Answer:
1.22 mol
Explanation:
Pre-Solving
We are given that a 5.86 L cylinder has a pressure of 6.27 atm at 368 K. We want to know how many moles of gas are present at these conditions.
We can use the ideal gas law in order to solve this question; recall that the ideal gas law is PV = nRT, where P is pressure in atm, V is volume in L, n is amount in moles, R is a constant ([tex]0.0821 \frac{atmL}{molK}[/tex]), and T is temperature in K.
Solving
Since we are given all other variables in the correct units, we can substitute what we know into the equation:
[tex]5.86 L * 6.27 atm = n * 0.0821 \frac{atmL}{molK} * 368 K[/tex]
Divide both sides by [tex]0.0821 \frac{atmL}{molK} * 368 K[/tex]
[tex]n = \frac{5.86 L * 6.27 atm}{0.0821 \frac{atmL}{molK} * 368 K } = 1.22 mol[/tex] (rounded to three sig figs)
