
